Question

A solution of HCl has [H+] = 0.01 M. What is the pH of this solution? Use pH=-log[H3O+]
A. –2
B. –1
C. 1
D. 2

Answer 1

Answer:

pH of solution is 2

Explanation:

HCl is a strong acid. Hence it gets completely dissociated in aqueous solution to produce $[H_{3}O^{+}]and Cl^{-}$.

Chemical equation related to dissociation of HCl is given as-

                      HCl+H_{2}O\rightarrow [H_{3}O^{+}]+Cl^{-}

pH of a solution is a tool to measure acidity. It is defined as-

                               $pH=-log[H^{+}]$

where $[H^{+}]$ represents concentration of $H^{+}$ in molarity.

In aqueous solution, all $H^{+}$ gets converted into $H_{3}O^{+}$.

Hence, in aqueous solution, $pH=-log[H_{3}O^{+}]$

Here $[H^{+}]=0.01M$. So $[H_{3}O^{+}]=0.01M$

Hence $pH=-log(0.01)=2$

Answer 2

Answer:

answer is 2

Explanation:

was right on edge