A) If \[2.0\]litre of a solution of \[{{H}_{2}}S{{O}_{4}}\] contains \[0.1\]mole, then pH of the solution is 2
B) The concentration of \[O{{H}^{-}}\] in \[0.005M\]\[HN{{O}_{3}}\] is \[2.0\times {{10}^{-12}}mol/l\]
C) The pH of \[0.01M\] \[KOH\] is 12
D) In a \[0.001\text{ }M\]solution of \[NaOH\] the concentration of \[{{H}^{+}}\] is \[{{10}^{-3}}mol/litre\]
Correct Answer: D
Solution :
In \[0.001M\text{ }NaOH,\] \[[O{{H}^{-}}]=0.001={{10}^{-3}}\] \[\therefore \] \[[{{H}^{+}}]=\frac{{{10}^{-14}}}{[O{{H}^{-}}]}=\frac{{{10}^{-14}}}{{{10}^{-3}}}={{10}^{-11}}\] Hence, is incorrect.
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