When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A) is represented as HA (aq) H¹ (aq) + A (aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H¹, forming more HA. When base is added, the base will react with H. reducing its concentration. The reaction then shifts to replace H+ through the dissociation of HA into Hand A. In both instances. [H] tends to remain constant. The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: [A] pH=pK₂ +log HA ▾ ▼ Part A What is the pH of a buffer prepared by adding 0.607 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66 x 10 7 Express the pH numerically to three decimal places. ▸ View Available Hint(s) pH- Submit Part B pH= Submit ΠΙΑΣΦΑ Part C What is the pH after 0.150 mol of HCI is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. View Available Hint(s) 1 196] ΑΣΦ C 3 ? C ? Review | Constants | Periodic Table What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base. Express the pH numerically to three decimal places. ▸ View Available Hint(s)
When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A) is represented as HA (aq) H¹ (aq) + A (aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H¹, forming more HA. When base is added, the base will react with H. reducing its concentration. The reaction then shifts to replace H+ through the dissociation of HA into Hand A. In both instances. [H] tends to remain constant. The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: [A] pH=pK₂ +log HA ▾ ▼ Part A What is the pH of a buffer prepared by adding 0.607 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66 x 10 7 Express the pH numerically to three decimal places. ▸ View Available Hint(s) pH- Submit Part B pH= Submit ΠΙΑΣΦΑ Part C What is the pH after 0.150 mol of HCI is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. View Available Hint(s) 1 196] ΑΣΦ C 3 ? C ? Review | Constants | Periodic Table What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base. Express the pH numerically to three decimal places. ▸ View Available Hint(s)
Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![# pH Changes in Buffers
### Buffer Solution Overview
When a solution contains a weak acid and its conjugate base, or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist changes in pH following the addition of acid or base. A buffer solution prepared from a weak acid (\(HA\)) and its conjugate base (\(A^-\)) is represented as:
\[ HA(aq) \rightleftharpoons H^+(aq) + A^-(aq) \]
According to Le Châtelier's principle, if acid is added, the reaction shifts to consume the added \(H^+\), forming more \(HA\). When a base is added, the base will react with \(H^+\), reducing its concentration. The reaction then shifts to replace \(H^+\) through the dissociation of \(HA\) into \(H^+\) and \(A^-\). In both instances, \([H^+]\) tends to remain constant.
The pH of a buffer is calculated using the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_a + \log \left( \frac{[A^-]}{[HA]} \right) \]
### Exercises
#### Part A
**Problem:**
What is the pH of a buffer prepared by adding 0.807 mol of the weak acid \(HA\) to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant \(K_a\) of \(HA\) is \(5.66 \times 10^{-7}\).
**Instructions:**
Express the pH numerically to three decimal places.
\[ \text{pH} = \]
#### Part B
**Problem:**
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid.
**Instructions:**
Express the pH numerically to three decimal places.
\[ \text{pH} = \]
#### Part C
**Problem:**
What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
**Instructions:**
Express the pH numerically to three decimal places.
\[ \text{pH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2eb625aa-5214-4c13-acfb-22e1dc70de69%2Fd0df912f-2fdd-42e6-83f7-84980a5e7b6d%2F6qck2u4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# pH Changes in Buffers
### Buffer Solution Overview
When a solution contains a weak acid and its conjugate base, or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist changes in pH following the addition of acid or base. A buffer solution prepared from a weak acid (\(HA\)) and its conjugate base (\(A^-\)) is represented as:
\[ HA(aq) \rightleftharpoons H^+(aq) + A^-(aq) \]
According to Le Châtelier's principle, if acid is added, the reaction shifts to consume the added \(H^+\), forming more \(HA\). When a base is added, the base will react with \(H^+\), reducing its concentration. The reaction then shifts to replace \(H^+\) through the dissociation of \(HA\) into \(H^+\) and \(A^-\). In both instances, \([H^+]\) tends to remain constant.
The pH of a buffer is calculated using the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_a + \log \left( \frac{[A^-]}{[HA]} \right) \]
### Exercises
#### Part A
**Problem:**
What is the pH of a buffer prepared by adding 0.807 mol of the weak acid \(HA\) to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant \(K_a\) of \(HA\) is \(5.66 \times 10^{-7}\).
**Instructions:**
Express the pH numerically to three decimal places.
\[ \text{pH} = \]
#### Part B
**Problem:**
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid.
**Instructions:**
Express the pH numerically to three decimal places.
\[ \text{pH} = \]
#### Part C
**Problem:**
What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
**Instructions:**
Express the pH numerically to three decimal places.
\[ \text{pH
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