Concept explainers
Videos
(a)
Interpretation:
The buffer capacity of 0.250 M lactic acid and 0.250 M lactate ion should be determined.
Concept introduction:
A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation
Also known as Henderson Hasselbalch’s equation
The buffer capacity is the capacity of a buffer to which it can resist a major change in pH on addition of acid or base.
It is dependent on the ratio of concentration of weak acid and concentration of its conjugate base.
(b)
Interpretation:
The buffer capacity of 0.250 M lactic acid and 0.125 M lactate ion should be determined.
Concept introduction: A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation.
Also known as Henderson Hasselbalch’s equation
The buffer capacity is the capacity of a buffer to which it can resist a major change in pH on addition of acid or base.
It is dependent on the ratio of concentration of weak acid and concentration of its conjugate base
(c)
Interpretation:
The buffer capacity of 0.250 M lactic acid and 0.0800 M lactate ion should be determined.
Concept introduction: A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation.
Also known as Henderson Hasselbalch’s equation
The buffer capacity is the capacity of a buffer to which it can resist a major change in pH on addition of acid or base.
It is dependent on the ratio of concentration of weak acid and concentration of its conjugate base
(d)
Interpretation:
The buffer capacity of 0.250 M lactic acid and 0.0500 M lactate ion should be determined.
Concept introduction:
A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation
Also known as Henderson Hasselbalch’s equation
The buffer capacity is the capacity of a buffer to which it can resist a major change in pH on addition of acid or base.
It is dependent on the ratio of concentration of weak acid and concentration of its conjugate base
Want to see the full answer?
Check out a sample textbook solution
Chapter 14 Solutions
Chemistry: Principles and Reactions
- Identify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal molar amounts of the following: a. HF, KC2H3O2, NaC2H3O2, and NaF b. HNO3, NaOH, H3PO4, and NaH2PO4arrow_forwardEnough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.arrow_forwardDoes the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?arrow_forward
- Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10–10) solution.arrow_forwardDefine buffering capacity. How do the followingbuffers differ in buffering capacity? How do they differ in pH?Buffer a: 0.01 M Na2HPO4 and 0.01 M NaH2PO4Buffer b: 0.10 M Na2HPO4 and 0.10 M NaH2PO4Buffer c: 1.0 M Na2HPO4 and 1.0 M NaH2PO4arrow_forwardGiven two buffer solutions: Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO Buffer 2 : 2.00 M CH3COOH - 2.00 M NaCH3COO (Ka CH3COOH=1.8x10-5) In terms of buffering capacity, which is correct? Buffer 1 < Buffer 2 Buffer 1 > Buffer 2 Buffer 1 = Buffer 2arrow_forward
- What are buffers? Define and discuss the differences between the twotypes of buffers presentedarrow_forwardWhich of these factors influence buffer capacity? How?(a) Conjugate acid-base pair(b) pH of the buffer(c) Concentration of buffer components(d) Buffer range(e) pKₐ of the acid componentarrow_forwardA student makes a buffer from 100 mL of 0.10 M formic acid (HCOOH) and 100 mL of 0.10 M potassium formate (KCHOO). Upon addition of 20 mL of 1M NaOH solution, the student observes the pH is significantly higher than the original pH of the buffer, and concludes the buffer was defective. Is the student correct? What is the buffer capacity?arrow_forward
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning