Multiple choice

If equal volumes of $0.1M$ $HBr$ and $0.1M$ $KOH$ are mixed then which of the following is/are correct about the resulting solution? (1) $\left[ { H }_{ 3 }{ O }^{ + } \right] =1.0{ \times 10 }^{ -7 }mol\quad { L }^{ -1 }$ (2) $\left[ { OH }^{ - } \right] ={ 1.0\times 10 }^{ -7 }mol\quad { L }^{ -1 }$ (3) $\left[ { K }^{ + } \right] =0.05mol\quad { L }^{ -1 }$ (4) $\left[ { Br }^{ - } \right] =1.0mol\quad { L }^{ -1 }$

  1. 1, 2 and 3 are correct

  2. 1 and 2 are correct

  3. 2 and 4 are correct

  4. 1 and 3 are correct
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A Correct answer
Explanation

Mixing equal volumes of 0.1M HBr and 0.1M KOH results in a complete neutralization reaction, forming 0.05M KBr in the final solution. The concentrations of H3O+ and OH- are both 10^-7 M due to the auto-ionization of water, and [K+] is 0.05 M. Statement 4 is incorrect because [Br-] is 0.05 M, not 1.0 M.

AI explanation

Mixing equal volumes of 0.1M HBr and 0.1M KOH causes a neutralization reaction between the strong acid and strong base. The resulting salt solution is perfectly neutral, giving hydronium and hydroxide ion concentrations of 1.0 x 10^-7 mol per liter. The concentration of K+ and Br- ions halves to 0.05 mol per liter due to the doubling of the total volume. Statements 1, 2, and 3 are correct.

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