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 is 2

Step-by-step explanation:

was right on edge

Answer 2

pH of solution is 2

Step-by-step 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`