Question

If $100$ ml of $1M{H}_{2}S{O}_4$ solution is mixed with $100$ ml of $98\%$ $\left(w/w\right)$ $H_{2}S{O}_4$ solution $(d=0.1g/ml)$, then :

• A. the concentration of solution remains the same
• B. the volume of solution becomes $200ml$
• C. the mass of $H_{2}S{O}_4$ in the solution is $98g$
• D. the mass of $H_{2}S{O}_4$ in the solution is $19.6g$

Answer 1

Answer: (A), (B), (D)

The correct options are
A the concentration of solution remains the same
B the volume of solution becomes $200ml$
D the mass of $H_{2}S{O}_4$ in the solution is $19.6g$

(A) The concentration of second solution is $\frac{10\times d\times x}{M}=1M$. It is same as that of the first solution. Thus, on mixing two solutions, the concentration of the solution remains same.

(B) Total volume of the solution after mixing $=100+100=200ml$.

(D) Mass of sulfuric acid in the solution $=\frac{200\times 1}{1000}\times 98=19.6g$.