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

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.

Answer 2

Answer:

A.0.10 HBr

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=$1\times 10^{-1}$

$pH=-[log(1\times 10^{-1})]$

$Log a^b=blog a$

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

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.