QuestionMay 9, 2025

1. If a solution has a H^+ concentration of 3.4times 10^-5 what is its pH? 2. What is the pOH in the above solution?

1. If a solution has a H^+ concentration of 3.4times 10^-5 what is its pH? 2. What is the pOH in the above solution?
1. If a solution has a H^+ concentration of 3.4times 10^-5 what is its pH? 2. What is the pOH in the above solution?

Solution
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Answer

pH = 4.469 ### pOH = 9.531 Explanation 1. Calculate pH Use the formula pH = -\log[H^+]. Substitute [H^+] = 3.4 \times 10^{-5} into the formula: pH = -\log(3.4 \times 10^{-5}) = -( \log(3.4) + \log(10^{-5})). \log(3.4) \approx 0.531, and \log(10^{-5}) = -5. Thus, pH = -(0.531 - 5) = 4.469. 2. Calculate pOH Use the relationship pH + pOH = 14. Rearrange to find pOH: pOH = 14 - pH = 14 - 4.469 = 9.531.

Explanation

1. Calculate pH<br /> Use the formula $pH = -\log[H^+]$. Substitute $[H^+] = 3.4 \times 10^{-5}$ into the formula: <br />$pH = -\log(3.4 \times 10^{-5}) = -( \log(3.4) + \log(10^{-5}))$. <br />$\log(3.4) \approx 0.531$, and $\log(10^{-5}) = -5$. <br />Thus, $pH = -(0.531 - 5) = 4.469$.<br /><br />2. Calculate pOH<br /> Use the relationship $pH + pOH = 14$. Rearrange to find $pOH$: <br />$pOH = 14 - pH = 14 - 4.469 = 9.531$.
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