AP EAMCET · Chemistry · Ionic Equilibrium
At \(27^{\circ} \mathrm{C} .100 \mathrm{~mL}\) of 0.4 M HCl is mixed with 100 mL of 0.5 M NaOH solution. To the resultant solution. 800 mL of distilled water is added. What is the pH of final solution?
- A \(12\)
- B \(2\)
- C \(1.3\)
- D \(1.0\)
Answer & Solution
Correct Answer
(A) \(12\)
Step-by-step Solution
Detailed explanation
Moles of \(\mathrm{HCl}=0.4 \mathrm{~m} \times 0.1 \mathrm{~L}=0.04\) moles For \(\mathrm{NaOH}:-\) Moles of \(\mathrm{NaOH}=0.5 \mathrm{M} \times 0.1 \mathrm{~L}=0.05\) moles HCl and NaOH react in \(1: 1\) Ratio…
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