Buffer Question 1: A 1.00L solution is made of 0.40mol/L NaNO2 and 0.25mol/L HNO2 (K₁ = 4.5 × 10-4). What is the pH of this solution? Buffer Question 2: To this solution, 20.0mL of 0.15 mol/L HNO3 is added. What is the resulting pH? Buffer Question 3: You have a 1.00L acetic acid buffer solution of pH 4.2. If the concentration of potassium acetate is 0.50 mol/L potassium acetate, what is the concentration of the acetic acid? (Ka = 1.8 × 10-5) Buffer Question 4: 250.0 mL of 0.50 mol/L sodium formate is added to 250.0 mL of 0.75 mol/L formic acid. What is the resulting pH of the solution (K₁ = 1.8 × 10-4)
Buffer Question 1: A 1.00L solution is made of 0.40mol/L NaNO2 and 0.25mol/L HNO2 (K₁ = 4.5 × 10-4). What is the pH of this solution? Buffer Question 2: To this solution, 20.0mL of 0.15 mol/L HNO3 is added. What is the resulting pH? Buffer Question 3: You have a 1.00L acetic acid buffer solution of pH 4.2. If the concentration of potassium acetate is 0.50 mol/L potassium acetate, what is the concentration of the acetic acid? (Ka = 1.8 × 10-5) Buffer Question 4: 250.0 mL of 0.50 mol/L sodium formate is added to 250.0 mL of 0.75 mol/L formic acid. What is the resulting pH of the solution (K₁ = 1.8 × 10-4)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.131QP: A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The...
Question
![Buffer Question 1: A 1.00L solution is made of 0.40mol/L NaNO2 and
0.25mol/L HNO2 (K₁ = 4.5 × 10-4).
What is the pH of this solution?
Buffer Question 2: To this solution, 20.0mL of 0.15 mol/L HNO3 is added. What is
the resulting pH?
Buffer Question 3: You have a 1.00L acetic acid buffer solution of pH 4.2. If the
concentration of potassium acetate is 0.50 mol/L potassium acetate, what is the
concentration of the acetic acid? (Ka = 1.8 × 10-5)
Buffer Question 4: 250.0 mL of 0.50 mol/L sodium formate is added to 250.0 mL of
0.75 mol/L formic acid. What is the resulting pH of the solution
(K₁ = 1.8 × 10-4)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F633dc666-1c4e-4222-82a0-1d910c7662c5%2F7273c6e3-4023-4d62-8a5a-33feabad92ed%2Fbdiaxtd_processed.png&w=3840&q=75)
Transcribed Image Text:Buffer Question 1: A 1.00L solution is made of 0.40mol/L NaNO2 and
0.25mol/L HNO2 (K₁ = 4.5 × 10-4).
What is the pH of this solution?
Buffer Question 2: To this solution, 20.0mL of 0.15 mol/L HNO3 is added. What is
the resulting pH?
Buffer Question 3: You have a 1.00L acetic acid buffer solution of pH 4.2. If the
concentration of potassium acetate is 0.50 mol/L potassium acetate, what is the
concentration of the acetic acid? (Ka = 1.8 × 10-5)
Buffer Question 4: 250.0 mL of 0.50 mol/L sodium formate is added to 250.0 mL of
0.75 mol/L formic acid. What is the resulting pH of the solution
(K₁ = 1.8 × 10-4)
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