Anna M. Michałowska-Kaczmarczyk ^{1}, Tadeusz Michałowski ^{2}

^{1}* Department of Oncology, The University Hospital in Cracow, 31-501 Cracow, Poland*

^{2 }*Department of Analytical Chemistry, Technical University of Cracow, 31-155 Cracow, Poland*

© 2018 Sift Desk Journals. All Rights Reserved

VOLUME: 2 ISSUE: 1

Anna M. Michałowska-Kaczmarczyk ^{1}, Tadeusz Michałowski ^{2}

^{1}* Department of Oncology, The University Hospital in Cracow, 31-501 Cracow, Poland*

^{2 }*Department of Analytical Chemistry, Technical University of Cracow, 31-155 Cracow, Poland*

Tadeusz Michalowski, The modified Gran methods in potentiometric redox titrations derived according to GATES/GEB principles(2018)Journal of Chemical Engineering And Bioanalytical Chemistry 2(1)

The paper concerns the modified Gran methods, designed for determination of equivalence volume (V_{eq}) and the slope (J) value of a redox indicator electrode (RIE) applied for potentiometric titrations in redox systems. The methods are exemplified by the titration of (1^{o}) FeSO_{4} and (2^{o}) FeSO_{4} + Fe_{2}(SO_{4})_{3} mixture with KMnO_{4} or Ce(SO_{4})_{2} solution as titrant. The modified Gran methods are based on detailed conclusions resulting from thermodynamic modelling of the related systems according to GATES/GEB principles.

** Keywords**: Redox titration; GATES/GEB; modified Gran methods; electrode calibration.

** Notations and acronyms**: D – titrand (solution titrated); E – voltage [V]; GATES – Generalized approach to electrolytic systems; GEB – Generalized electron balance; LSM – least squares method; T – titrant; V

The original versions of the Gran I [1,2] and Gran II [3,4] methods, denoted later as G(I) and G(II) methods (for brevity), were designed for evaluation of equivalence volume (V_{eq}) in potentiometric titrations, based on transformation of fragments of S-shaped titration curve into linear segments. Both methods, of extrapolative nature (extrapolative standard addition method), especially G(II) method, were widely exploited later in practice by chemists-analysts.

The progress in applications of the G(I) and G(II) methods for analytical purposes was not uniform when referred to the main areas of titrimetric analyses, i.e., acid-base, redox, complexation and precipitation titrations. The methods were devoted mainly to acid-base titration, with special emphasis put on alkalinity. As refers to redox systems, only a few papers of other authors were issued hitherto; all them were based on primitive models resulting from stoichiometry of redox reactions, where only the species entering the redox reaction notation were involved, see e.g. [5]. The functional dependencies based on those assumptions, gave erroneous experimental results for V_{eq}, as were stated in [6-8], and confirmed later in the papers [9-12].

The modified Gran methods, based on the GATES/GEB [13-24] principles, will be illustrated on three examples of potentiometric redox titrations, T(V) ⟹ D(V_{0}). The redox systems considered in this paper will be denoted as follows:

System I : KMnO_{4} (C) + CO_{2} (C_{2}) ⟹ FeSO_{4} (C_{02}) + H_{2}SO_{4} (C_{04}) + CO_{2} (C_{05}) ,

System II : KMnO_{4} (C) + CO_{2} (C_{2}) ⟹ FeSO_{4} (C_{02}) + Fe_{2}(SO_{4})_{3} (C_{03}) + H_{2}SO_{4} (C_{04}) + CO_{2} (C_{05}) ,

System III : Ce(SO_{4})_{2} (C) + H_{2}SO_{4} (C_{1}) + CO_{2} (C_{2}) ⟹ FeSO_{4} (C_{02}) + H_{2}SO_{4} (C_{04}) + CO_{2} (C_{05}) ,

where C, C_{1}, C_{2} and C_{02}, C_{03}, C_{04}, C_{05} are concentrations [mol/L] of the corresponding solutes in T and D, respectively, completed by water. From formal viewpoint, the System I can be considered as a particular case of the System II, at C_{03} = 0. Some similarities inherent in the balances will be applied for further presentation of the balances in a compact form.

The detailed considerations regarding the modified Gran methods will be preceded by formulation of the Generalized Electron Balance (GEB) for the Systems II and III, according to the Approach II to GEB. The algebraic equivalency of Approaches I and II to GEB will also be proved.

**Components and species**

The terms: components of the system and species in the system are distinguished. *After mixing the components *(solvent + solutes)*, a mixture of defined species * *is formed.*

We refer here to aqueous electrolytic systems, where the species exist as hydrates , i=1,…, I; z_{i} = 0, ±1, ±2,…is a charge, expressed in elementary charge units, e = F/N_{A} (F = 96485 C∙mol^{−1}** – **Faraday’s constant, N_{A} = 6.022∙10^{23} mol^{-1} – Avogadro’s number), n_{i} = n_{iW} = n_{i}H_{2}O ≥ 0 is a mean number of water (W=H_{2}O) molecules attached to ; the case n_{iW}=0 is then also admitted.

*For some reasons, it is justifiable to start the balancing from the numbers of particular entities: N _{0j} – for components (j = 1,…,J) represented by molecules, and N_{i} – for the species *

The System II involves the non-redox subsystems:

(II.1) T(V) subsystem, composed of KMnO_{4} (N_{01}) + H_{2}O (N_{02}) + CO_{2} (N_{03}) ;

(II.2) D(V_{0}) subsystem, composed of FeSO_{4}∙7H_{2}O (N_{04}) + Fe_{2}(SO_{4})_{3}·xH_{2}O (N_{05}) + H_{2}SO_{4} (N_{06}) + H_{2}O (N_{07}) + CO_{2} (N_{08}).

For I.2, we have N_{05} = 0 in the D(V_{0}) subsystem.

The System III involves the non-redox subsystems:

(III.1) T(V) subsystem, composed of Ce(SO_{4})_{2}∙4H_{2}O (N_{01}) + H_{2}SO_{4} (N_{02}) + H_{2}O (N_{03}) + CO_{2} (N_{04}) ;

(III.2) D(V_{0}) subsystem, composed of FeSO_{4}∙7H_{2}O (N_{05}) + H_{2}SO_{4} (N_{06}) + H_{2}O (N_{07}) + CO_{2} (N_{08}).

The common list of species, that will be applied/selected to particular Systems (I, II, III), is as follows:

H_{2}O (N_{1}); H^{+1} (N_{2}, n_{2}), OH^{-1} (N_{3}, n_{3}); HSO_{4}^{-1} (N_{4}, n_{4}), SO_{4}^{-2} (N_{5}, n_{5}); H_{2}CO_{3} (N_{6}, n_{6}), HCO_{3}^{-1} (N_{7}, n_{7}),

CO_{3}^{-2} (N_{8}, n_{8}); Fe^{+2} (N_{9}, n_{9}), FeOH^{+1} (N_{10}, n_{10}), FeSO_{4} (N_{11}, n_{11}), Fe^{+3} (N_{12}, n_{12}), FeOH^{+2} (N_{13}, n_{13}),

Fe(OH)_{2}^{+1} (N_{14}, n_{14}), Fe_{2}(OH)_{2}^{+4} (N_{15}, n_{15}); FeSO_{4}^{+1} (N_{16}, n_{16}), Fe(SO_{4})_{2}^{-1} (N_{17}, n_{17}); K^{+1} (N_{18}, n_{18});

MnO_{4}^{-1} (N_{19}, n_{19}), MnO_{4}^{-2} (N_{20}, n_{20}), Mn^{+3} (N_{21}, n_{21}), MnOH^{+2} (N_{22}, n_{22}), Mn^{+2} (N_{23}, n_{23}),

MnOH^{+1} (N_{24}, n_{24}), MnSO_{4} (N_{25}, n_{25}); Ce^{+4} (N_{26}, n_{26}), CeOH^{+3} (N_{27}, n_{27}), Ce_{2}(OH)_{3}^{+5} (N_{28}, n_{28}),

Ce_{2}(OH)_{4}^{+4} (N_{29}, n_{29}), CeSO_{4}^{+2} (N_{30}, n_{30}), Ce(SO_{4})_{2} (N_{31}, n_{31}), Ce(SO_{4})_{3}^{-2} (N_{32}, n_{32}), Ce^{+3} (N_{33}, n_{33}),

CeOH^{+2} (N_{34}, n_{34}), CeSO_{4}^{+1} (N_{35}, n_{35}), Ce(SO_{4})_{2}^{-1} (N_{36}, n_{36}), Ce(SO_{4})_{3}^{-3} (N_{37}, n_{37}).

The species, with the related ordinal numbers, will be applied in the balances, formulated below. Molar concentrations [mol/L] of the species are denoted as , for brevity.

The presence of carbonate species is considered here as an effect of CO_{2} from air, as the admixture of ‘pure’ water used on the step of D and T preparation; it may imitate the real conditions of the analysis, realised according to titrimetric mode.

The T and D can be considered as static (sub)systems of the dynamic D+T system realised in the titration T(V) ⟹ D(V_{0}), where V mL of T is added into V_{0} mL of D, up to a defined point of the titration, and V_{0}+V mL of D+T mixture is obtained at this point, if the additivity of the volumes is valid/tolerable. The D+T mixture is homogenized after each (small) consecutive portion of T added into D, to imitate the titration as the *quasistatic* process realised in a closed system, under isothermal conditions, pre-assumed for modelling purposes.

- Not
**ation of balances**

In aqueous media, we formulate charge balance, *f*_{0} = ChB, and elemental balances: *f*_{1} = *f*(H) for *E*_{1} = H (hydrogen) and *f*_{2} = *f*(O) for *E*_{2} = O (oxygen),… ; other elemental or core balances are denoted as *f*_{k} = *f*(*Y*_{k}), *Y*_{k} = *E*_{k} or *core*_{k} (k=3,…,K). A core is considered as a cluster of different atoms with defined composition (expressed by chemical formula), structure and external charge, unchanged in the system in question; e.g., SO_{4}^{-2} is a core within the set of sulfate species: HSO_{4}^{-1}∙n_{4}H_{2}O, SO_{4}^{-2 }∙n_{5}H_{2}O, FeSO_{4}∙n_{11}H_{2}O in the (I.2) D(V_{0}) subsystem.

In order to formulate the reliable (formally correct) set of balances for a given system, it is necessary to collect detailed, possibly complete (qualitative and quantitative) information regarding this system. The qualitative information concerns the components that make up the given system, and the species formed in this system. This information should subject thorough verification, when regarding the preparation of the appropriate solutions; e.g., Ce(SO_{4})_{2}∙4H_{2}O is dissolved in H_{2}SO_{4} solution, not in water.

To avoid possible/simple mistakes in the realization of the linear combination procedure, w*e apply the equivalent relations:*

for elements with negative oxidation numbers, or

for elements with positive oxidation numbers, k ∈ 3,…,K. In this notation, *f*_{k} will be essentially treated not as the algebraic expression on the left side of the equation *f*_{k} = 0, but as an equation that can be expressed in alternative forms presented above.

4**. Formulation of balances for the System II**

The balances are as follows:

*f*_{0} = ChB

N_{2} – N_{3} – N_{4} – 2N_{5} – N_{7} – 2N_{8} + 2N_{9} + N_{10} + 3N_{12} + 2N_{13} + N_{14} + 4N_{15} + N_{16} – N_{17} + N_{18} – N_{19} – 2N_{20} +

3N_{21} + 2N_{22} + 2N_{23} + N_{24} = 0 (1)

*f*_{1} = *f*(H)

2N_{1} + N_{2}(1+2n_{2}) + N_{3}(1+2n_{3}) + N_{4}(1+2n_{4}) + 2N_{5}n_{5} + N_{6}(2+2n_{6}) + N_{7}(1+2n_{7}) + 2N_{8}n_{8} + 2N_{9}n_{9} +

N_{10}(1+2n_{10}) + 2N_{11}n_{11} + 2N_{12}n_{12} + N_{13}(1+2n_{13}) + N_{14}(2+2n_{14}) + N_{15}(2+2n_{15}) + 2N_{16}n_{16} + 2N_{17}n_{17} +

2N_{18}n_{18} + 2N_{19}n_{19} + 2N_{20}n_{20} + 2N_{21}n_{21} + N_{22}(1+2n_{22}) + 2N_{23}n_{23} + N_{24}(1+2n_{24}) + 2N_{25}n_{25}

= 2N_{02} + 14N_{04} + 2xN_{05} + 2N_{06} + 2N_{07}

*f*_{2} = *f*(O)

N_{1} + N_{2}n_{2} + N_{3}(1+n_{3}) + N_{4}(4+n_{4}) + N_{5}(4+n_{5}) + N_{6}(3+n_{6}) + N_{7}(3+n_{7}) + N_{8}(3+n_{8}) + N_{9}n_{9} +

N_{10}(1+n_{10}) + N_{11}(4+n_{11}) + N_{12}n_{12} + N_{13}(1+n_{13}) + N_{14}(2+n_{14}) + N_{15}(2+n_{15}) + N_{16}(4+n_{16}) + N_{17}(8+n_{17}) +

N_{18}n_{18} + N_{19}(4+n_{19}) + N_{20}(4+n_{20}) + N_{21}n_{21} + N_{22}(1+n_{22}) + N_{23}n_{23} + N_{24}(1+n_{24}) + N_{25}(4+n_{25})

= 4N_{01} + N_{02} + 2N_{03} + 11N_{04} + (12+x)N_{05} + 4N_{06} + N_{07} + 2N_{08}

–*f*_{3} = –*f*(SO_{4})

N_{04} + 3N_{05} + N_{06} = N_{4} + N_{5} + N_{11} + N_{16} + 2N_{17} + N_{25} (2)

–*f*_{4} = –*f*(CO_{3})

N_{03} + N_{08} = N_{6} + N_{7} + N_{8} (3)

–*f*_{5} = –*f*(Fe)

N_{04} + 2N_{05} = N_{9} + N_{10} + N_{11} + N_{12} + N_{13} + N_{14} + 2N_{15} + N_{16} + N_{17} (4)

–*f*_{6} = –*f*(K)

N_{01} = N_{18} (5)

–*f*_{7} = –*f*(Mn)

N_{01} = N_{19} + N_{20} + N_{21} + N_{22} + N_{23} + N_{24} + N_{25} (6)

*f*_{12} = 2∙*f*_{2} – *f*_{1}

–N_{2} + N_{3} + 7N_{4} + 8N_{5} + 4N_{6} + 5N_{7} + 6N_{8} + N_{10} + 8N_{11} + N_{13} + 2N_{14} + 2N_{15} + 8N_{16} + 16N_{17} +

8N_{19} + 8N_{20} + N_{22} + N_{24} + 8N_{25} = 8N_{01} + 4N_{03} + 8N_{04} + 24N_{05} + 6N_{06} + 4N_{08} (7)

2∙*f*_{2} – *f*_{1} + *f*_{0} – 6*f*_{3} – 4*f*_{4} – *f*_{6} = 0 ⟺ (+1)∙*f*_{1} +(–2)∙*f*_{2} + (+6)∙*f*_{3} + (+4)∙*f*_{4} + (+1)∙*f*_{6 }– *f*_{0} = 0 ⟺

(+1)∙*f*(H) + (–2)∙*f*(O) + (+6)∙*f*(SO_{4}) + (+4)∙*f*(CO_{3}) + (+1)∙*f*(K) – ChB = 0 (8)

2(N_{9}+N_{10}+N_{11}) + 3(N_{12}+N_{13}+N_{14}+2N_{15}+N_{16}+N_{17}) + 7N_{19} + 6N_{20} + 3(N_{21}+N_{22}) + 2(N_{23}+N_{24}+N_{25})

= 7N_{01} + 2N_{04} + 6N_{05} (9)

Denoting the atomic numbers: Z_{Fe} = 26, Z_{Mn} = 25, from equations: 4, 6 and 9, we obtain the balance

Z_{Fe}∙*f*_{5} + Z_{Mn}∙*f*_{7} – (2∙*f*_{2} – *f*_{1} + *f*_{0} – 6*f*_{3} – 4*f*_{4} – *f*_{6})

(Z_{Fe}–2)(N_{9}+N_{10}+N_{11}) + (Z_{Fe}–3)(N_{12}+N_{13}+N_{14}+2N_{15}+N_{16}+N_{17}) + (Z_{Mn}–7)N_{19} + (Z_{Mn}–6)N_{20} +

