The $pH$ of neutral water at room temperature is nearly:

The $pH$ of $1 \ N \ H_2O$ is

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

When a large amount of water is added to a solution of $BiCl_3$,then........

$2$. Given below are two statements:
Statement $I$: The changes in $pH$ with temperature are so small that we often ignore them.
Statement $II$: When the hydrogen ion concentration changes by a factor of $100$,the $pH$ changes by one unit.
In the light of the above statements,identify the correct answer from the options given below:

What is the $pH$ of a solution containing $2.2 \times 10^{-6} \ M$ hydrogen ions?