Question

100 mL of a 1 M $H_{2}S{O}_4$ solution is mixed with 200 mL of a 0.5 M HCl solution and diluted to a final volume of 500 mL. 200 mL of this solution is further diluted with 300 ml of water. Find the normality of $H^{+}$ ions in the final solution.

• A. 0.51 N
• B. 0.32 N
• C. 0.24 N
• D. 0.16 N

Answer 1

The correct option is C 0.24 N

Milliequivalents of HCl $=200\times 0.5=100$
Milliequivalents of $H^{+}$= 100
Milliequivalents of $H_{2}S{O}_4=100\times 2\times 1=200$
Milliequivalents of $H^{+}$= 200
Total volume = 500 mL
Normality of $H^{+}$ $=\frac{300}{500}=0.6$ N
Now, 200 mL of this solution is diluted to 500 mL by adding 300 mL water.
$N_1{V}_1=N_2{V}_2$
$0.6\times 200=N_2\times 500$
On solving, $N_2=0.24$ N