(Z_{Mn}–3)(N_{21}+N_{22}) + (Z_{Mn}–2)(N_{23}+N_{24}+N_{25}) = (Z_{Fe}–2)N_{04} + 2(Z_{Fe}–3)N_{05} + (Z_{Mn}–7)N_{01} (10)

Next, we can apply the combination of equations 4, 6 and 10, giving the shortest form of GEB

3*f*_{5} + 2*f*_{7} – (2*f*_{2} – *f*_{1} + *f*_{0} – 6*f*_{3} – 4*f*_{4} – *f*_{6}) = 0

(N_{9}+N_{10}+N_{11}) – (5N_{19} + 4N_{20} + N_{21}+N_{22}) = N_{04} – 5N_{01} (11)

Applying the relations:

∙(V_{0}+V) = 10^{3}∙ CV = 10^{3}∙N_{01}/N_{A}, C_{2}V = 10^{3}∙N_{03}/N_{A} , C_{02}V_{0} = 10^{3}∙N_{04}/N_{A} , C_{03}V_{0} = 10^{3}∙N_{05}/N_{A} ,

C_{04}V_{0} = 10^{3}∙N_{06}/N_{A} , C_{05}V_{0} = 10^{3}∙N_{08}/N_{A} (12)

in the balances derived above, we have the optional/equivalent equations for GEB. From eq. 7, considered as the *pr*imary form of Generalized Electron Balance (GEB), *f*_{12} = *pr*-GEB, we obtain the equation

– [ H^{+1}] + [OH^{-1}] + 7[HSO_{4}^{-1}] + 8[SO_{4}^{-2}] + 4[H_{2}CO_{3}] + 5[HCO_{3}^{-1}] + 6[CO_{3}^{-2}] + [FeOH^{+1}] +

8[FeSO_{4}] + [FeOH^{+2}] + 2[Fe(OH)_{2}^{+1}] + 2[Fe_{2}(OH)_{2}^{+4}] + 8[FeSO_{4}^{+1}] + 16[Fe(SO_{4})_{2}^{-1}] +

8[MnO_{4}^{-1}] + 8[MnO_{4}^{-2}] + [MnOH^{+2}] + [MnOH^{+1}] + 8[MnSO_{4}]

– (8CV + 4C_{2}V + 8C_{02}V_{0} + 24C_{03}V_{0} + 6C_{04}V_{0} + 4C_{05}V_{0})/(V_{0}+V) = 0 (7a)

Optionally, we have alternative forms of GEB for the System II:

2([Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}]) + 3([Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}] +2[Fe_{2}(OH)_{2}^{+4}]+[FeSO_{4}^{+1}]+

[Fe(SO_{4})_{2}^{-1}]) + 7[MnO_{4}^{-1}] + 6[MnO_{4}^{-2}] + 3([Mn^{+3}]+[MnOH^{+2}])

+ 2([Mn^{+2}]+[MnOH^{+1}]+[MnSO_{4}]) – (2C_{0}V_{0 }+7CV)/(V_{0}+V) = 0 (9a)

(Z_{Fe}–2)([Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}]) + (Z_{Fe}–3)([Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}] + [FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}]) + (Z_{Mn}–7)[MnO_{4}^{-1}] + (Z_{Mn}–6)[MnO_{4}^{-2}] + (Z_{Mn}–3)([Mn^{+3}]+[MnOH^{+2}]) +

(Z_{Mn}–2)([Mn^{+2}]+[MnOH^{+1}]+[MnSO_{4}]) – ((Z_{Fe}–2)C_{0}V_{0} + (Z_{Mn}–7)CV)/(V_{0}+V) = 0 (10a)

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] – (5[MnO_{4}^{-1}] + 4[MnO_{4}^{-2}] + [Mn^{+3}] + [MnOH^{+2}])

– (C_{0}V_{0} – 5CV)/(V_{0}+V) = 0 (11a)

In other words, the GEB can be chosen arbitrarily from the set of equivalent equations: 7a, 9a, 10a, or 11a. The eq. 11a, as one of them, is completed by charge and concentration balances:

[H^{+1}] – [OH^{-1}] – [HSO_{4}^{-1}] – 2[SO_{4}^{-2}] – [HCO_{3}^{-1}] – 2[CO_{3}^{-2}] + 2[Fe^{+2}] + [FeOH^{+1}] + 3[Fe^{+3}] + 2[FeOH^{+2}] + [Fe(OH)_{2}^{+1}]+ 4[Fe_{2}(OH)_{2}^{+4}] + [FeSO_{4}^{+1}] – [Fe(SO_{4})_{2}^{-1}] + [K^{+1}] – [MnO_{4}^{-1}] – 2[MnO_{4}^{-2}]

+ 3[Mn^{+3}] + 2[MnOH^{+2}] + 2[Mn^{+2}] + [MnOH^{+1}] = 0 (1a)

[HSO_{4}^{-1}] + [SO_{4}^{-2}] + [FeSO_{4}] + [FeSO_{4}^{+1}] + 2[Fe(SO_{4})_{2}^{-1}] + [MnSO_{4}] – (C_{02}+3C_{03}+C_{04})V_{0}/(V_{0}+V) = 0 (2a)

[H_{2}CO_{3}] + [HCO_{3}^{-1}] + [CO_{3}^{-2}] – (C_{05}V_{0}+C_{2}V)/(V_{0}+V) = 0 (3a)

[Fe^{+2}] + [FeOH^{+1}] + [FeSO_{4}] + [Fe^{+3}] + [FeOH^{+2}] + [Fe(OH)_{2}^{+1}] + 2[Fe_{2}(OH)_{2}^{+4}]_{} +

[FeSO_{4}^{+1}] + [Fe(SO_{4})_{2}^{-1}] – (C_{02}+2C_{03})V_{0}/(V_{0}+V) = 0 (4a)

[K^{+1}] = CV/(V_{0}+V) (5a)

[MnO_{4}^{-1}] + [MnO_{4}^{-2}] + [Mn^{+3}] + [MnOH^{+2}] + [Mn^{+2}] + [MnOH^{+1}] + [MnSO_{4}] – CV/(V_{0}+V) = 0 (6a)

The relation (5a), where only one species is involved, is considered as equality, not equation.

**Formulation of balances for the System III**

The balances are as follows:

*f*_{0} = ChB

N_{2} – N_{3} – N_{4} – 2N_{5} – N_{7} – 2N_{8} + 2N_{9} + N_{10} + 3N_{12} + 2N_{13} + N_{14} + 4N_{15} + N_{16} – N_{17} + 4N_{18} +

3N_{19} + 5N_{20} + 4N_{21} + 2N_{22} – 2N_{24} + 3N_{25} + 2N_{26} + N_{27} – N_{28} – 3N_{29} = 0 (13)

*f*_{1} = *f*(H)

2N_{1} + N_{2}(1+2n_{2}) + N_{3}(1+2n_{3}) + N_{4}(1+2n_{4}) + 2N_{5}n_{5} + N_{6}(2+2n_{6}) + N_{7}(1+2n_{7}) + 2N_{8}n_{8} + 2N_{9}n_{9} +

N_{10}(1+2n_{10}) + 2N_{11}n_{11} + 2N_{12}n_{12} + N_{13}(1+2n_{13}) + N_{14}(2+2n_{14}) + N_{15}(2+2n_{15}) + 2N_{16}n_{16} + 2N_{17}n_{17} +

2N_{26}n_{26} + N_{27}(1+2n_{27}) + N_{28}(3+2n_{28}) + N_{29}(4+2n_{29}) + 2N_{30}n_{30} + 2N_{31}n_{31} + 2N_{32}n_{32} + 2N_{33}n_{33} +

N_{34}(1+2n_{34}) + 2N_{35}n_{35} + 2N_{36}n_{36} + 2N_{37}n_{37} = 8N_{01} + 2N_{02} + 2N_{03} + 14N_{05} + 2N_{06} + 2N_{07}

*f*_{2} = *f*(O)

N_{1} + N_{2}n_{2} + N_{3}(1+n_{3}) + N_{4}(4+n_{4}) + N_{5}(4+n_{5}) + N_{6}(3+n_{6}) + N_{7}(3+n_{7}) + N_{8}(3+n_{8}) + N_{9}n_{9} + N_{10}(1+n_{10}) +

