Question

Calculate the number of $H^{+}$ ions present in $1mL$ of a solution whose pH is $10$.

Answer 1

Given, $pH=10$

$\left[H^{+}\right]=1\times {10}^{-10}mol/L$

$\because$ Number of $H^{+}$ ions in $1L$ of solution $=6.023\times {10}^{23}\times 1\times {10}^{-10}$
$=6.023\times {10}^{13}$

$\therefore$ Number of $H^{+}$ ions in $1mL$ of solution $=6.023\times {10}^{13}\times {10}^{-3}$
$=6.023\times {10}^{10}$