Question

100 mL of a 0.2 M $H_{2}S{O}_4$ solution, 200 mL of a 0.1 M $HN{O}_3$ solution and 300 mL of a 0.2 M NaOH solution are mixed. The resultant solution will be

• A. Acidic
• B. Basic
• C. Neutral
• D. Can't say

Answer 1

The correct option is C Neutral

Milliequivalents of $H_{2}S{O}_4=100\times 0.2\times 2=40$
Milliequivalents of $HN{O}_3=200\times 0.1\times 1=20$
Total milliequivalents of the acid = 40 + 20 = 60
Milliequivalents of $NaOH=300\times 0.2\times 1=60$
Milliequivalents of the base = milliequivalents of acid
Hence, the resultant solution will be neutral.