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18 Nov 2019

3.)a.)Calculate the pH of an aqueous solution of 0.1840 M sodium carbonate.pH =

b.)Calculate the pH of an aqueous solution of 0.1020 M potassium carbonate.pH = .

c.)The pH of an aqueous solution of 0.0631 M sodium hydrogen sulfite, NaHSO3 would be _________(greater than, equal to, or less than seven.)

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Sixta Kovacek
Sixta KovacekLv2
27 Feb 2019

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Related questions

1.Determine the pH (to two decimal places) of a solution prepared by adding 51.3 mL of 0.0915 M sodium hydrogen sulfite (NaHSO3) to 39.4 g of sodium sulfite (Na2SO3). Assume the volume of the solution does not change and that the 5% approximation is valid.

2.Calculate the pH (to two decimal places) of the buffer solution after the addition of 1.15 g of sodium butanoate (NaC3H7COO) to the buffer solution above.
Assume 5% approximation is valid and that the volume of solution does not change.

3. The mole fraction of an aqueous solution of ammonium nitrite is 0.494. Calculate the molarity (in mol/L) of the ammonium nitrite solution, if the density of the solution is 1.45 g mL-1.

4. Determine the mole fraction of calcium nitrite in a 9.28 M aqueous solution of calcium nitrite. The density of the solution is 1.47 g mL-1.

Please answer the following 4 questions. Will upvote

a) A buffer solution contains 0.455 M NaHSO3 and 0.254 M K2SO3. Determine the pH change when 0.096 mol NaOH is added to 1.00 L of the buffer.

pH after addition − pH before addition = pH change = ___________

b) Determine the pH change when 0.131 mol KOH is added to 1.00 L of a buffer solution that is 0.460 M in CH3COOH and 0.280 M in CH3COO-.

pH after addition − pH before addition = pH change = ___________

c) When a 25.0 mL sample of a 0.369 M aqueous acetic acid solution is titrated with a 0.311 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration?
pH = _________

d) A 17.3 mL sample of a 0.427 M aqueous hypochlorous acid solution is titrated with a 0.441 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added?

pH = __________

1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid?

pOH =


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pOH =

4. What is the pH of an aqueous solution of 3.08×10-2 M potassium hydroxide?

pH =

5. Calculate the pH of a 0.409 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

6. Calculate the pH of a 0.0130 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4).

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9. Calculate the percent ionization of a 0.347 M solution of formic acid, HCOOH.

% Ionization=

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