7.6 Back Titration

1.1 Significance of Chemical Equations

3.1 Mass-Mass Relationship
3.2 Mass-Volume Relationship
3.3 Volume-Volume Relationship

4.1 Titration
4.2 Molarity $(M)$
4.3 Molality $(m)$
4.4 Normality $(N)$
4.5 Equivalent Weight

5.1 Acid-Base Reaction

6.1 Precipitation/Double Decomposition Reactions

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

8.1 Iodimetric Titrations
8.2 Iodometric Titrations

11.1 Temporary Hardness
11.2 Permanent Hardness

Let us consider that we have an impure solid substance $‘Z’$ weighing $‘w’$ $g$ and we are required to calculate the percentage purity of $‘Z’$ in the sample. We are also provided with two solutions $‘X’$ and $‘Y’$, where the concentration of $‘Y’$ is known $\left( {{N_1}} \right)$ and that of $‘X’$ is unknown. For the back titration to work, following conditions are to be satisfied

(a) Compounds $‘X’$, $‘Y’$ and $‘Z’$ should be such that $‘X’$ and $‘Y’$ reacts with each other.

(b) $‘X’$ and pure $‘Z’$ also reacts with each other but the impurity present in $‘Z’$ does not react with $‘X’$.

\[Z{\text{ }} + {\text{ }}X{\text{ }}\left( {excess} \right) \to Product{\text{ }}1\]

\[Remaining{\text{ }}\left( X \right){\text{ }} + {\text{ }}Y \to Product{\text{ }}2\]