N_{11}(4+n_{11}) + N_{12}n_{12} + N_{13}(1+n_{13}) + N_{14}(2+n_{14}) + N_{15}(2+n_{15}) + N_{16}(4+n_{16}) + N_{17}(8+n_{17}) + N_{26}n_{26} +

N_{27}(1+n_{27}) + N_{28}(3+n_{28}) + N_{29}(4+n_{29}) + N_{30}(4+n_{30}) + N_{31}(8+n_{31}) + N_{32}(12+n_{32}) + N_{33}n_{33} + N_{34}(1+n_{34}) +

N_{35}(4+n_{35}) + N_{36}(8+n_{36}) + N_{37}(12+n_{37}) = 12N_{01} + 4N_{02} + N_{03} + 2N_{04} + 11N_{05} + 4N_{06} + N_{07} + 2N_{08}

–*f*_{3} = –*f*(SO_{4})

2N_{01} + N_{02} + N_{05} + N_{06} = N_{4} + N_{5} + N_{11} + N_{16} + 2N_{17} + N_{30} + 2N_{31} + 3N_{32} + N_{35} + 2N_{36} + 3N_{37} (14)

–*f*_{4} = –*f*(CO_{3})

N_{04} + N_{08} = N_{6} + N_{7} + N_{8} (15)

–*f*_{5} = –*f*(Fe)

N_{05} = N_{9} + N_{10} + N_{11} + N_{12} + N_{13} + N_{14} + 2N_{15} + N_{16} + N_{17} (16)

–*f*_{6} = –*f*(Ce)

N_{01} = N_{26} + N_{27} + 2N_{28} + 2N_{29} + N_{30} + N_{31} + N_{32} + N_{33} + N_{34} + N_{35} + N_{36} + N_{37} (17)

*f*_{12} = 2∙*f*_{2} – *f*_{1}

–N_{2} + N_{3} + 7N_{4} + 8N_{5} + 4N_{6} + 5N_{7} + 6N_{8} + N_{10} + 8N_{11} + N_{13} + 2N_{14} + 2N_{15} + 8N_{16} + 16N_{17} + N_{27} + 3N_{28} +

4N_{29} + 8N_{30} + 16N_{31} + 24N_{32} + N_{34} + 8N_{35} + 16N_{36} + 24N_{37} = 16N_{01} + 6N_{02} + 4N_{04} + 8N_{05} + 6N_{06} + 4N_{08} (18)

The linear combination

*f*_{12} + *f*_{0} – 6*f*_{3} – 4*f*_{4} = 0 ⟺ (+1)∙*f*_{1} + (–2)∙*f*_{2} + (+6)∙*f*_{3} + (+4)∙*f*_{4} – *f*_{0} = 0 ⟺

(+1)∙*f*(H) + (–2)∙*f*(O) + (+6)∙*f*(SO_{4}) + (+4)∙*f*(CO_{3}) – ChB = 0 (19)

involving K^{*}=4 balances for electron-non-active elements: H, O, S, C (*f*(SO_{4}) = *f*(S), *f*(CO_{3}) = *f*(C)) gives the equation:

2(N_{9}+N_{10}+N_{11}) + 3(N_{12}+N_{13}+N_{14}+2N_{15}+N_{16}+N_{17}) + 4(N_{26}+N_{27}+2N_{28}+2N_{29}+N_{30}+N_{31}+N_{32}) +

3(N_{33}+N_{34}+N_{35}+N_{36}+N_{37}) = 2N_{05} + 4N_{01} (20)

Denoting atomic numbers: Z_{Fe} = 26, Z_{Ce} = 58, from equations: 16, 17 and 20, we obtain the balance

Z_{Fe}∙*f*_{5} + Z_{Ce}∙*f*_{6} – (2∙*f*_{2} – *f*_{1} + *f*_{0} – 6*f*_{3} – 4*f*_{4})

(Z_{Fe}–2)∙(N_{9}+N_{10}+N_{11}) + (Z_{Fe}–3)∙(N_{12}+N_{13}+N_{14}+2N_{15}+N_{16}+N_{17}) + (Z_{Ce}–4)∙(N_{26}+N_{27}+2N_{28}+2N_{29}+N_{30}+N_{31}+N_{32}) + (Z_{Ce}–3)∙(N_{33}+N_{34}+N_{35}+N_{36}+N_{37}) = (Z_{Fe}–2)∙N_{05} + (Z_{Ce}–4)∙N_{01} (21)

Applying the relations:

∙(V_{0}+V) = 10^{3}∙, C_{02}V_{0} = 10^{3}∙N_{01}/N_{A}, and CV = 10^{3}∙N_{05}/N_{A} (22)

in eq. 21, we obtain GEB, written in terms of molar concentrations

(Z_{Fe}–2)([Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}]) + (Z_{Fe}–3)([Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]

+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}]) + (Z_{Ce}–4)([Ce^{+4}]+[CeOH^{+3}]+2[Ce_{2}(OH)_{3}^{+5}] +2[Ce_{2}(OH)_{4}^{+4}]+[CeSO_{4}^{+2}] +[Ce(SO_{4})_{2}]+[Ce(SO_{4})_{3}^{-2}]) + (Z_{Ce}–3)([Ce^{+3}]+[CeOH^{+2}]+[CeSO_{4}^{+1}] +[Ce(SO_{4})_{2}^{-1}]+[Ce(SO_{4})_{3}^{-3}])

– ((Z_{Fe}–2)·C_{02}V_{0} + (Z_{Ce}–4)·CV)/(V_{0}+V) = 0 (21a)

Other linear combinations are also possible. Among others, we obtain the simpler form of GEB

3*f*_{5} + 3*f*_{6} – (*f*_{12} + *f*_{0} – 6*f*_{3} – 4*f*_{4}) = 0

(N_{11}+N_{12}+N_{13}) – (N_{21}+N_{22}+2N_{23}+2N_{24}+N_{25}+N_{26}+N_{27}) = N_{01} – N_{05} ⟹ (23)

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] – ([Ce^{+4}]+[CeOH^{+3}]+2[Ce_{2}(OH)_{3}^{+5}]+2[Ce_{2}(OH)_{4}^{+4}]+

[CeSO_{4}^{+2}]+[Ce(SO_{4})_{2}]+[Ce(SO_{4})_{3}^{-2}]) – (C_{02}V_{0} – CV)/(V_{0}+V) = 0 (23a)

From eq. 18, considered as the *pr*imary form of Generalized Electron Balance (GEB), *f*_{12} = *pr*-GEB, we obtain the equation

– [H^{+1}] + [OH^{-1}] + 7[HSO_{4}^{-1}] + 8[SO_{4}^{-2}] + 4[H_{2}CO_{3}] + 5[HCO_{3}^{-1}] + 6[CO_{3}^{-2}] + [FeOH^{+1}] + 8[FeSO_{4}] +

[FeOH^{+2}] + 2[Fe(OH)_{2}^{+1}] + 2[Fe_{2}(OH)_{2}^{+4}]+8[FeSO_{4}^{+1}]+16[Fe(SO_{4})_{2}^{-1}] + [CeOH^{+3}] + 3[Ce_{2}(OH)_{3}^{+5}] +

4[Ce_{2}(OH)_{4}^{+4}] + 8[CeSO_{4}^{+2}] + 16[Ce(SO_{4})_{2}] + 24[Ce(SO_{4})_{3}^{-2}] + [CeOH^{+2}] + 8[CeSO_{4}^{+1}] +

16[Ce(SO_{4})_{2}^{-1}] + 24[Ce(SO_{4})_{3}^{-3}] – (16CV + 6(C_{01}V_{0} + C_{1}V) + 4(C_{02}V_{0} + C_{2}V))/(V_{0}+V) = 0 (18a)

where, in addition to relations 22, we apply

From eq. 20 we have

2∙([Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}]) + 3∙([Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}]) + 4∙([Ce^{+4}]+[CeOH^{+3}]+2[Ce_{2}(OH)_{3}^{+5}]+2[Ce_{2}(OH)_{4}^{+4}]+[CeSO_{4}^{+2}] +[Ce(SO_{4})_{2}]+[Ce(SO_{4})_{3}^{-2}]) + 3∙([Ce^{+3}]+[CeOH^{+2}]+[CeSO_{4}^{+1}]+[Ce(SO_{4})_{2}^{-1}]+[Ce(SO_{4})_{3}^{-3}]) – (2·C_{0}V_{0} + 4·CV)/(V_{0}+V) = 0 (20a)

The linear combination of equations: 16 (multiplied by 2), 17 (multiplied by 4) and 20 gives the next/shortest form of GEB

[Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}] –

([Ce^{+3}]+[CeOH^{+2}]+[CeSO_{4}^{+1}]+[Ce(SO_{4})_{2}^{-1}]+[Ce(SO_{4})_{3}^{-3}]) = 0 (25)

where oxidized forms of Fe and reduced forms of Ce are interrelated; molar concentrations: C_{02} and C are not involved there explicitly.

