The concentration of `H_(3)O^(+)` ions in solution A is 1000 times than that in solution B. what is the difference between the values of pH of these two solutions?

Explanation

Given: `[H_(3)O^(+)]_(A)=1000xx[H_(3)O^(+)]_(B)`, where `[H_(3)O^(+)}_(A)` and `[H_(3)O^+]_(B)` are the concentration of `H_(3)O^(+)` ions in solutions A and B respectively.
Therefore, pH (solution A)
`=-log_(10)[H_(3)O^(+)]_(A)=-log(10^(3)xx[H_(3)O^(+)]_(B))`
`=-3-log_(10)[H_(3)O^(+)]_(B)=-3+pH` of solution B
`therefore pH ("solution B")-pH("solution A")=3`.