Question

Find the concentration of H+ ions at a pH = 11 and

Answer 1

Explanation:

the pH of the solution defined as negatuve logarithm of $H^+$ ion concentration.

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

1. Hydrogen ion concentration when pH of the solution is 11.

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

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

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

2. Hydrogen ion concentration when the pH of the solution is 6.

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

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

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

3. On dividing (1) by (2).

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

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

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

$1\times 10^{-6} mol/L-1\times 10^{-11} mol/L=9.99\time 10^{-7} mol/L$

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

Answer 2

Answer:

for table C

Explanation:

What is the concentration of H+ ions at a pH = 11?

1.  ⇒ 0.00000000001 mol/L  

What is the concentration of H+ ions at a pH = 6?

2.  ⇒ 0.000001 mol/L  

How many fewer H+ ions are there in a solution at a

pH = 11 than in a solution at a pH = 6?

3.  ⇒ 100,000