S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Some Basic Concepts of Chemistry, Exercise 4: PROBLEMS FOR PRACTICE

When $4.2$ gram of $\mathrm{NaHCO}$₃ is added to a solution of acetic acid weighing $10.0$ grams. It is observed that $2.2$ grams of $\mathrm{CO}$₂ is released into atmosphere. The residue left behind is found to weigh $12$ grams. Show that these observations are in agreement with law of conservation of mass.

If $6.3 \mathrm{g}$ of ${\mathrm{NaHCO}}_3$ are added to $15.0 \mathrm{g}$ of ${\mathrm{CH}}_3\mathrm{COOH}$ solution, the residue is found to weigh $18.0 \mathrm{g}$. What is the mass of ${\mathrm{CO}}_2$ released in the reaction?

$2.16$ g of copper metal when treated with nitric acid following by ignition of the nitrate gave$2.70$ g of copper oxide. In another experiment $1.15$ g of copper oxide upon reduction with hydrogen gave $0.92$ g of copper. Show that the above data illustrate the law of Definite proportions.