Chemistry > Stoichiometry > 6.0 Redox Reactions
Stoichiometry
1.0 The Mole
2.0 The Limiting Reagent
3.0 Gravimetric Analysis
4.0 Volumetric Analysis
5.0 Calculation of n-factor
6.0 Redox Reactions
7.0 Titration
7.1 Simple Titration
7.2 Double Titration
7.3 Method
7.4 Titration of the solution containing both $N{a_2}C{O_3}$ and $NaHC{O_3}$
7.5 Titration of the solution containing both $NaOH$ and $N{a_2}C{O_3}$
7.6 Back Titration
8.0 Iodimetric and Iodometric Titrations
9.0 Volume strength peroxide solution
10.0 Percentage Labeling of Oleum
11.0 Hardness of Water
6.1 Precipitation/Double Decomposition Reactions
7.2 Double Titration
7.3 Method
7.4 Titration of the solution containing both $N{a_2}C{O_3}$ and $NaHC{O_3}$
7.5 Titration of the solution containing both $NaOH$ and $N{a_2}C{O_3}$
7.6 Back Titration
In such reaction, there is no change in oxidation state of any atom. The n-factor of the salt can be calculated by multiplying the oxidation state of the cation/anion by total no. of atoms per molecule of the salt. For example
\[\mathop {BaC{l_2}}\limits_{n = 2} + \mathop {N{a_2}S{O_4}}\limits_{n = 2} \xrightarrow{{}}BaS{O_4} \downarrow + 2NaCl\]
for $BaC{l_2}$
n-factor = Oxidation state of Ba atom in $BaC{l_2}$ × number of Ba atoms in 1 molecule of $BaC{l_2}$
$ = {\text{ }}\left( { + 2} \right){\text{ }} \times {\text{ }}1{\text{ }} = {\text{ }}2$
for $N{a_2}S{O_4}$
n-factor = Oxidation state of $Na$ × number of $Na-atoms$ in 1 molecule of $N{a_2}S{O_4}$
$ = \left( { + 1} \right){\text{ }} \times {\text{ }}2{\text{ }} = {\text{ }}2$