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TS EAMCET · Chemistry · Ionic Equilibrium

\(75 \mathrm{~mL}\) of \(0.2 \mathrm{M} \mathrm{HCl}\) is mixed with \(25 \mathrm{~mL}\) of \(1 \mathrm{M}\) \(\mathrm{HCl}\). To this solution, \(300 \mathrm{~mL}\) of distilled water is added. What is the \(\mathrm{pH}\) of the resultant solution?

  1. A \(1\)
  2. B \(2\)
  3. C \(4\)
  4. D \(0.2\)
Verified Solution

Answer & Solution

Correct Answer

(A) \(1\)

Step-by-step Solution

Detailed explanation

\begin{aligned} V_1 & =75 \mathrm{~mL}, V_2=25 \mathrm{~mL} \\ M_1 & =0.2 \mathrm{M}, M_2=1 \mathrm{M} \\ V_3 & =300 \mathrm{~mL}, \mathrm{pH}=? \\ V & =V_1+V_2=75+25=100 \mathrm{~mL} \\ M & =\frac{V_1 M_1+V_2 M_2}{V_1+V_2}=\frac{75 \times 0.2 \times 25+1}{75+25}=0.4 \mathrm{M}…