For calculation purposes, related to the System III, the GEB, e.g. eq. 23a, is completed by charge and concentrations balances, obtained from equations 13-17 and relations 22, 24:

[H^{+1}] – [OH^{-1}] – [HSO_{4}^{-1}] – 2[SO_{4}^{-2}] – [HCO_{3}^{-1}] – 2[CO_{3}^{-2}] + 2[Fe^{+2}] + [FeOH^{+1}] +

3[Fe^{+3}] + 2[FeOH^{+2}] + [Fe(OH)_{2}^{+1}] + 4[Fe_{2}(OH)_{2}^{+4}] + [FeSO_{4}^{+1}] – [Fe(SO_{4})_{2}^{-1}] +

4[Ce^{+4}] + 3[CeOH^{+3}] + 5[Ce_{2}(OH)_{3}^{+5}] + 4[Ce_{2}(OH)_{4}^{+4}] + 2[CeSO_{4}^{+2}] – 2[Ce(SO_{4})_{3}^{-2}] +

3[Ce^{+3}] + 2[CeOH^{+2}] + [CeSO_{4}^{+1}] – [Ce(SO_{4})_{2}^{-1}] – 3[Ce(SO_{4})_{3}^{-3}] = 0 (13a)

[HSO_{4}^{-1}] + [SO_{4}^{-2}] + [FeSO_{4}] + [FeSO_{4}^{+1}] + 2[Fe(SO_{4})_{2}^{-1}] + [CeSO_{4}^{+2}] + 2[Ce(SO_{4})_{2}] +

3[Ce(SO_{4})_{3}^{-2}] + [CeSO_{4}^{+1}] + 2[Ce(SO_{4})_{2}^{-1}] + 3[Ce(SO_{4})_{3}^{-3}] –

(C_{0}V_{0} + C_{01}V_{0} + 2CV + C_{1}V)/(V_{0}+V) = 0 (14a)

[H_{2}CO_{3}] + [HCO_{3}^{-1}] + [CO_{3}^{-2}] – (C_{02}V_{0} + C_{2}V)/(V_{0}+V) = 0 (15a)

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] + [Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}] – C_{02}V_{0}/(V_{0}+V) = 0 (16a)

[Ce^{+4}] + [CeOH^{+3}] + 2[Ce_{2}(OH)_{3}^{+5}] + 2[Ce_{2}(OH)_{4}^{+4}] + [CeSO_{4}^{+2}] + [Ce(SO_{4})_{2}] + [Ce(SO_{4})_{3}^{-2}] + [Ce^{+3}] + [CeOH^{+2}] + [CeSO_{4}^{+1}] + [Ce(SO_{4})_{2}^{-1}] + [Ce(SO_{4})_{3}^{-3}] – CV/(V_{0}+V) = 0 (17a)

**The relations for equilibrium constants values**

Concentrations of some species are interrelated in the set of independent expressions, where numerical values for the corresponding equilibrium constants are involved, and applied in the related algorithms.

[H^{+1}][OH^{-1}] = 10^{-14.0}; [HSO_{4}^{-1}] = 10^{1.8}[H^{+1}][SO_{4}^{-2}]; [H_{2}CO_{3}] = 10^{16.4}[H^{+1}]^{2}[CO_{3}^{2}]; [HCO_{3}^{-1}] = 10^{10.1}[H^{+1}][CO_{3}^{-2}];

[Fe^{+3}] = [Fe^{+2}]∙10^{A(E – 0.771)}; [FeOH^{+1}] =10^{4.5}[Fe^{+2}][OH^{-1}]; [FeOH^{+2}] = 10^{11.0}[Fe^{+3}][OH^{-1}];

[Fe(OH)_{2}^{+1}] = 10^{21.7}[Fe^{+3}][OH^{-1}]^{2}; [Fe_{2}(OH)_{2}^{+4}] = 10^{21.7}[Fe^{+3}]^{2}[OH^{-1}]^{2}; [FeSO_{4}] = 10^{2.3}[Fe^{+2}][SO_{4}^{-2}];

[FeSO_{4}^{+1}] = 10^{4.18}[Fe^{+3}][SO_{4}^{-2}]; [Fe(SO_{4})_{2}^{-1}] = 10^{7.4}[Fe^{+3}][SO_{4}^{-2}]^{2};

[MnO_{4}^{-1}] = [Mn^{+2}]∙10^{5A(E – 1.507) + 8pH}; [MnO_{4}^{-2}] = [Mn^{+2}]∙10^{4A(E – 1.743) + 8pH}; [Mn^{+3}] = [Mn^{+2}]∙10^{A(E – 1.509)};

[MnOH^{+2}] = 10^{14.2}[Mn^{+3}][OH^{-1}]; [MnSO_{4}] = 10^{2.28}∙[Mn^{+2}][SO_{4}^{-2}];

[Ce^{+4}] = [Ce^{+3}]∙10^{A(E–1.70)}; [CeOH^{+3}] = 10^{13.3}[Ce^{+4}][OH^{-1}]; [Ce_{2}(OH)_{3}^{+5}] = 10^{13.3}[Ce^{+4}]^{2}[OH^{-1}]^{3};

[Ce_{2}(OH)_{3}^{+5}] = 10^{40.3}[Ce^{+4}]^{2}[OH^{-1}]^{3}; [Ce_{2}(OH)_{4}^{+4}] = 10^{53.7}[Ce^{+4}]^{2}[OH^{-1}]^{4}; [CeOH^{+2}] = 10^{5.0}[Ce^{+3}][OH^{-1}]; [CeSO_{4}^{+1}] = 10^{1.63}[Ce^{+3}][SO_{4}^{-2}]; [Ce(SO_{4})_{2}^{-1}] = 10^{2.34}[Ce^{+3}][SO_{4}^{-2}]^{2}; [Ce(SO_{4})_{3}^{-3}] = 10^{3.08}[Ce^{+3}][SO_{4}^{-2}]^{3}; [CeSO_{4}^{+2}] = 10^{3.5}[Ce^{+4}][SO_{4}^{-2}]; [Ce(SO_{4})_{2}] = 10^{8.0}[Ce^{+4}][SO_{4}^{-2}]^{2}; [Ce(SO_{4})_{3}^{-2}] = 10^{10.4}[Ce^{+4}][SO_{4}^{-2}]^{3}. (26)

where

**7. Fraction titrated**

The results of simulated titrations, with measurable values: potential E and/or pH of the D+T system, are plotted as the functions E = E(V) and/or pH = pH(V). In some instances, it is more advantageous/reasonable to plot the graphs: E = E(Φ) and/or pH = pH(Φ), with the fraction titrated [25-28].

on the abscissa, where C_{0} – concentration [mol/L] of the analyte A in D, C – concentration [mol/L] of reagent B in T; V_{0} mL is the volume of D taken for titration, V is the current/total volume of T added into D from the start up to a given point/moment of the titration. The Φ provides a kind of uniformity/normalization of the related plots, i.e., independency on V_{0} value.

For the Systems I and III, where FeSO_{4} is the single analyte, eq. 28 can be rewritten as follows

where C_{0} = C_{02}.

The fraction titrated Φ (eq. 28) will be applied first to formulate the Generalized Equivalent Mass (GEM) concept.

