mg of pure was used to make an aqueous solution. 25.0 mL of 0.1 M solution is used when the solution was titrated against it. The numerical value of is __________ (Nearest integer). Given: Molar mass of and are 36.5 and respectively.

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Solution

Q.
$x$ mg of pure $HCl$ was used to make an aqueous solution. 25.0 mL of 0.1 M $Ba {(OH)}_{2}$ solution is used when the $HCl$ solution was titrated against it. The numerical value of $x$ is __________ $\times 10^{- 1}$ (Nearest integer).

Given: Molar mass of $HCl$ and $Ba {(OH)}_{2}$ are 36.5 and $171.0 {g mol}^{- 1}$ respectively. [2026]

Ans.
(1825)

$Ba {(OH)}_{2 (aq)} + 2 {HCl}_{(aq)} \to {BaCl}_{2 (aq)} + 2 H_{2} O_{(l)}$

$2.5 mmole 5 mmole$

$wt of HCl = 5 \times 36.5 (milligram)$

$= 182.5 (milligram)$

$Hence x = 1825 .$

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