$10 g$ of a mixture of ${C a C O}_{3}$ and ${N a}_{2} {C O}_{3}$ on ignition suffered a loss in weight of $2.2 g$ . The mass ratio of ${C a C O}_{3}$ and ${N a}_{2} {C O}_{3}$ is

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1.4:1

1.75:1

1:1.4

1:1

answer is A.

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Detailed Solution

Let the weight of ${C a C O}_{3}$ be x g

So, weight of ${N a}_{2} {C O}_{3}$ = (10-x) g

Moles of ${C a C O}_{3} = \frac{x}{100}$

Balanced chemical reaction

${C a C O}_{3} \to C a O + {C O}_{2}$

Moles of ${C O}_{2}$ formed = $x / 100$

$\frac{x}{100} \times 44 = 2.2$

$x = 2.2 \times \frac{100}{44}$

$x = 5$

Weight of ${C a C O}_{3}$ = 5g.

Weight of ${N a}_{2} {C O}_{3}$ = 10 –5 = 5g.

So, the mass ratio of ${C a C O}_{3}$ and ${N a}_{2} {C O}_{3}$ is 1:1.

Therefore, option A is correct.

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