The $pH$ of a $0.005 \ M \ H_2SO_4$ solution will be:

What is the $pH$ of the $NaOH$ solution when $0.04 \ g$ of it is dissolved in water to make a $100 \ mL$ solution?

Calculate the $pOH$ of a $0.01 \text{ M}$ monobasic acid solution that is completely dissociated at $298 \text{ K}$.

When equal volumes of solutions with $pH = 6$ and $pH = 3$ are mixed,what is the $pH$ of the resulting solution?

Assuming complete ionisation,the $pH$ of $0.1\,M\,HCl$ is $1$. The molarity of $H_2SO_4$ with the same $pH$ is (in $,M$)

At $27^{\circ} C$, $100 \ mL$ of $0.5 \ M$ $HCl$ is mixed with $100 \ mL$ of $0.4 \ M$ $NaOH$ solution. To this resultant solution, $800 \ mL$ of distilled water is added. What is the $pH$ of the final solution?