The $\mathrm{pH}$ of a $0.72 \mathrm{M}$ solution of $\mathrm{HF}$ is....
3.60
1.81
12.19
0.14
.02

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***B*** ∻Key Concept∻ ⚹Weak Acid Ionization and pH Calculation⚹ ∻Explanation∻ ⚹Hydrofluoric acid (HF) is a weak acid that partially dissociates in water. To find the pH of a weak acid solution, we use the acid dissociation constant (Ka) and the initial concentration to solve for the concentration of hydrogen ions ($[H^+]$). The pH is then calculated using the formula $pH = -\log[H^+]$. Given that the Ka of HF is $6.8 imes 10^{-4}$, we can set up an ICE table to solve for $[H^+]$ and then calculate the pH, which should be around 1.81 for a 0.72 M HF solution.⚹◊What is the formula to calculate the pH of a solution of HF?⍭ Generate me a similar question◊

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