What will happen to the pH of a substance if the concentration of hydrogen $[H^{+}]$ $[H^+]$ ions increases from $1.0 \times 10^{- 8}$ $1.0 times 10^-8$ to $1.0 \times 10^{- 6}$ $1.0 times 10^-6$ ?

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Answer 1 · 2017-04-17T16:43:36

It will decrease by $2$ $2$ .

The $pH$ $"pH"$ of solution is defined as - $log ([H^{+}])$ $log(["H"^+])$ .

For $[H^{+}] = 10^{- 8},$ $["H"^+]=10^-8,$ $pH = 8$ $"pH"=8$

For $[H^{+}] = 10^{- 6},$ $["H"^+]=10^-6,$ $pH = 6$ $"pH"=6$

What will happen to the pH of a substance if the concentration of hydrogen [H^+][H+][H^+] ions increases from 1.0 times 10^-81.0×10−81.0 times 10^-8 to 1.0 times 10^-61.0×10−61.0 times 10^-6?