calculate the $\mathrm{pH}$ of a solution that is $0.050 \mathrm{M}$ in formic acid and $0.10 \mathrm{M}$ in sodium formate

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∻Solution∻ ‖ 1 ⋮ **Use the Henderson-Hasselbalch equation**: To find the pH of the buffer solution, we apply the Henderson-Hasselbalch equation, which is given by $ ext{pH} = ext{pKa} + \log\left(\frac{[ ext{A}^-]}{[ ext{HA}]} ight)$, where $ ext{pKa}$ is the acid dissociation constant of the weak acid, $[ ext{A}^-]$ is the concentration of the conjugate base, and $[ ext{HA}]$ is the concentration of the weak acid. ‖ ‖ 2 ⋮ **Calculate the pH**: The pKa of formic acid is approximately 3.75. Using the concentrations given, $[ ext{A}^-] = 0.10\ ext{M}$ and $[ ext{HA}] = 0.050\ ext{M}$. Plugging these values into the Henderson-Hasselbalch equation gives $ ext{pH} = 3.75 + \log\left(\frac{0.10}{0.050} ight) = 3.75 + \log(2) = 3.75 + 0.3010 = 4.0510$. ‖ ∻Answer∻ ⚹ The pH of the solution is 4.0510 ⚹ ∻Key Concept∻ ⚹ Henderson-Hasselbalch equation ⚹ ∻Explanation∻ ⚹ The Henderson-Hasselbalch equation is used to calculate the pH of a buffer solution based on the concentrations of the acid and its conjugate base. ⚹◊What is the relationship between the concentrations of formic acid and sodium formate in determining the pH of the solution⍭ Generate me a similar question◊

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