Question
For the given reaction;
$${CaCO}_{3} + 2HCl \rightarrow {CaCl}_{2} + H_{2}O + {CO}_{2} $$If $90\text{ }g{CaCO}_{3}$ is added to 300 mL of HCl which contains $38.55\% HCl$ by mass and has density $1.13\text{ }g{\text{ }mL}^{- 1}$, then which of the following option is correct?
Given molar mass of $H,Cl,Ca$ and O are 1, 35.5, 40 and $16\text{ }g{\text{ }mol}^{- 1}$ respectively.
Options
Solution
Density of HCl solution $(d) = 1.13\text{ }g/ml$
$$V = 300ml $$Wt. of HCl solution $= 339\text{ }g$
Wt. of $HCl = 339 \times \frac{38.55}{100} = 130.68\text{ }g$
(LR)
$${{CaCO}_{3} + 2HCl \rightarrow {CaCl}_{2} + H_{2}O + {CO}_{2} }{\frac{90}{100}\ \frac{130.68}{36.5} }{= 0.90\text{ }mole\ = 3.58\text{ }mole }$$Moles of HCl remained $= 1.78$ mole.
Mass of HCl remained $= 64.97\text{ }g$.
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