Question

Which of the solutions below will have the lowest ph? 0.10 m hbr 0.10 m hf 0.25 m hc2h3o2?

Answer 1

A.0.10 HBr

Step-by-step explanation:

We are given that some solutions

We have to find the solution which have lowest pH

1.0.10 m HBr

We know that

`p^H=-[log H^+]`

[H+]=0.10=
`1* 10^(-1)`

`pH=-[log(1* 10^(-1))]`

`Log a^b=blog a`

`pH=-(log 1-log 10)`

We know that log 1=0 abd log 10=1

Then we get

`pH=1`

HBr is strongest acid ,therefore, it completely ionize into its ions.

But HF and
`HC_2H_3O_2` are weaker acids and do not ionize completely into its ions.

The pH of these two acids are greater than one.

Hence, the pH of HBr is lowest.

Option A is true.

Answer 2

pH value of 0.10 m of HBr, a strong acid.
When dissolved in water it gives H+ and Br-, so H+ is the concentration.
pH = - log H+) => pH = - log (0.10) = -(-1) = 1
HF and HC2H3O2 are weak acids. They both will have pH value greater than 1 as they ionize in solution.