A0.450 g sample of impure caco3(s) is dissolved in 50.0 ml of 0.150 m hcl ( aq ) . the equation for the reaction is caco3 ( s ) + 2 hcl ( aq ) ⟶ cacl2 ( aq ) + h2o ( l ) + co2 ( g ) the excess hcl ( aq ) is titrated by 5.35 ml of 0.125 m naoh ( aq ) . calculate the mass percentage of caco3(s) in the sample.

The mass percentage of CaCO3(s) in the sample is 83.4%

Explanation:

CaCO₃ + 2HCl  →  CaCl₂  +  H2O  +  CO₂

Let's find out the moles of each reactant:

[HCl] = 0.150 mol/L

Molarity . volume = moles

0.150 m/L . 0.050L = 7.5x10⁻³ moles HCl

Molar mass of CaCO₃ =100.08 g

Moles of CaCO₃ = Mass / Molar mass

0.450 g/100.08 g = 4.49x10⁻³ moles of salt

Ratio is 1:2

If 2 moles of HCl react with 1 mol of salt

7.5x10⁻³ moles of HCl react with 7.5x10⁻³ / 2 = 3.75x10⁻³ moles

We must find out the mass

Moles of CaCO₃ . Molar mass CO₃ = 0.3753 g

So now, the mass percentage of salt will be

0.450g ___ 100%

0.3753 g (0.3753 .100 )/0.450 =83.4 %

idk

explanation:

i need the pts ignore this answer

your answer is c

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