OnlineCBT
Chemistry · EQUILIBRIUM
हिन्दीEqual volumes of two strong acid solutions with \( \text{pH} = 2.0 \) and \( \text{pH} = 4.0 \) are mixed together at \( 298\text{ K} \). What is the \( \text{pH} \) of the resulting mixture? (Given: \( \log 5.05 \approx 0.70 \))
View Answer & Solution
Correct answer · Option A
2.30
Explanation
\( [\text{H}^+]_1 = 10^{-2}\text{ M} \), \( [\text{H}^+]_2 = 10^{-4}\text{ M} \). For equal volumes \( V \), \( [\text{H}^+]_{\text{mix}} = \frac{10^{-2} + 10^{-4}}{2} = 5.05 \times 10^{-3}\text{ M} \). Thus, \( \text{pH} = 3 - \log 5.05 = 3 - 0.70 = 2.30 \).