**8. Generalized equivalent mass (GEM)**

The main task of a titration made for analytical purposes is the estimation of the equivalent volume, V_{eq}, corresponding to the volume V of T, where the fraction titrated (eq. 28) assumes the value

equal to the ratio p/q of small natural numbers p and q, Φ_{eq} = p/q. This ratio will be formulated on the basis of location of characteristic points on redox titration curves E = E(Φ).

In contradistinction to visual titrations, where the end (e) volume V_{e}V_{eq} is registered [21,27], all instrumental titrations aim, in principle, to obtain the V_{eq} value on the basis of experimental data {(V_{j}, y_{j}) | j=1,…,N}, where y = pH or E for potentiometric methods of analysis. Referring again to eq. 28, we have

where m_{A} [g] and M_{A} [g/mol] denote mass and molar mass of analyte (A), respectively. From equations: 28 and 30, we get

The value of the fraction in eq. 31, obtained from eq. 28,

is constant during the titration. Particularly, at the end (e) and equivalent (eq) points we have

The V_{e} [mL] value is the volume of T consumed up to the end (e) point, where the titration is terminated (ended). The V_{e} value is usually determined in visual titration, when a pre-assumed color (or color change) of D+T mixture is obtained. In a visual acid-base titration, pH_{e} value corresponds to the volume V_{e} [mL] of T added from the start of the titration, and

is the ɸ-value related to the end point. From equations 31 and 33, one obtains:

This does not mean, however, that we may choose between equations 35a and 35b, to calculate m_{A}. Namely, eq. 35a cannot be applied for the evaluation of m_{A}: V_{e} is known, but F_{e} is unknown; calculation of F_{e} needs prior knowledge of C_{0} value. However, C_{0} is unknown before the titration; otherwise, the titration would be purposeless. Also eq. 35b is useless: the ‘round’ Φeq value is known exactly, but V_{eq} is unknown; V_{e} (not V_{eq}) is determined in visual titrations.

Because the equations: 35a and 35b appear to be useless, the third, approximate formula for m_{A}, has to be applied, namely:

where Φ_{eq} is put for F_{e} in eq. 35a, and

is named as the equivalent mass. The relative error in accuracy, resulting from this substitution, equals to

The Generalized Equivalence Mass (GEM) concept was formulated (1979) by Michałowski [18,19,21,25], as the counterproposal to earlier (1978) IUPAC decision [29], see also [30].

**7. Computer program for the System I**

The calculations in GATES/GEB are realized according to iterative computer program. The exemplary computer program, related to the System I, is as follows.

function F = Function_MnO4_Fe(x)

global V Vmin Vstep Vmax V0 C C2 C02 C04 C05 H OH fi pH E

global Kw pKw A K logK

global HSO4 SO4 logHSO4 logSO4

global H2CO3 HCO3 CO3 logH2CO3 logHCO3 logCO3

global Mn7O4 Mn6O4 Mn3 Mn3OH

global logMn7O4 logMn6O4 logMn3 logMn3OH

global Mn2 Mn2OH Mn2SO4

global logMn2 logMn2OH logMn2SO4

global Fe2 Fe2OH Fe2SO4

global logFe2 logFe2OH logFe2SO4

global Fe3 Fe3OH Fe3OH2 Fe32OH2 Fe3SO4 Fe3SO42

global logFe3 logFe3OH logFe3OH2 logFe32OH2 logFe3SO4 logFe3SO42

pH=x(1);

E=x(2);

Mn2=10.^-x(3);

Fe2=10.^-x(4);

SO4=10.^-x(5);

H2CO3=10.^-x(6);

H=10.^-pH;

pKw=14;

Kw=10.^-14;

OH=Kw./H;

A=16.9;

ZFe=26;

ZMn=25;

Mn7O4=Mn2.*10.^(5.*A.*(E-1.507)+8.*pH);

Mn6O4=Mn2.*10.^(4.*A.*(E-1.743)+8.*pH);

Mn3=Mn2.*10.^(A.*(E-1.509));

Fe3=Fe2.*10.^(A.*(E-0.771));

HSO4=10.^1.8.*H.*SO4;

HCO3=10.^(pH-6.3)*H2CO3.

CO3=10^(pH-10.1)*HCO3.

Fe2OH=10.^4.5.*Fe2.*OH;

Fe2SO4=10.^2.3.*Fe2.*SO4;

Fe3OH=10.^11.0.*Fe3.*OH;

Fe3OH2=10.^21.7.*Fe3.*OH.^2;

Fe32OH2=10.^25.1.*Fe3.^2.*OH.^2;

Fe3SO4=10.^4.18.*Fe3.*SO4;

Fe3SO42=10.^7.4.*Fe3.*SO4.^2;

Mn2OH=10.^3.4.*Mn2.*OH;

Mn2SO4=10.^2.28.*Mn2.*SO4;

Mn3OH=10.^14.2.*Mn3.*OH;

K=C.*V./(V0+V);

%Charge balance

F=[(H-OH+K-HSO4-HCO3-2.*CO3-2.*SO4-Mn7O4-2.*Mn6O4...

+3*Mn3+2.*Mn3OH+2.*Mn2+Mn2OH+2.*Fe2+Fe2OH+3.*Fe3...

+2.*Fe3OH+Fe3OH2+4.*Fe32OH2+Fe3SO4-Fe3SO42);

%Concentration balance of Mn

(Mn7O4+Mn6O4+Mn3+Mn3OH+Mn2+Mn2OH+Mn2SO4-C.*V./(V0+V));

%Concentration balance of Fe

(Fe2+Fe2OH+Fe2SO4+Fe3+Fe3OH+Fe3OH2+2.*Fe32OH2...

+Fe3SO4+Fe3SO42-C02.*V0./(V0+V));

%Concentration balance of S

(HSO4+SO4+Mn2SO4+Fe2SO4+Fe3SO4+2.*Fe3SO42...

-(C02+C04).*V0./(V0+V));

%Concentration balance of C

(H2CO3+HCO3+CO3-(C2*V+C05*V0)./(V0+V);

%Electron balance

((ZMn-7).*Mn7O4+(ZMn-6).*Mn6O4+(ZMn-3).*(Mn3+Mn3OH)...

+(ZMn-2).*(Mn2+Mn2OH+Mn2SO4)+(ZFe-2).*(Fe2+Fe2OH+Fe2SO4)...

+(ZFe-3).*(Fe3+Fe3OH+Fe3OH2+Fe32OH2+Fe3SO4+Fe3SO42)...

-((ZFe-2).*C02.*V0+(ZMn-7).*C.*V)./(V0+V))];

logMn2=log10(Mn2);

logMn2OH=log10(Mn2OH);

logMn2SO4=log10(Mn2SO4);

logMn3=log10(Mn3);

logMn3OH=log10(Mn3OH);

logMn6O4=log10(Mn6O4);

logMn7O4=log10(Mn7O4);

logFe2=log10(Fe2);

logFe2OH=log10(Fe2OH);

logFe2SO4=log10(Fe2SO4);

logFe3=log10(Fe3);

logFe3OH=log10(Fe3OH);

logFe3OH2=log10(Fe3OH2);

logFe32OH2=log10(Fe32OH2);

logFe3SO4=log10(Fe3SO4);

logFe3SO42=log10(Fe3SO42);

logHSO4=log10(HSO4);

logSO4=log10(SO4);

logH2CO3=log10(H2CO3);

logHCO3=log10(HCO3);

logCO3=log10(CO3);

logK=log10(K);

**8. Graphical and numerical presentation of results **

The results of calculations for the System I are presented graphically in Figures 1a-d, 2a-d (with E = E(Φ) and pH = pH(Φ) functions), and 3a,b, 4a,b (with speciation diagrams). Numerical data (Φ,E) from the vicinity of the jump in potential E-value (Fig. 1a) are collected in Table 1 [31]. The jump occurs here at Φ = Φ_{eq} = 0.2, named as equivalent (eq) point; note that 0.20000 ≡ ≡ 1 : 5. The coordinates of equivalent point are (Φ_{eq}, E_{eq}) = (0.20000, 1.034), with Φ_{eq} as the stoichiometric point of the reaction

MnO_{4}^{-1} + 5Fe^{+2} + 8H^{+1} = Mn^{+2} + 5Fe^{+3} + 4H_{2}O (39)

This reaction written in terms of predominating species (see Figures 3a,b) is as follows

MnO_{4}^{-1} + 5FeSO_{4} + 6HSO_{4}^{-1} + 2H^{+1} = MnSO_{4} + 5Fe(SO_{4})_{2}^{-1} + 4H_{2}O (40)

No changes in slope on the pH = pH(Φ) curves occur at Φ_{eq} = 0.2 (Fig. 1b), although one would expect, at first glance, that MnO_{4}^{-1} may act, especially in reaction 39, like 'octopus' swallowing H^{+1} at Φ < 0.2, while the reaction 39 does not occur at Φ > 0.2. High value of the dynamic buffer capacity [32-34] in the D+T system is responsible for suppressing this effect. Analogous remark is related to the System III, represented by E = E(Φ) and pH = pH(Φ) relationships (Fig. 2), and speciation curves (Fig. 4).

