Question1. The pH of a $6.81 \times 10^{-2} \mathrm{M}$ solution of a weak monoprotic acid is 5.28 . Calculate the percent dissociation of the acid to 3 significant figures. \% Submit Answer Tries 0/99

Studdy Solution

STEP 1

1. The solution is of a weak monoprotic acid.
2. The concentration of the acid is $6.81 \times 10^{-2} \mathrm{M}$ .
3. The pH of the solution is 5.28.
4. We need to calculate the percent dissociation of the acid to 3 significant figures.

STEP 2

1. Calculate the concentration of hydrogen ions $[\mathrm{H}^+]$ using the pH.
2. Determine the initial concentration of the acid.
3. Calculate the percent dissociation of the acid.

STEP 3

Calculate the concentration of hydrogen ions $[\mathrm{H}^+]$ using the pH.
The formula to find the concentration of hydrogen ions from pH is: $\mathrm{pH} = -\log_{10}[\mathrm{H}^+]$
Rearrange to find $[\mathrm{H}^+]$ : $[\mathrm{H}^+] = 10^{-\mathrm{pH}}$
Substitute the given pH value: $[\mathrm{H}^+] = 10^{-5.28}$
Calculate $[\mathrm{H}^+]$ : $[\mathrm{H}^+] \approx 5.25 \times 10^{-6} \mathrm{M}$

STEP 4

Determine the initial concentration of the acid, which is given as: $[\text{Acid}]_0 = 6.81 \times 10^{-2} \mathrm{M}$

STEP 5

Calculate the percent dissociation of the acid.
Percent dissociation is given by the formula: $\text{Percent Dissociation} = \left( \frac{[\mathrm{H}^+]}{[\text{Acid}]_0} \right) \times 100\%$
Substitute the values: $\text{Percent Dissociation} = \left( \frac{5.25 \times 10^{-6}}{6.81 \times 10^{-2}} \right) \times 100\%$
Calculate the percent dissociation: $\text{Percent Dissociation} \approx 0.00771\%$
Round to 3 significant figures: $\text{Percent Dissociation} \approx 0.00771\%$

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