We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.44. We titrate this solution with a 0.250 M NaOH solution and we need 33.3 mL of this 0.250 M NaOH solution to reach the equivalence point. The temperature is 25.0 ◦C throughout. (a) What is the molar mass of HA? (b) What is the dissociation constant, Kb, of A−(aq)? (c) What would be the pH of a 2.222 M solution of A−(aq)?
We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.44. We titrate this solution with a 0.250 M NaOH solution and we need 33.3 mL of this 0.250 M NaOH solution to reach the equivalence point. The temperature is 25.0 ◦C throughout. (a) What is the molar mass of HA? (b) What is the dissociation constant, Kb, of A−(aq)? (c) What would be the pH of a 2.222 M solution of A−(aq)?
General, Organic, and Biological Chemistry
7th Edition
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:H. Stephen Stoker
Chapter10: Acids, Bases, And Salts
Section: Chapter Questions
Problem 10.118EP: Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer...
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We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of
this solution is 1.44. We titrate this solution with a 0.250 M NaOH solution and we need 33.3 mL of this
0.250 M NaOH solution to reach the equivalence point. The temperature is 25.0 ◦C throughout.
(a) What is the molar mass of HA?
(b) What is the dissociation constant, Kb, of A−(aq)?
(c) What would be the pH of a 2.222 M solution of A−(aq)?
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