The acidity of a solution is measured by its pH .
If represents the concentration of hydrogen ions (in moles/liter) in the solution,
the pH is defined by
Based on careful measurements and calculations, a chemist examines two solutions and asserts:
“The hydrogen ion concentration of Solution A
is 6.22 times greater than
the hydrogen ion concentration of Solution B.”
If the pH of solution B is 3.3 , determine the pH of Solution A.
Report your answer to one decimal place.
Solution A has pH equal to Number

Ask by Fitzgerald Lawson. in the United States

Mar 20,2025

Question

The acidity of a solution is measured by its pH .
If represents the concentration of hydrogen ions (in moles/liter) in the solution,
the pH is defined by
Based on careful measurements and calculations, a chemist examines two solutions and asserts:
“The hydrogen ion concentration of Solution A
is 6.22 times greater than
the hydrogen ion concentration of Solution B.”
If the pH of solution B is 3.3 , determine the pH of Solution A.
Report your answer to one decimal place.
Solution A has pH equal to Number

Ask by Fitzgerald Lawson. in the United States

Mar 20,2025

UpStudy AI · Accepted Answer

Given that the pH of Solution B is 3.3, we can use the formula $$ \mathrm{pH} = -\log \left[\mathrm{H}^{+}\right] $$ to find the concentration of hydrogen ions in Solution B.

Let's denote the concentration of hydrogen ions in Solution B as $$ \left[\mathrm{H}^{+}\right]_{B} $$. We have:
$$ \mathrm{pH}_{B} = -\log \left[\mathrm{H}^{+}\right]_{B} $$
$$ 3.3 = -\log \left[\mathrm{H}^{+}\right]_{B} $$

To find the concentration of hydrogen ions in Solution B, we can rearrange the equation:
$$ \left[\mathrm{H}^{+}\right]_{B} = 10^{-3.3} $$

Now, we are given that the hydrogen ion concentration of Solution A is 6.22 times greater than the hydrogen ion concentration of Solution B. Let's denote the concentration of hydrogen ions in Solution A as $$ \left[\mathrm{H}^{+}\right]_{A} $$. We have:
$$ \left[\mathrm{H}^{+}\right]_{A} = 6.22 \times \left[\mathrm{H}^{+}\right]_{B} $$

Substitute the value of $$ \left[\mathrm{H}^{+}\right]_{B} $$ into the equation:
$$ \left[\mathrm{H}^{+}\right]_{A} = 6.22 \times 10^{-3.3} $$

Now, we can find the pH of Solution A using the formula $$ \mathrm{pH} = -\log \left[\mathrm{H}^{+}\right] $$:
$$ \mathrm{pH}_{A} = -\log \left(6.22 \times 10^{-3.3}\right) $$

Let's calculate the pH of Solution A.
The pH of Solution A is approximately 2.5.
The pH of Solution A is 2.5.

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