A sulphuric acid solution has $pH=3$. Its normality is:

Q. $0.02M$ solution of $H_{2}A$ has $pH=4$. If $K_{a_1}$ for the acid is $5\times {10}^{-7}M$, the concentration of $H{A}^{-}$ ion in the solution would be :

Q. Calculate the accurate pH of $5\times {10}^{-3}M$ formic acid solution.
$K_a\left(HCOOH\right)=2\times {10}^{-4}$

Q. Consider a strong acid HA having a pH=4 mixed in an equal volume with another solution of strong acid HB to give a resultant pH of 3. Then the $H^{+}$ concentration of solution containing strong acid HB is :

Q. Calculate the molar concentration of a solution of acetic acid (HOAc) that has a pH of $4.00(K_a=1.8\times {10}^{-5})$

Q. Calculate pH of a solution which is ${10}^{-1}M$ in HCl & ${10}^{-3}M$ in $C{H}_{3}COOH[K_a=2\times {10}^{-5}]$. Also calculate $\left[H^{+}\right]$ From $C{H}_{3}COOH.$