WBJEE · Chemistry · Solutions
Equal volumes of aqueous solution of \(0.1(\mathrm{M}) \mathrm{HCl}\) and \(0.2(\mathrm{M}) \mathrm{H}_2 \mathrm{SO}_4\) are mixed. The concentration of \(\mathrm{H}^{+}\)ions in the resulting solution is
- A \(0.15(\mathrm{M})\)
- B \(0.30(\mathrm{M})\)
- C \(0.10(\mathrm{M})\)
- D \(\quad 0.25(\mathrm{M})\)
Answer & Solution
Correct Answer
(D) \(\quad 0.25(\mathrm{M})\)
Step-by-step Solution
Detailed explanation
Hint : Concentration of \(\mathrm{H}^{+}\)in molarity \(=\frac{\text { Total no. of moleof } \mathrm{H}^{+}}{\text {Total volume of solution }(\mathrm{in} \mathrm{L})}=\frac{\sum \mathrm{M} \times \mathrm{V}(\mathrm{inL}) \times \text { Basicity }}{\sum \mathrm{V}}\)…
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