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19 Nov 2019

Prepare a solution that is 0.1M acetic acid and 0.1M sodium acetate by measuring out 5.0 ml of each and diluting to 50.0 ml with water. The Ka for acetic acid is 1.8x10^-5

What is the PH after adding 1.00 ml of 1.0 M sodium Hydroxide bringing the total volume to 51 ml

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Sixta Kovacek
Sixta KovacekLv2
19 Nov 2019

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Related questions

One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water. Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one. What accounts for the difference in the hydronium ion concentrations? Explain this based on equilibrium concepts; in other words, saying that “one solution is a buffer” is not sufficient. H3O+(aq) + C2H3O2-(aq) ⇄ HC2H3O2(aq) +H2O Ka of acetic acid = 1.8 x 10-5 Acetic acid/sodium acetate buffer: Acetic acid = 0.1M, Sodium acetate = 0.1M

Calculate the mass of solid sodium acetate required to mix with 50.0 mL of 0.120 M acetic acid to prepare a pH 4.10 buffer. The molar mass of sodium acetate is 82.03 g/mol. Ka (CH3COOH) = 1.8x10-5.

A solution is made up by combining 50 ml of a 1M acetic acid solution and 50 ml of a 1.13 M sodium acetate solution. Then, 400 ml of water is added. What is the pH of the new solution? Ka of acetic acid is 1.8x10^-5.

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