Can someone double check my answers for me. My answers are in bold. A buffer is...
Can someone double check my answers for me. My answers are in bold.
A buffer is __________ (chemical definition) that ____________ (functional definition).
(i) A mixture of a weak acid or base and its conjugate
(ii) A mixture of an acid and a base
(iii) Resists pH changes in aqueous solutions
(iv) Reduces reactivity of aqueous solutions
| A |
(ii), (iii) and (iv) |
|
| B |
(i), (iii) and (iv) |
|
| C |
(ii) and (iii) |
|
| D |
(i) and (iii) |
|
| E |
(i) and (iv) |
Most biologically relevant bases are:
|
A. amines |
||
|
B. sulfides or sulfhydryls |
||
|
C. carboxylates |
||
|
D. amino acids |
E. Metal hyroxides
The Henderson-Hasselbach equation doesn't work when you mix: (not sure)
|
A. A weak acid and its conjugate |
||
|
B. A weak acid and a strong base |
||
|
C. A weak base and its conjugate |
||
|
D. A weak base and a strong acid |
||
|
E. A strong acid and a strong base |
Homework Answers
For Buffer ( i) and ( iii) are answers i.e option D
Amines are biologically relevant basses
For last question Henderson equation wont work when we dont have Buffer. Those cases are when we have
Strong acid and strong Base.
Hence option E
Add Answer to:
Can someone double check my answers for me. My answers are in
bold.
A buffer is...
0, Which of the statements below about an acid-base buffer solution is/are true? IIt can be...
0, Which of the statements below about an acid-base buffer solution is/are true? IIt can be prepared by combining a strong acid with a salt of its conjugate base VII. It can be prepared by combining a weak acid with a salt of its conjugate base IID It can be prepared by combining a weak base with its conjugate acid V. The pH of a buffer solution does not change when the solution is diluted. A buffer solution resists changes...
3.(16.3) Identify all the correct statements about an acid-base buffer solution. I. It can be prepared...
3.(16.3) Identify all the correct statements about an acid-base buffer solution. I. It can be prepared by combining a strong acid with a salt of its conjugate base. II. It can be prepared by combining a weak acid with a salt of its conjugate base. III. It can be prepared by combining a weak base with its conjugate acid. IV. The pH of a buffer solution does not change when the solution is diluted. V. A buffer solution resists changes...
Which of the following are accurate descriptions of buffer solutions? 1. If a solution is buffered, its pH is nearl...
Which of the following are accurate descriptions of buffer solutions? 1. If a solution is buffered, its pH is nearly neutral. II. The mechanism by which buffered solutions resist pH changes is not well understood. III. Addition of strong acid to a buffer shifts the equilibrium such that Ht is consumed. IV. If strong base is added to a buffer, it reacts with the acid component of the mixture. V. Buffers only work well if the one conjugate is present...
I missed class and a classmate sent her notes over and I am confused on what the notes in purple ...
I missed class and a classmate sent her notes over and I am
confused on what the notes in purple mean.
General Chemistry II Module 6 Chapter 16: Aqueous lonic Equilibrium 16.2 Buffers: Solutions That Resist pH Change 1. What is a buffer? significant amounts of weak acids and its conjugate base. The weak acid in a buffer A buffer resists pH change by neutralizing added acid or base. Buffers contain neutralizes added base. The conjugate base in a buffer...
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the so...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
3. 10 points total. Consider the buffer solution that can be created from the weak acid,...
3. 10 points total. Consider the buffer solution that can be created from the weak acid, HF and its conjugate base a. Write the balanced equilibrium equation for this buffer solution. (5 points) b. Applying Le Chatlier's principle, predict which way equilibrium shift with the following disturbances: (1 point each) i. Add hydroxide ii. Remove hydronium iii. Add hydronium c. If 2.5 mol of HF is used to make the buffer solution, how much of the conjugate base (in moles)...
This is from a Study of Buffer Solutions and pH of Salt Solutions Lab. I calculated...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
I need help with the problem in the last photo.. I thought I’d post my lab...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
0, Which of the statements below about an acid-base buffer solution is/are true? IIt can be prepared by combining a strong acid with a salt of its conjugate base VII. It can be prepared by combining a weak acid with a salt of its conjugate base IID It can be prepared by combining a weak base with its conjugate acid V. The pH of a buffer solution does not change when the solution is diluted. A buffer solution resists changes...
3.(16.3) Identify all the correct statements about an acid-base buffer solution. I. It can be prepared by combining a strong acid with a salt of its conjugate base. II. It can be prepared by combining a weak acid with a salt of its conjugate base. III. It can be prepared by combining a weak base with its conjugate acid. IV. The pH of a buffer solution does not change when the solution is diluted. V. A buffer solution resists changes...
Which of the following are accurate descriptions of buffer solutions? 1. If a solution is buffered, its pH is nearly neutral. II. The mechanism by which buffered solutions resist pH changes is not well understood. III. Addition of strong acid to a buffer shifts the equilibrium such that Ht is consumed. IV. If strong base is added to a buffer, it reacts with the acid component of the mixture. V. Buffers only work well if the one conjugate is present...
I missed class and a classmate sent her notes over and I am
confused on what the notes in purple mean.
General Chemistry II Module 6 Chapter 16: Aqueous lonic Equilibrium 16.2 Buffers: Solutions That Resist pH Change 1. What is a buffer? significant amounts of weak acids and its conjugate base. The weak acid in a buffer A buffer resists pH change by neutralizing added acid or base. Buffers contain neutralizes added base. The conjugate base in a buffer...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
3. 10 points total. Consider the buffer solution that can be created from the weak acid, HF and its conjugate base a. Write the balanced equilibrium equation for this buffer solution. (5 points) b. Applying Le Chatlier's principle, predict which way equilibrium shift with the following disturbances: (1 point each) i. Add hydroxide ii. Remove hydronium iii. Add hydronium c. If 2.5 mol of HF is used to make the buffer solution, how much of the conjugate base (in moles)...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
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