**Fig. 1.** The (1a) E = E(Φ) and (1b) pH = pH(Φ) curves plotted for the System I at V_{0} = 100, (C_{02},V_{0},C) = (0.01,100, 0.02) and different C_{04} values [mol/L], indicated in Figures 1b, 1c and 1d (in enlarged scales), before and after Φ_{eq} = 0.2; C_{2}=C_{05}=0.

**Table 1.** The pairs of (Φ, E) values for the System I, (C_{02},C_{04},V_{0},C) = (0.01,1.0,100, 0.02) in the close vicinity of (Φ_{eq}, E_{eq}); E in NHE scale

Φ |
E [V] |

0.19800 0.19900 0.19980 0.19990 0.19998 0.20000 0.20002 0.20010 0.20020 0.20200 |
0.701 0.719 0.761 0.778 0.820 1.034 1.323 1.365 1.382 1.442 |

**Fig. 2.** The (2a) E = E(Φ) and (2b) pH = pH(Φ) curves plotted for the System III at V_{0} = 100, (C_{02},V_{0},C,C_{1}) = (0.01,100, 0.1,1.0) and different C_{04} values [mol/L], indicated in Figures 2b, 2c and 2d (in enlarged scales), before and after Φ_{eq} = 1.0; C_{2}=C_{05}=0.

**Fig. 3**. Dynamic speciation diagrams for (3a) Fe-species, (3b) Mn-species in the System I ; (C_{02},C,C_{04}) = (0.01,0.02,1.0), C_{2}=C_{05}=0, V_{0}=100.

**9. Formulation of the modified Gran methods**

**9.1. Preliminary relations **

The redox potential E of a chemical system is measured with use of an inert metal (usually: platinum) as the indicator electrode in conjunction with a reference/counter electrode to form a complete cell; the E value in the system, involved with redox reaction

Fe^{+3} + e^{-1} = Fe^{+2} (41)

is expressed by the Nernst equation

where ϑ = a∙ln10 is the real slope of indicator electrode; and values are assumed constant during the titration; the involves standard redox potential E_{0} for reaction 41, potential of reference electrode, and liquid junction potential.

**Fig.4.** Dynamic speciation diagrams for (4a) Fe-species, (4b) Ce-species in the System III; (C,C_{1},C_{02},C_{04}) = (0.1,0.5,0.02,1.0), C_{2}=C_{05}=0, V_{0}=100.

For further discussion, we collect first the equations for GEB related to two different D+T systems: System I and System III, with FeSO_{4} (C_{02}) + H_{2}SO_{4} (C_{04}) as D. The GEB expressed by eq. 11a, and rewritten as follows:

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] – (5[MnO_{4}^{-1}]+4[MnO_{4}^{-2}]+[Mn^{+3}]+[MnOH^{+2}]) = (C_{02}V_{0} – 5CV)/(V_{0}+V) (11b)

is applicable for the Systems I and II, whereas concentration balance for Fe in the System II is presented as follows

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] + [Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}] = (C_{02}+2C_{03})V_{0}/(V_{0}+V) (4b)

For the System I, we have C_{03}=0 in eq. 4b, i.e.,

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}]+[Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]_{}+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}]= = C_{02}V_{0}/(V_{0}+V) (4c)

In turn, for the System III we refer to equations 23a and 16a, rewritten analogously:

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] – ([Ce^{+4}]+[CeOH^{+3}]+2[Ce_{2}(OH)_{3}^{+5}]+2[Ce_{2}(OH)_{4}^{+4}]+ [CeSO_{4}^{+2}]+[Ce(SO_{4})_{2}]+[Ce(SO_{4})_{3}^{-2}]) = (C_{02}V_{0} – CV)/(V_{0}+V) , and (23b)

[Fe^{+2}]+[FeOH^{+1}]+[FeSO_{4}] + [Fe^{+3}]+[FeOH^{+2}]+[Fe(OH)_{2}^{+1}]+2[Fe_{2}(OH)_{2}^{+4}]+[FeSO_{4}^{+1}]+[Fe(SO_{4})_{2}^{-1}] = C_{02}V_{0}/(V_{0}+V) (16b)

The latter one is identical with eq. 4c.

**9.2. Derivation of formulas for the Systems I and III**

From relations: CV = Φ∙C_{02}V_{0}, and CV_{eq} = Φ_{eq}∙C_{02}V_{0}, we have

At low pH values (Figures 1b, 2b), on the basis of speciation diagrams (Figures 3, 4), the balances: 11b and 23b at Φ < Φ_{eq} can be presented in the simplified forms:

[Fe^{+2}] + [FeSO_{4}] = (C_{02}V_{0} – 5CV)/(V_{0}+V) (at Φ_{eq} < 0.2, for the Systems I, II) (11c)

[Fe^{+2}] + [FeSO_{4}] = (C_{02}V_{0} – CV)/(V_{0}+V) (at Φ_{eq} < 1.0, for the System III) (23c)

At Φ_{eq} < 0.2 for the System I (Fig. 2) and at Φ_{eq} < 1.0 (Fig. 4) for the System III, the simplified balance for Fe can be applied

[Fe^{+2}] + [FeSO_{4}] + [Fe^{+3}] + [FeSO_{4}^{+1}] + [Fe(SO_{4})_{2}^{-1}] = C_{02}V_{0}/(V_{0}+V) (4c)

Applying the appropriate formulas found in (26), from equations: 11c, 23c and 4c we get, by turns:

[Fe^{+2}]∙b_{2} = (C_{02}V_{0} – 5CV)/(V_{0}+V) (11d)

[Fe^{+2}]∙b_{2} = (C_{02}V_{0} – CV)/(V_{0}+V) (23d)

[Fe^{+2}]∙b_{2} + [Fe^{+3}]∙b_{3} = C_{02}V_{0}/(V_{0}+V) (4d)

where : b_{2 }= 1 + 10^{2.3}×[SO_{4}^{–2}] , b_{3 }= 1 + 10^{4.18}×[SO_{4}^{–2}] + 10^{7.4}×[SO_{4}^{–2}]^{2}, i.e.,

whereas from equations: 23d, 4d, 43 and Φ_{eq} =1, we have

i.e., the expressions for the ratio [Fe^{ +3}] /[Fe^{ +2}] are identical in the Systems: I and III. In the System III, the value of b_{3}/b_{2} (eq. 44) depends on H_{2}SO_{4} concentrations: C_{04} in D, and C_{1} in T, whereas in the System I, we have C_{1} = 0 in T. Then from equations: 42 and 45 (or 46), we get the relation

valid for V < V_{eq}.

The θ = In b_{3}/b_{2} vs. Φ relationships [10] are plotted for the Systems: I (Fig. 5a) and III (Fig. 5b). We see that dθ/dΦ <0 in Fig. 5a, and dθ/dΦ <0 in Fig. 5b. The θ vs. Φ relationships are *quasi*-linear, especially for greater C_{04} values. Then we can assume the relation

where ω = is the new constant value, obtained from constant values introduced above. From eq. 49 we have, by turns,

where ϑ = a∙ln10, and

At high C_{04} value, the change of value is relatively small (Figures 5a,b); b = 1.7×10^{-3} at C_{04} = 1 mol/L. Then the assumption = const can be applied below in the simplified model. Putting β = 0 in eq. 50, we get

where G_{2} = = const. Applying in eq. 50 the approximation , valid for ≪ 1, we have, by turns

where:

P = G_{2}∙β , Q = G_{2}∙(β∙V_{eq} + 1) , R = G_{2}∙V_{eq} (54)

Eq. 53 rewritten in the form of regression equation

is the basis for calculation of values for parameters: P, Q, R, determined according to the LSM. On the basis of relations 54, we get, by turns,

Equations 53a and 55 are the basis for the modified Gran II method in its accurate version, denoted in [ACA606] as MG(II)A, which improves the results dramatically. Moreover, the error z of analysis is not affected significantly by the true ϑ value for the slope of an indicator electrode.

