a. Calculate the pH of a buffer that is 0.4 M in acetic acid (CH3COOH) and 0.4 M in potassium acetate (CH3 COOK). The pK, for acetic acid is 4.74. pH = b. What is the pH of a buffer that is 3 M in acetic acid and 3 M in potassium acetate? pH= c. What is the difference between the buffers described in parts a and b? The solution in part b has buffer capacity than the solution in part a. Submit Answer Try Another Version 5 item attempts remaining

a. Calculate the pH of a buffer that is 0.4 M in acetic acid (CH3COOH) and 0.4 M in potassium acetate (CH3 COOK). The pK, for acetic acid is 4.74. pH = b. What is the pH of a buffer that is 3 M in acetic acid and 3 M in potassium acetate? pH= c. What is the difference between the buffers described in parts a and b? The solution in part b has buffer capacity than the solution in part a. Submit Answer Try Another Version 5 item attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: 1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that contains 0.100 M HNO2 and 0.200 M…

Q: HA 0.05 L buffer solution (pH = 11.00) was prepared from 0.02 L, 0.2 M NaHCO3 and bottle of sodium…

A: Given the volume of the buffer solution prepared = 0.05 L pH of the buffer = 11.00 NaHCO3 and…

Q: A

Q: b. adding a small amount of 1 M hydrochloric acid C. adding a small amount of 1 M sodium hydroxide

A: pH and pka is given of buffer solution.

Q: A student is asked to prepare a buffer with a pH of 5.40 by adding sodium hydroxide to a weak acid.…

A: a) Buffer is a solution that resists a change in pH when a small amount of acid or base is added to…

Q: Consider the bases in the table. Which base would be the best choice for preparing a pH =…

A: Henderson-Hasselbalch equation: This equation is used to calculate the pH values for the buffer. For…

Q: Out of the following choices, the one with the highest buffer capacity is? A. 0.50 M H₂PO4/0.50 M…

A: The formula for buffer capacity is the moles of acid or base required to raise the pH of a solution…

Q: ΝΗ A chemistry graduate student is given 500. mL of a 0.50M diethylamine ((C₂H₂)₂NH) solution.…

Q: . A buffer is prepared by mixing 48.2 mL of 0.196 M NaOH with 141.2 mL of 0.231 M acetic acid. What…

Q: a. What is the pH of 50.00 mL buffer solution which is 2.00 M in HC,HO2 and 2.00 M in NaC2H3O2? (K,…

Q: What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.20 buffer? (Kb for CH₃NH₂ is 4.4 ×…

Q: a. How many grams of dry NH4CI need to be added to 2.40 L of a 0.300 M solution of ammonia, NH3, to…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: 1) Which one of the following combinations of solutions will NOT form a buffer solution? a. NaCl and…

A: As per bartleby Q&A lines.we can solve first question only .please re upload remaining another…

Q: A Calculating the pH of a Buffer: pH-pk +log HA the Henderson-Hasselbalch equation. This applies…

A: The solution that resists the change in pH is known as a buffer solution. The buffer solution is an…

Q: 1. What is the pH of a buffer that is 0.20 M HF and 0.085 M KF? pKa = 3.152. What is the pH of a…

A: 1. The concentration of The concentration of 2. The number of moles of The number of moles of The…

Q: A buffer was prepared by mixing 19.53 g NaF and 10.41 g HF in a 1.0 L reaction vessel. Ka = 7.1 x…

Q: None

A: Step 1: Calculate the pKapKa = -log(1.3 x 10-5) = 4.89 Step 2: Use the Henderson-Hasselbalch…

Q: The titration curve of a weak acid, HnA has 3 inflection points at pH = 3.5, 6.7 and 10.3. If 0.1 M…

Q: A buffer contains 0.15 mol of propionic acid ( CH₂COOH) and 0.24 mol of sodium propionate…

Q: In which solution would you expect zinc hydroxide to be the most soluble given that Ksp of Zn(OH)2…

A: 1 M strong base

Q: What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric…

A: Buffer solutions: When a tiny amount of acid or base is added to a solution, buffer solutions resist…

Q: Calculating the composition of a buffer of a given pH -5 A chemistry graduate student is given 500.…

A: NH4Br = 28 gramsExplanation:Step 1:+We can use the Henderson hasselbach equation to get the moles of…

Q: What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric…

A: Given the pH of the buffer = 4.25 Given the total molarity of HF/KF buffer, C = 0.450 M Total…

Q: . Are these results precise? Explain.

A: No, these results are not precise.

