Question

H+ ions increase in concentration at lower pH values. Calculate how many more H+ ions there are in a solution at a pH = 2 than in a solution at a pH = 6. Find the concentration of H+ ions at a pH = 2 and at a pH = 6 in Table B. Then divide the concentration of H+ ions at a
pH = 2 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 = 2?


mol/L

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


mol/L

How many more H+ ions are there in a solution at a
pH = 2 than in a solution at a pH = 6?


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Answer 1

The H⁺ ion concentration can be calculated from pH values using the following equation:

$pH=-log[H⁺]$

1.) Given pH = 2

Using the above equation, 2 = - log [H⁺]

Therefore, [H⁺] = 10⁻² mol/L

2.) Given pH = 6

Using the same equation, we have 6 = - log [H⁺]

Hence, [H⁺] = 10⁻⁶ mol/L

3.) Taking the ratio of [H⁺] for pH = 2 and pH = 6, we have

$\frac{10^{-2} }{10^{-6} }$ = 10⁴

So, there are 10,000 times more H⁺ ions in a solution of pH = 2 than that of pH = 6.

Answer 2

Answer:

0.01

0.000001

10,000

Explanation:

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