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A 0.558 g sample of a diprotic acid with a molar mass of 255.8 g>mol is dissolved in
Chapter 16, Problem 140(choose chapter or problem)
A 0.558 g sample of a diprotic acid with a molar mass of 255.8 g/mol is dissolved in water to a total volume of 25.0 mL. The solution is then titrated with a saturated calcium hydroxide solution.
a. Assuming that the \(\mathrm{p} K_{\mathrm{a}}\) values for each ionization step are sufficiently different to see two equivalence points, determine the volume of added base for the first and second equivalence points.
b. The pH after adding 25.0 mL of the base is 3.82. Find the value of \(K_{\mathrm{a}_{1}}\).
c. The pH after adding 20.0 mL past the first equivalence point is 8.25. Find the value of \(K_{\mathrm{a}_{2}}\).
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QUESTION:
A 0.558 g sample of a diprotic acid with a molar mass of 255.8 g/mol is dissolved in water to a total volume of 25.0 mL. The solution is then titrated with a saturated calcium hydroxide solution.
a. Assuming that the \(\mathrm{p} K_{\mathrm{a}}\) values for each ionization step are sufficiently different to see two equivalence points, determine the volume of added base for the first and second equivalence points.
b. The pH after adding 25.0 mL of the base is 3.82. Find the value of \(K_{\mathrm{a}_{1}}\).
c. The pH after adding 20.0 mL past the first equivalence point is 8.25. Find the value of \(K_{\mathrm{a}_{2}}\).
ANSWER:Step 1 of 5
Calculate the number of moles of the acid. Multiply the grams of the sample with the molar mass:
\(0.558 \mathrm{~g} \text { acid } \times \frac{1 \mathrm{~mol} \mathrm{acid}}{255.8 \mathrm{~g} \text { acid }}=2.18 \times 10^{-3} \text { molacid }\)
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