An aqueous solution is prepared to be 0.394 M in sodium acetylsalicylate and 0.283 M in benzoic acid. (1) Is this solution a buffer solution? (2) What is the pH of this solution? pH = (3) If 0.138 moles of hydrochloric acid are added to one liter of this solution, what is the pH of the resulting solution? pH =

An aqueous solution is prepared to be 0.394 M in sodium acetylsalicylate and 0.283 M in benzoic acid. (1) Is this solution a buffer solution? (2) What is the pH of this solution? pH = (3) If 0.138 moles of hydrochloric acid are added to one liter of this solution, what is the pH of the resulting solution? pH =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 14QAP: A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to...

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A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
How many moles of sodium hydroxide would have to be added to 125 mL of a 0.301 M hypochlorous acid solution, in order to prepare a buffer with a pH of 7.440? _________________moles
a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
Explain how the pH of a mixture of aqueous ammonium chloride and aqueous ammonium remains constant when a small amount of strong base is added.Give suitable equations in your explanation.
An aqueous solution of 0.1 M hydrochloric acid with a volume of 200 milliliters is mixed with 100 mL of an aqueous solution of 0.1 M potassium hydroxide. To two digits past the decimal, what is the pH of the resulting solution once the reaction is complete?
Demonstrate an understanding of acids and bases andtheir relationship with buffers.
An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 7.260? ________mL
A buffer solution contains 0.289 M KH2PO4 and 0.399 M K2HPO4.If 0.0485 moles of hydroiodic acid are added to 250. mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume does not change upon adding hydroiodic acid)pH =
If 20.0 ml of 0.01 M HCl is added to 5. 6 ml 0. 10 M NaOH, the resulting pH of the solution will be
An aqueous solution contains 0.494 M ethylamine (C2H5NH2).How many mL of 0.206 M hydroiodic acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.600? mL??
The pOH of an acidic buffer is 9.725. What is the Ka of the acid if the ratio of [ionized] to [unionized] is 1380?