If 90 g C a C O 3 is added to 300 mL of HCl which contains 38.55% HCl by mass and has density 1.13 g m L - 1 , then which of the following option is correct ? [2026]

Question

For the given reaction;

$C a C O_{3} + 2 H C l ⟶ C a C l_{2} + H_{2} O + C O_{2} $

If 90 g $C a C O_{3}$ is added to 300 mL of HCl which contains 38.55% HCl by mass and has density 1.13 g $m L^{- 1}$ , then which of the following option is correct ?

Given molar mass of H, Cl, Ca and O are 1, 35.5, 40 and 16 g $m o l^{- 1}$ respectively. [2026]

Smart Achievers · Accepted Answer

(2)

$Density of HCl solution (d) = 1.13 g/mL$

$V = 300 mL$

$Wt. of HCl solution = 339 g$

$Wt. of HCl = 339 \times \frac{38.55}{100} = 130.68 g$

$m L^{- 1}$

$Moles of HCl remained = 1.78 mole$

$Mass of HCl remained = 64.97 g$

Solution

1 97.30 g of HCl reacted

2 64.97 g of HCl remains unreacted

3 60.32 g of HCl remains unreacted

4 32.85 g of $C a C O_{3} $ remains unreacted

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Solution

Q. For the given reaction; CaCO3​+2HCl⟶CaCl2​+H2O+CO2​ If 90 g CaCO3 is added to 300 mL of HCl which contains 38.55% HCl by mass and has density 1.13 g 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 g mol-1 respectively. [2026]

1 97.30 g of HCl reacted

2 64.97 g of HCl remains unreacted

3 60.32 g of HCl remains unreacted

4 32.85 g of CaCO3​ remains unreacted

Ans. (2) Density of HCl solution (d)=1.13 g/mL V=300 mL Wt. of HCl solution=339 g Wt. of HCl=339×38.55100=130.68 g (LR)CaCO3+2HCl→CaCl2+H2O+CO290100130.6836.5=0.90 mole=3.58 mole Moles of HCl remained=1.78 mole Mass of HCl remained=64.97 g

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4 32.85 g of $C a C O_{3} $ remains unreacted