Directions : In the following question more than one of the answers given may be correct. Select the correct answer and mark it according to the code:
If equal volumes of\[0.1\text{ }M\text{ }HBr\]and\[0.1\text{ }M\text{ }KOH\]are mixed, then which of the following is/are correct about the resulting solution? (1)\[[{{H}_{3}}{{O}^{+}}]=1.0\times {{10}^{-7}}mol\text{ }{{L}^{-1}}\] (2)\[[O{{H}^{-}}]=1.0\times {{10}^{-7}}mol\text{ }{{L}^{-1}}\] (3)\[[{{K}^{+}}]=0.05\text{ }mol\text{ }{{L}^{-1}}\] (4)\[[B{{r}^{-}}]\text{ }=0.10\text{ }mol\text{ }{{\text{L}}^{-1}}\]A) 1, 2 and 3 are correct
B) 1 and 2 are correct
C) 2 and 4 are correct
D) 1 and 3 are correct
Correct Answer: A
Solution :
\[HBr+KOH\xrightarrow{{}}KBr+{{H}_{2}}O;\] Volume of resulting solution will be doubled and the solution will be neutral. Hence, \[[{{K}^{+}}]=[B{{r}^{-}}]=\frac{0.1}{2}=0.05\text{ }mol\text{ }{{L}^{-1}}\] \[[{{H}_{3}}{{O}^{+}}]=[O{{H}^{-}}]={{10}^{-7}}mol\text{ }{{L}^{-1}}\]
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