question 7 plz 6. A buffer is made by mixing 50.0 mL of 0.10 M acetic acid and 50.0 mL of 0.25 M potassium acetatea. Calculate the pH of the buffer solution.b. Calculate the pH of the buffer solution after adding 1.0 mL of 3.0 M NaOH.c. If 1.0 mL of 3.0 M NaOH were added to 100.0 mL of pure water, what would be theresulting pH?7. A 100.0 mL sample of 0.10 M benzoic acid is titrated with 0.20 M KOH. Determine the pH of thesolution at the equivalence point.8. What is the molar solubility of Ni(OH)2 in a basic solution with a pH of 11.0?9. A 45 mL sample of 0.015 M calcium chloride is added to 55 mL of 0.010 M sodium sulfate. Is aprecipitate expected? Show calculation.your

The pH of the solution at neutralisation point is 7.9245

Answered: 7. A 100.0 mL sample of 0.10 M benzoic…

7. A 100.0 mL sample of 0.10 M benzoic acid is titrated with 0.20 M KOH. Determine the pH of the solution at the equivalence point.

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 72QAP: Four grams of a monoprotic weak acid are dissolved in water to make 250.0 mL of solution with a pH...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

question 7 plz

6. A buffer is made by mixing 50.0 mL of 0.10 M acetic acid and 50.0 mL of 0.25 M potassium acetate
a. Calculate the pH of the buffer solution.
b. Calculate the pH of the buffer solution after adding 1.0 mL of 3.0 M NaOH.
c. If 1.0 mL of 3.0 M NaOH were added to 100.0 mL of pure water, what would be the
resulting pH?
7. A 100.0 mL sample of 0.10 M benzoic acid is titrated with 0.20 M KOH. Determine the pH of the
solution at the equivalence point.
8. What is the molar solubility of Ni(OH)2 in a basic solution with a pH of 11.0?
9. A 45 mL sample of 0.015 M calcium chloride is added to 55 mL of 0.010 M sodium sulfate. Is a
precipitate expected? Show calculation.
your

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A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
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Four grams of a monoprotic weak acid are dissolved in water to make 250.0 mL of solution with a pH of 2.56. The solution is divided into two equal parts, A and B. Solution A is titrated with strong base to its equivalence point. Solution B is added to solution A after solution A is neutralized. The pH of the resulting solution is 4.26. What is the molar mass of the acid?
A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?
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