Fig. 5. The q = ln(b_{3}/b_{2}) vs. F relationships for the Systems: I (5a), at (C,C_{02}) = (0.02,0.01), and III (5b), plotted at (C,C_{1},C_{02}) = (0.1,0.5,0.01), V_{0}=100, C_{2}=C_{05}=0, and different C_{04} values indicated at the corresponding curves.

**9.3. Accurate model **

For two consecutive points (V_{j}, E_{j}) and (V_{j+1}, E_{j+1}) referred to potentiometric titration of D with T, from eq. 49 we have

Applying in eq. 56 the identities:

we get

Applying in eq. 52 the approximation [9-11,25,35] (see Fig. 6)

we write

where

Fig. 6. Comparison of the plots for: (1) f_{1}(x) = ln(1+x), (2) f_{2}(x) = and (3) f_{3}(x) = x, x ∈ < 0, 1 > .

Applying eq. 60b in eq. 58, we get the accurate model, written in terms of regression equation

The parameters: V_{eq}, a and β are obtained there according to an iterative computer program, by minimization of the sum of squares

**9.4. Approximate models (β=0)**

** Model 1**.

Putting β = 0 in eq. 62, we get, after transformation

where

is a constant value, for the specific titration, see eq. 61. Denoting

from eq. 58 we have the regression equation

The R and G_{I} are determined there according to LSM:

and then we get

where

in equations 68, 69; N – number of exp. points (V_{j},E_{j}) | j=1,…,N. The formulation applied here is the basis for the modified G(I) method in its simplified version, denoted as MG(I)S version [10]. The great advantage of MG(I)S over G(I) method results from application of formulas 59 instead of approximation ln(1±x) ≈ ± x inherent in the G(I) method, see Fig. 6.

** Model 2**.

Referring again to eq. 52, we calculate the first and second derivatives of (eq. 51) [11]:

Note that the first derivative of eq. 52 is ** **

Zeroing the second derivative (eq. 71) gives

The first and second derivatives on the right side of Eq. 71 can be approximated by differential quotients

where

For the set of experimental points {(V_{j}, E_{j})│j = 1,…, N – 1}, we have: ΔV = V_{j+1} – V_{j}, ΔE = E_{j+1} – E_{j}. Both differential quotients:

are put at V_{j}^{*} (eq. 61). Then the J_{j} = J(V_{j}) values were calculated from the formula 72a. The formulas presented here are the basis for the MG(II)B method [11]. An alternative is here the MG(II)C method [11], based on the Lagrange polynomial interpolation method.

The interrelations between G(I), G(II) and different modifications of these methods are collected in [11].

**9.5. Derivation of formulas for the System II **

Referring to the System II, one can state/assume that the composition of the titrand D can be affected here by partial oxidation of the iron(+2) species by oxygen from air, as in the case of natural waters.

As stated above, eq. 11b and eq. 11d, as its simplified form, are valid also for the System II. At Φ < 0.2, the balance 4b can be written as follows

Then from equations 11d and 73 we get, by turns,

At C_{03}=0, eq. 74 is transformed into equations 45, 46. From equations 42 and 74 we have

Assuming = const, i.e., β = 0 in eq. 48, and applying eq. 75 for two consecutive points (V_{j}, E_{j}) and (V_{j+1}, E_{j+1}) referred to potentiometric titration of D with T in the System II, we have

Denoting

from eq. 76 we get

Applying the approximations 59 for 77, after transformations of eq. 76 we get, by turns,

and is the difference between the u_{j} value found from measurements and the u() value found at V = from the model assumed. Then we calculate [9]

**Application of Gran methods for calibration purposes**

Calibration of redox indicator electrodes (RIEs) is of primary importance in potentiometric measurements performed in redox systems. The difficulties in calibration of RIEs were probably the main reason for generating the opinion on inapplicability of the Gran II (G(II)) method for determination of equivalence volume (V_{eq}) in redox titrations. This problem has been exposed [10], where inaccuracy of the results obtained according to G(II) method at greater discrepancies between true (correct, J) and pre-assumed (J_{c}) slope values, |J_{c }– J| for RIEs has been proved [10]. It was also stated that the error in V_{eq} can be substantially decreased, even at greater |J_{c }– J| values, if the modified Gran II method in its accurate version (MG(II)A) proposed in [10] is applied; the MG(II)A method improves the results dramatically (Fig. 7). The error *z *is not affected significantly by the true ϑ-value of an indicator electrode.

**Fig. 7.** The relationships between relative error e [%] in V_{eq} determination vs J [mV] plotted for G(II) and MG(II)A methods, at J_{c} = 56 mV value pre-assumed in calculations [11].

**Final comments**

It is stated that the linearizing approaches, inherent in original G(I) and G(II) methods, may provide inaccurate results of analyses. It were stated that the original Gran methods, particularly G(I) method [1], do not provide accurate results for V_{eq}; the errors involved in G(I) may exceed tens percents, as indicated in [12]. Far more accurate results of analysis are obtainable according to the modified methods proposed by Michałowski in a series of papers [9-12,25], after recalling to the physicochemical nature of the system tested.

Also the original G(II) [3] method may not provide accurate results in the titrations; the matter lies in the divergence (ranging several percents [9]) between true and Nernstian slopes of the indicator electrode and in some difficulties encountered in calibration of this electrode.

In contradistinction to the G(II) method, the G(I) method offers the possibility to perform the potentiometric titrations without prior knowledge of ϑ – provided that ϑ is constant within defined V-range covered in the Gran methods, where the validity of assumption ϑ = ϑ(V) = const is increased – in contradistinction to the methods based on the inflection point location; a dramatic change of the analyte concentration occurs in the vicinity of this point. Such advantages of G(I) method were successfully exploited in the modified G(I) methods [9-12,25], thereafter referred to as simplified (MG(I)S) and accurate (MG(I)A) methods [10].

The results of calculations related to redox systems were obtained according to GATES/GEB principles, with use of the iterative computer program MATLAB and the generator of pseudo-random numbers [36]; these results were confirmed experimentally in [10,11].

The Generalized approach to electrolytic systems (GATES) [13] with the generalized electron balance (GEB) involved as GATES/GEB, is adaptable for resolution of thermodynamic (equilibrium and metastable) redox systems of any degree of complexity; none simplifying assumptions are needed [10]. Application of GATES provides the reference levels for real analytical systems, where some effects involved with kinetics and transportation (diffusion) phenomena occurred at the electrodes. The GATES makes possible to exhibit some important details, of qualitative and quantitative nature, invisible in real experiment, e.g. speciation. Reliability of physicochemical data (standard potentials, equilibrium constants of complexes, etc.) values is needed for this purpose. This requirement is fulfilled, among others, for 1◦ manganometric and 2◦ cerometric titrations of ferrous ions, where equilibria are established rapidly in the bulk solution. This way, we provide an approach to a more general problem involved with optimization *a priori *in redox systems, realized according to GATES principle.

The GATES approach is based on mathematical foundations, expressed by a system of nonlinear algebraic equations, not on a “fragile” chemical reaction notation, based on stoichiometry. Within GATES, the stoichiometry concept, as a resultant of all particular (stoichiometric, in principle) chemical reactions occurred in a dynamic system (as titration is) is not applied. Among others, the generalized equivalence mass (GEM) concept, based on GATES, is not involved with the stoichiometry concept. The stoichiometry is only a redundant concept within GATES and then formulation of reaction notation can be considered only as a kind of intellectual/didactic occupation, that can be made after presentation of the related curves obtained from calculations based on GATES.

The GEB (as Approaches I and II to GEB), GATES, GEM and all modifications of the Gran methods were discovered/suggested/formulated by Michałowski [9-12,25], and extended on different acid-base systems, involved also with total alkalinity [28,36,37], also with fulvic acids involved [38], and carbonate alkalinity [39], in particular.

** **

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