Question

Find the concentration of H+ ions at a pH = 11 and pH = 6. Then divide the concentration of H+ ions at a pH = 11 by the of H+ ions at a pH = 6. Record your answer in Table C. What is the concentration of H+ ions at a pH = 11? mol/L What is the concentration of H+ ions at a pH = 6? mol/L How many fewer H+ ions are there in a solution at a pH = 11 than in a solution at a pH = 6?

Answer 1

Answer:

0.00000000001

0.000001

100,000

Explanation:

Answer 2

Explanation:

When pH of the solution is 11.

$pH=-\log[H^+]$

$11=-\log[H^+]$

$[H^+]=1\times 10^{-11} M$..(1)

At pH = 11, the concentration of $H^+$ ions is $1\times 10^{-11} M$.

When the pH of the solution is 6.

$pH=-\log[H^+]'$

$6=-\log[H^+]'$

$[H^+]'=1\times 10^{-6} M$..(2)

At pH = 6, the concentration of $H^+$ ions is $1\times 10^{-6} M$.

On dividing (1) by (2).

$\frac{[H^+]}{[H^+]'}=\frac{1\times 10^{-11} M}{1\times 10^{-6}}=1\times 10^{-5}$

The ratio of hydrogen ions in solution of pH equal to 11 to the solution of pH equal to 6 is $1\times 10^{-5}$.

Difference between the $H^+$ ions at both pH:

$1\times 10^{-6} M-1\times 10^{-11} M=9.99\time 10^{-7} M$

This means that Hydrogen ions in a solution at pH = 7 has $9.99\time 10^{-7} M$ ions fewer than in a solution at a pH = 6