Redox Equivalent Concept & Titration formulas

Every formula JEE Advanced expects you to know for Redox Equivalent Concept & Titration, with the variables spelled out. Free, no sign-up. Read it before a mock, not during one.

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Formulas: 22
Subject: Chemistry
Exam: JEE Advanced
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Redox Equivalent Concept & Titration, every formula

22 formulas, typeset and free. Print it, or keep it open beside your practice.

Oxidation
$loss of electrons (increase in oxidation number)$
Reduction
$gain of electrons (decrease in oxidation number)$
n-factor (acid)
$n = number of replaceable H^{+}$
n-factor (base)
$n = number of replaceable O H^{-}$
n-factor (redox)
$n = change in oxidation number$
Equivalent weight
$E = \frac{molar mass}{n -factor}$
Gram equivalents
$eq = \frac{mass}{E} = n \times moles$
Normality
$N = \frac{gram equivalents}{volume (L)}$
Normality–molarity
$N = M \times n -factor$
Law of equivalents
$N_{1} V_{1} = N_{2} V_{2}$
at end point
Equivalents balance
$eq of oxidant = eq of reductant$
Percentage purity
$% = \frac{mass of pure substance}{mass of sample} \times 100$
Molarity of a mixture
$M = \frac{N _{1} V _{1} + N _{2} V _{2}}{V _{1} + V _{2}}$
Volume-strength of H₂O₂
$V.S. = 5.6 \times N$
Hardness (ppm CaCO₃)
$ppm = \frac{mass of CaCO _{3}}{mass of water} \times 1 0^{6}$
Oxidation number of O
$- 2 (usually), - 1 (peroxides)$
Oxidation number of H
$+ 1 (usually), - 1 (hydrides)$
Sum of oxidation numbers
$neutral molecule = 0, ion = charge$
Disproportionation
$same element both oxidised and reduced$
Equivalents from Faraday
$eq = \frac{I t}{96500}$
Back titration principle
$eq_{e x cess} = eq_{a dd e d} - eq_{r e a c t e d}$
Mole–equivalent relation
$equivalents = n -factor \times moles$

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Redox Equivalent Concept & Titration formulas

Redox Equivalent Concept & Titration, every formula

Oxidation

Reduction

n-factor (acid)

n-factor (base)

n-factor (redox)

Equivalent weight

Gram equivalents

Normality

Normality–molarity

Law of equivalents

Equivalents balance

Percentage purity

Molarity of a mixture

Volume-strength of H₂O₂

Hardness (ppm CaCO₃)

Oxidation number of O

Oxidation number of H

Sum of oxidation numbers

Disproportionation

Equivalents from Faraday

Back titration principle

Mole–equivalent relation

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