Mathematics: What is the pH of a buffer that is 0.6 M HF and 0.2 M NaF? The Ka of HF is 6.8 Ã 10â4. What is the pH of a buffer that is: a. 3.65b. 3.17c. 3.50d. 2.69

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What is the pH of a buffer that is 0.6 M HF and 0.2

polo1397

08.02.2022

The correct option is d

Step-by-step explanation:

From the question we are told that

The concentration of HF is [HF] = 0.6 M

The concentration of NaF is [NaF ] = 0.2 M

The Ka of HF is $K_a = 6.8 *10^{-4} \$

Generally HF(Hydrogen fluoride ) is ionized as follows

$HF_{(aq)} + H_2 O _{(l)} \rightleftharpoons H_3O^+ _{(aq) } + F^- _{(aq)}$

Generally NaF(Sodium fluoride ) is ionized as follows

$NaF_{(aq)} + H_2 O _{(l)} \rightleftharpoons Na^+ _{(aq) } + F^- _{(aq)}$

Generally the from Henderson-Hasselbalch equation the pH of the buffer is mathematically represented as

$pH = pKa + log [\frac{[NaF ]}{HF} ]$

=> $pH = -log(K_a) + log [\frac{[NaF ]}{HF} ]$

=> $pH = -log(6.8 *10^{-4}) + log [\frac{[0.2 ]}{0.6} ]$

=> pH = 2.69

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