Question

If 1 mole of $H_{3}P{O}_4$ reacts with 1 mole of $X(OH{)}_2$ as shown below:
$H_{3}P{O}_4+X(OH{)}_2\to XHP{O}_4+2H_{2}O$ then:

• A. The equivalent mass of base is $\frac{\text{mol. mass}}{2}$
• B. The equivalent mass of $H_{3}P{O}_4$ is $\frac{98}{3}$
• C. The resulting solution requires 1 mole NaOH for complete neutralization
• D. Minimum 1 mole of $X(OH{)}_2$ is required for complete neutralization of $XHP{O}_4$

Answer 1

Answer: (A), (C)

The correct options are
A The equivalent mass of base is $\frac{\text{mol. mass}}{2}$
C The resulting solution requires 1 mole NaOH for complete neutralization

$\underset{\text{n-factor = 2}}{H_{3}P{O}_4}+\underset{\text{n - factor = 2}}{X(OH{)}_2}\to XHP{O}_4+2H_{2}O$

(A) Equivalent weight of base = $=\frac{\text{mol. wt}}{2}$

(B) Equivalent weight of $H_{3}P{O}_4=\frac{98}{2}$

(C) Moles of $NaOH\times 1$ = moles of $XHP{O}_4\times 1$
Moles of $NaOH=1\times 1=1$

(D) Moles of $X(OH{)}_2$ required $=\frac{1}{2}$