# What is the molarity of the masonic acid solution? H_2C_3H_2O_4 + 2NaOH -> Na_2C_3H_2O_4 + 2H_2O

## A solution of malonic acid, ${H}_{2} {C}_{3} {H}_{2} {O}_{4}$, was standardized by titration with 0.1000 M $N a O H$ solution. If 20.76 mL of the $N a O H$ solution were required to neutralize completely 13.15 mL of the malonic acid...

Jul 7, 2016

$\text{Concentration of malonic acid } \cong$ $8 \times {10}^{-} 2 \cdot m o l \cdot {L}^{-} 1$
$\text{Moles of NaOH}$ $=$ $0.1000 \cdot m o l \cdot {L}^{-} 1 \times 20.76 \times {10}^{-} 3 L = 2.076 \times {10}^{-} 3 \cdot m o l$
$\text{Concentration of malonic acid}$ $=$ $\frac{\frac{1}{2} \times 2.076 \times {10}^{-} 3 \cdot m o l}{13.15 \times {10}^{-} 3 \cdot L}$ $=$ ??mol*L^-1
Note that I had to use $\frac{1}{2} \times 2.076 \times {10}^{-} 3 \cdot m o l \text{ with respect to malonic acid}$ as malonic acid is a diacid, $H O \left(O = C\right) C {H}_{2} C \left(= O\right) O H$.