Question

Sodium carbonate (2.4134 g) is dissolved in enough deionized water to give a solution with a total volume of 250.0 mL. What is the pH of the resulting solution? Hint: For carbonic acid, pKa1 = 6.351 and pKa2 = 10.329. What is the equilibrium concentration of H2CO3 in the solution? calculate the value of alpha HCO3-. I already have the answer to the first part of the question. I just need the equilibrium concentration and value of alpha please!

Answer #1

Sodium carbonate (2.4134 g) is dissolved in enough deionized
water to give a solution with a total volume of 250.0 mL. What is
the pH of the resulting solution? For carbonic acid, pKa1 = 6.351
and pKa2 = 10.329.
Also:
What is the equilibrium concentration of H2CO3 in the
solution
calculate the value of aHCO3−.
Write a mass balance and charge balance equation
please show all work!

Give a recipe for preparing a carbonate/bicarbonate
buffer solution having a pH of 7.5.
For carbonic acid, H2CO3, pKa1 = 6.37 and
pKa2 = 10.25.

A weak acid H3A has pKa values of 1.95 (pKa1), 3.08
(pKa2), and 9.54 (pKa3). The disodium salt of
that weak acid was dissolved in deionized water to make 250.0 mL of
a 0.025 M solution. a) What was the pH of the resulting
solution? b)What was the equilibrium concentration of H2A-?

100 mg of H2CO3 are dissolved in 700 mL of
water. A lab assistant measured the resulting pH= 4.9. Determine
the molar concentration of H2CO3,
HCO3- and CO32-in the
solution.

A
saturated sodium carbonate solution at 100 degrees celsius contains
45.5 g of dissolved sodium carbonate per 100. mL of solution. The
solubility product constant for sodium carbonate at this temp is
79.0
0.316
0.0790
36.8
316.

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Calculate the Ka for the acid.

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Calculate the Ka for the acid.

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Calculate the Ka for the acid.

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Calculate the Ka for the acid.

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