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When $KBr$ is dissolved in water,$K^{+}$ ions are

At $90\,^{\circ}C$ pure water has $[H_3O^{+}] = 10^{-6}\,M$. The value of $K_w$ at this temperature will be:

The hydrogen ion concentration of a solution is $3.98 \times 10^{-6} \text{ mole per liter}$. The $pH$ value of this solution will be

What is the $pH$ of the solution containing $1.342 \times 10^{-3} \ M \ H^{+}$ ions?
$(\log 1.342 = 0.1277)$

$A$ beer has a $pH$ of $4.30$. What is the $[H_3O^{+}]$ concentration?

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