How to calculate equivalent weight ?
Eequivalent weight Calculations
So, if you want to calculate equivalent weight you must have a clear concept on valency factor which we say n-factor , Equivalent weight of any molecule can be define as Molecular weight divided by n-factor , so let’s understand the meaning of n-factor to have clear idea of calculating the equivalent weight of any molecules.
Equivalent weight. = Molecular weight/n-factor
The equivalent of a substance is calculated as
∴ Number of equivalents ==
∴ Number of equivalents = no. of moles × n factor
n Factor Calculation
Since, equivalent of a substance = and eqv. mass =
Thus, to calculate the equivalents of any substance, the knowledge of n factor calculation is a must. The n factor of various substances is calculated as:
1. Acids : The number of moles of replaceable H+ ions per mole of the acid i.e. basicity.
For example, HNO3; n = 1; H2SO4; n =2; H3PO4; n = 3, H3PO3; n = 2, H3BO3; n = 1
All these values are the maximum values of n factor for the corresponding acid e.g. the n factor for H2SO4 may be 1 or 2 depending on the reaction it undergoes.
H2SO4 + NaOH NaHSO4 + H2O …(i)
H2SO4 + 2NaOH Na2SO4 + H2O …(ii)
For bases: Bases will be treated as species which furnish OH− ions when dissolved in a solvent. The n-factor of a base is the no. of OH− ions that a molecule of the base would give when dissolved in a solvent (Acidity).
For example, NaOH (n = 1), Ba(OH)2 (n = 2), Al(OH)3 (n = 3), etc.
For salts: A salt reacting such that no atom of the salt undergoes any change in oxidation state.
For example, 2AgNO3 + MgCl2 Mg(NO3)2 + 2AgCl
In this reaction, it can be seen that the oxidation state of Ag, N, O, Mg and Cl remains the same even in the product. The n-factor for such a salt is the total charge on cation or anion.
InRedox Change
For oxidizing agent or reducing agent n-factor is the change in oxidation number per mole of the substance.
SOME OXIDIZING AGENTS /REDUCING AGENTS WITH Equivalent weight
Species |
Changed to |
Reaction |
Electrons exchanged or change in O.N. |
Eq. wt. |
MnO4-(O.A.) |
Mn2+ |
MnO4- + 8H+ +5e- →Mn2++ 4H2O |
5 |
|
MnO4-(O.A.) |
MnO2 |
MnO4- + 3e- +2H2O→ MnO2 + 4OH-
|
3 |
|
MnO4-(O.A.) |
MnO4 2- |
MnO4- + e- → MnO42- |
1 |
|
Cr2O72-(O.A.) |
|
Cr2O72- +14H++6e → 2Cr3+ + 7H2O |
6 |
|
MnO2(O.A.) |
Mn2+ |
MnO2 + 4H++2e-→Mn2+ +2H2O |
2 |
|
Cl2(O.A.) (in bleaching powder) |
Cl-Cl- |
Cl2 + 2e- →2Cl- |
2 |
|
Species |
Changed to |
Reaction |
Electrons exchanged or change in O.N. |
Eq. wt. |
CuSO4(O.A.) (in iodometric titration) |
Cu+ |
Cu2+ +e- → Cu+
|
1 |
|
S2O32-(R.A.) |
S4O62- |
2S2O32- → S4O62- +2e- |
2 (for two molecules) |
|
H2O2(O.A.) |
H2O |
H2O2 +2H+ +2e-→2H2O |
2 |
|
H2O2(R.A.) |
O2 |
H2O2 →O2 +2H+ + 2e-(O. N. of oxygen in H2O2 is −1 per atom) |
2 |
|
Fe2+(R.A.) |
Fe3+ |
Fe2+ → Fe3+ +e- |
1 |
|
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