1.25 g of a solid dibasic acid is completely | vedclass

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(D) The reaction between a dibasic acid $(H_2A)$ and barium hydroxide $(Ba(OH)_2)$ is: $H_2A + Ba(OH)_2 \rightarrow BaA + 2H_2O$.From the stoichiometr

Vedclass · Accepted Answer

$200$

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(D) The reaction between a dibasic acid $(H_2A)$ and barium hydroxide $(Ba(OH)_2)$ is: $H_2A + Ba(OH)_2 ightarrow BaA + 2H_2O$.From the stoichiometry,$1 	ext{ mole}$ of $Ba(OH)_2$ reacts with $1 	ext{ mole}$ of dibasic acid.Number of moles of $Ba(OH)_2 = 	ext{Molarity} 	imes 	ext{Volume (in L)} = 0.25 \ M 	imes 0.025 \ L = 0.00625 \ mol$.Since the acid is dibasic,the number of moles of acid is also $0.00625 \ mol$.Molecular mass of acid $= \frac{	ext{Mass}}{	ext{Moles}} = \frac{1.25 \ g}{0.00625 \ mol} = 200 \ g/mol$.

$1.25 \ g$ of a solid dibasic acid is completely neutralized by $25 \ mL$ of $0.25 \ M$ $Ba(OH)_2$ solution. The molecular mass of the acid is:

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