Q: 3. TRIS, N-tri[hydroxymethyl]aminomethane, is one of Good's buffers. In its unprotonated form, it is…

A: The objective of the question is to calculate the pH of the resulting solution when 20 mL of 0.2 M…

Q: U ☐ x10 A chemistry graduate student is given 300. mL of a 0.10M chloroacetic acid (HCH2CICO₂)…

A: Finally, we convert moles to grams. The molar mass of NaCH2ClCO2 (sodium chloroacetate) is…

Q: Which of the following statements is true about a 1-L buffer solution prepared by mixing 1.13 mol…

Q: A buffer is made with 200.0 mL of 0.30 M propanoic acid (HC3H50₂) and 300.0 mL of 0.267 M NaC3H5O2.…

A: Buffer solution is the solution which have capacity to resist the change of its pH value even with…

Q: I want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM NaOH. I…

A: In the given question we have to calculate the volume of each solution that is present in the…

Q: a. What is the pH of a buffer solution that is 0.28 M NH3 and 0.28 M NH4+? K for NH3 is 1.8 × 10-5…

A: Given : a. Concentration of NH3 = 0.28 M Concentration of NH4+ = 0.28 M Kb of NH3 = 1.8 x 10-5…

Q: A buffer contains 0.10 mol of a weak acid and 0.20 mol of its conjugate base in 1.0 L of solution.…

A: Whether the addition of the given buffer solutions exceeds the capacity of the buffer or not has to…

Q: Calculating the composition of a buffer of a given pH 4 A chemistry graduate student is given 125.…

A: 1.873 x 10-⁷ gExplanation:Step 1: To make buffers solution, we need to calculate the ratio of the…

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

[References]
a. Calculate the pH of a buffer that is 0.4 M in acetic acid (CH3 COOH) and 0.4 M in potassium acetate (CH3 COOK). The pK, for acetic acid is 4.74.
pH =
b. What is the pH of a buffer that is 3 M in acetic acid and 3 M in potassium acetate?
pH =
c. What is the difference between the buffers described in parts a and b?
The solution in part b has
buffer capacity than the solution in part a.
Submit Answer
Try Another Version
5 item attempts remaining

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A chemistry graduate student is given 500. mL of a 0.30 M benzoic acid (HC6H5CO2) solution. Benzoic acid is a weak acid with K= 6.3x 10-5 . What mass of NaC6H5CO2 should the student dissolve in the HC6H5CO2 solution to turn it into a buffer with pH = 4.25? You may assume that the volume of the solution doesn't change when the NaC6H5CO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
None
Which of the following statements is true about a 1-L buffer solution prepared by mixing 1.13 mol propionic acid (C2H5COOH) and 2.03 mol sodium propionate (C2H5COONa)? Ka(C2H5COOH) = 1.34 x 10-5? (Choose one option only). Options: a. The pH of the above buffer solution is less than the pKa of C2H5COOH. b. By adding water to dilute the above buffer solution, the pH of the buffer solution will decrease. c. By adding water to dilute the above buffer solution, the pH of the buffer solution will increase. d. By readjusting the amount of propionic acid and sodium propionate, we can prepare a buffer solution at pH = 8.00. e. The pH of the above buffer solution is greater than the pKa of C2H5COOH.
What mass (in g) of ammonium chloride (NH4Cl) should be added to 2.60 L of a 0.155 M NH3 to obtain a buffer with a pH of 9.45? (Kb for NH3 is 1.8 x 10-5)
Consider a buffer made by adding 132.8 g of NaC-H5O, to 300.0 mL of 1.97 M HC-H.O, (Ka = 6.3 x 10-5) a. What is the pH of this buffer? b. What is the pH of the buffer after 0.750 mol of H+ has been added? c. What is the pH of the buffer after 0.250 mol of OH- has been added?
We have to make a borate buffer with pH = 8.8 where the boric acid pKa = 9.00. If we start with a 1 liter of 0.1 M boric acid solution, what mass of hydroxide ions should be added to get the desired pH? Boric acid has the molecular formula B (OH) 3 and the borate ion B (OH)
6. A buffer solution contains 0.120 moles of propionic acid, HC3H502, and 0.100 moles of sodium propionate, NaC3H5O2, in 1.00 L of solution. Ka = 1.32 x 10-5 a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.010 mol of NaOH? c. Beginning with the initial buffer from part a, what is the pH of the buffer after the addition of 0.010 mol of HBr?
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
A weak acid/conjugate base buffer has a pH smaller than the pKa of the acid. How does this affect the buffer capacity? Think about two experiments, one where you are adding base and one where you are adding acid. Are the buffer capacities the same? Which will the buffer resist better?
5
1a. How many grams of solid sodium cyanide should be added to 1.50 L of a 0.108 M hydrocyanic acid solution to prepare a buffer with a pH of 10.043 ?grams sodium cyanide = 1b. How many grams of solid ammonium bromide should be added to 1.00 L of a 0.244 M ammonia solution to prepare a buffer with a pH of 9.820 ? grams ammonium bromide = 1c. How many grams of solid sodium hypochlorite should be added to 1.00 L of a 0.206 M hypochlorous acid solution to prepare a buffer with a pH of 8.249 ?grams sodium hypochlorite =
8. What is the pH of a weak acid with [HA] = 0.125 mol/L and Ka = 5.4×107? 9. A buffer is created by adding 0.35 mol of sodium benzoate to 1.00 L of a 0.40 mol/L benzoic acid solution. The Ka of benzoic acid is 6.3×105. Determine the pH of the buffer.