The $pH$ of $0.1 \ M \ NaOH$ is

Select the correct option that has the same $pH$ value.
$(1) 0.005 \, M \, H_2SO_4$
$(2) 0.1 \, M \, Na_2SO_4$
$(3) 10^{-2} \, M \, NaOH$
$(4) 0.01 \, M \, HCl$

An aqueous solution of a strong monoacidic base has a concentration of $1 \times 10^{-4} \ M$. What is the value of $pH$ at $25^{\circ} C$?

The $pH$ of a $H_2SO_4$ solution is $5.0$. If more $H_2SO_4$ is added to this solution,the $pH$ becomes $2.0$. The concentration of $H^{+}$ ions will become how many times the initial concentration?

What is the $pH$ of a $2.6 \times 10^{-8} \ M \ H^{+}$ ion solution?
$(\log 2.6 = 0.4150)$

The $pH$ of a $0.05 \,M$ solution of a strong dibasic acid $(H_2A)$ is: