The pH of a solution is 10. What is its $[H^{+}]$ $[H^+]$ concentration?

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Answer 1 · 2017-08-15T06:41:28

$[H^{+}] / [H_{3} O^{+}] = 10^{- 10} \cdot m o l \cdot L^{- 1}$ $[H^+]"/"[H_3O^+]=10^(-10)*mol*L^-1$

By definition, $p H = - {log}_{10} [H^{+}]$ $pH=-log_10[H^+]$ .

In water, under standard conditions, $p H$ $pH$ characterizes the autoprotolysis reaction.......

$2 H_{2} O ⇌ H_{3} O^{+} + H O^{-}$ $2H_2OrightleftharpoonsH_3O^+ + HO^-$

$K_{w} = [H O^{-}] [H_{3} O^{+}] = 10^{- 14}$ $K_w=[HO^-][H_3O^+]=10^-14$ , we take ${log}_{10}$ $log_10$ of BOTH SIDES...

${log}_{10} K_{w} = {log}_{10} [H O^{-}] + {log}_{10} [H_{3} O^{+}]$ $log_10K_w=log_10[HO^-]+log_10[H_3O^+]$

And on rearrangement,

$underbrace(-log_10(10^-14))_(pK_w)=underbrace(-log_10[HO^-])_(pOH)underbrace(-log_10[H_3O^+])_(pH)$

And thus $14=pOH+pH$ .

The pH of a solution is 10. What is its [H^+][H+][H^+] concentration?