Questions: If a sample of a certain solution is determined to have a [H3O+] concentration of 6.69 × 10^-13 moles/liter, what is its pH? Round off your answer to one decimal place.

If a sample of a certain solution is determined to have a [H3O+] concentration of 6.69 × 10^-13 moles/liter, what is its pH? Round off your answer to one decimal place.
Transcript text: If a sample of a certain solution is determined to have a $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$concentration of $6.69 \times 10^{-13}$ moles/liter, what is its pH? Round off your answer to one decimal place.
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Solution

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Solution Steps

Step 1: Understanding the pH Formula

The pH of a solution is calculated using the formula: \[ \text{pH} = -\log_{10} \left[\mathrm{H}_3\mathrm{O}^+\right] \] where \([\mathrm{H}_3\mathrm{O}^+]\) is the concentration of hydronium ions in moles per liter.

Step 2: Applying the Formula

Given the concentration of hydronium ions is \(6.69 \times 10^{-13}\) moles/liter, we substitute this value into the pH formula: \[ \text{pH} = -\log_{10} (6.69 \times 10^{-13}) \]

Step 3: Calculating the pH

Using a calculator, compute the logarithm: \[ \text{pH} = -\log_{10} (6.69 \times 10^{-13}) \approx 12.2 \]

Final Answer

The pH of the solution is \(\boxed{12.2}\).

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