2. Calculate the pH of the following solutions:a. A solution that is 0.50M H2CO3 and 0.20M NaHCO3b. 50.0 mL of 0.30M HCN mixed with 75.0 mL of 0.70M NaCNc.A buffer solution that contains a 2:3 ratio of acetic acid to sodium acetate.d.A solution that is made by adding 25.0 g of sodium hydrogen phosphate (be carefulwhen you write the formula) to 500.0 mL of 1.0M potassium phosphate.3. Write the reaction that happens when you add HCl into a NaH2PO4/Na2HPO4 buffer solution.4. Write the reaction that happens when you add NaOH into a NaH2PO4/Na2HPO4 buffer solution5. What amounts of reagents are needed to make the following buffer solutions?a. 300.0 mL, pH = 9.40, lesser component = 0.50M, using 6.0 M NH3 and solid ammoniumchloride.b. 100.0 mL, pH = 8.85, lesser component = 0.10M, using 0.50 M HCN and 1.0 M NaCN.

Answered: Image /qna-images/answer/b93a7f65-eff0-43dd-a4dd-05425d14243c.jpg

2. Calculate the pH of the following solutions: a. A solution that is 0.50M H2CO3 and 0.20M NaHCO3 b. 50.0 mL of 0.30M HCN mixed with 75.0 mL of 0.70M NaCN c. A buffer solution that contains a 2:3 ratio of acetic acid to sodium acetate. d. A solution that is made by adding 25.0 g of sodium hydrogen phosphate (be careful when you write the formula) to 500.0 mL of 1.0M potassium phosphate.

2. Calculate the pH of the following solutions: a. A solution that is 0.50M H2CO3 and 0.20M NaHCO3 b. 50.0 mL of 0.30M HCN mixed with 75.0 mL of 0.70M NaCN c. A buffer solution that contains a 2:3 ratio of acetic acid to sodium acetate. d. A solution that is made by adding 25.0 g of sodium hydrogen phosphate (be careful when you write the formula) to 500.0 mL of 1.0M potassium phosphate.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.17QAP

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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

2. Calculate the pH of the following solutions:
a. A solution that is 0.50M H2CO3 and 0.20M NaHCO3
b. 50.0 mL of 0.30M HCN mixed with 75.0 mL of 0.70M NaCN
c.
A buffer solution that contains a 2:3 ratio of acetic acid to sodium acetate.
d.
A solution that is made by adding 25.0 g of sodium hydrogen phosphate (be careful
when you write the formula) to 500.0 mL of 1.0M potassium phosphate.
3. Write the reaction that happens when you add HCl into a NaH2PO4/Na2HPO4 buffer solution.
4. Write the reaction that happens when you add NaOH into a NaH2PO4/Na2HPO4 buffer solution
5. What amounts of reagents are needed to make the following buffer solutions?
a. 300.0 mL, pH = 9.40, lesser component = 0.50M, using 6.0 M NH3 and solid ammonium
chloride.
b. 100.0 mL, pH = 8.85, lesser component = 0.10M, using 0.50 M HCN and 1.0 M NaCN.

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A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?
Two samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the equivalence point with a 1.00 M solution of sodium hydroxide, while the other sample is titrated to the equivalence point with a 1.00 M solution of calcium hydroxide. a Compare the volumes of sodium hydroxide and calcium hydroxide required to reach the equivalence point for each titration. b Determine the pH of each solution halfway to the equivalence point. c Determine the pH of each solution at the equivalence point.
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