Titrations and Buffers

Titrations and Buffers

Time limit: 0

Quiz Summary

0 of 21 Questions completed

Questions:

Information

You have already completed the quiz before. Hence you can not start it again.

Quiz is loading…

You must sign in or sign up to start the quiz.

You must first complete the following:

Results

Quiz complete. Results are being recorded.

Results

0 of 21 Questions answered correctly

Your time:

Time has elapsed

You have reached 0 of 0 point(s), (0)

Earned Point(s): 0 of 0, (0)
0 Essay(s) Pending (Possible Point(s): 0)

Categories

Not categorized 0%

1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21

Current
Review
Answered
Correct
Incorrect

Question 1 of 21

1. Question
If a strong acid and a strong base are titrated with one another what will the pH at the equivalence point be?
- <7
- =7
- >7
Correct

Incorrect
Question 2 of 21

2. Question
If a strong acid is titrated with a weak base what will the pH at the equivalence point be?
- <7
- =7
- >7
Correct

Incorrect
Question 3 of 21

3. Question
If you titrate a weak acid with a weak base what will the pH at the equivalence point be?
- <7
- =7
- >7
Correct

Incorrect
Question 4 of 21

4. Question
If you titrate HCl with NaCH₃COO what will the pH be at the equivalence point?
- <7
- =7
- >7
Correct

Incorrect
Question 5 of 21

5. Question
If you titrate NaOH with hexanoic acid what will the pH at the equivalence point be?
- <7
- =7
- >7
Correct

Incorrect
Question 6 of 21

6. Question
Two mols of base was titrated with a solution of HCl to reach the equivalence point. How many mols of acid are present in the solution?
- 1 mol
- 2 mols
- 3 mols
- 4 mols
Correct

Incorrect
Question 7 of 21

7. Question
0.5 L of 0.04 M acetic acid was titrated with an unknown solution of base in order to reach the equivalence point. How many moles of base does the unknown solution contain?
- 0.01 mols
- 0.02 mols
- 0.04 mols
- 0.08 mols
Correct

Incorrect
Question 8 of 21

8. Question
A 0.6 M solution of HCl was added to 25 mL of an ammonia solution. If it took 500 mL of the HCl solution to reach the equivalence point what was the original concentration of the ammonia solution?
- 0.012 M
- 0.06 M
- 0.6 M
- 1.2 M
Correct

Incorrect
Question 9 of 21

9. Question
A tris buffer (pKa=8.1) could effectively buffer a solution within what pH range?
- 7.1 – 9.1
- 8.1 – 9.1
- 7.1 – 8.1
Correct

Incorrect
Question 10 of 21

10. Question
A scientist is attempting to evaluate the function of a protein at a pH of 6. Which of the following buffers should the experiment be carried out in?
- POPSO (pKa = 7.8)
- CABS (pKa = 10.7)
- MOPSO (pKa = 6.9)
- NAACE (pKa =4.7)
Correct

Incorrect
Question 11 of 21

11. Question
Which of the following buffers would be suitable for conducting an experiment at pH 9?
- Cacodylate (pKb = 7.8)
- Glycine HCl (pKb = 9.2)
- Glycine NaOH (pKb = 4.3)
- Barbital (pKb = 6.1)
Correct

Incorrect
Question 12 of 21

12. Question
Which of the following buffers could effectively buffer a solution at a pH of 5?
- Buffer A (Ka = 8×10^-5)
- Buffer B (Ka = 5×10^-11)
- Buffer C (Ka = 2×10^-2)
- Buffer D (Ka = 1×10^-3)
Correct

Incorrect
Question 13 of 21

13. Question
A buffer is created from acetic acid (pKa =4.8) and its conjugate base acetate and adjusted to a pH of 5.8. Which of the following is true about the solution?
- It has a higher concentration of acetic acid as compared to acetate
- It has a higher concentration of acetate as compared to acetic acid
- It has the same concentration of acetate and acetic acid
Correct

Incorrect
Question 14 of 21

14. Question
A buffer is created out of benzoic acid (pKa = 4.2) and its conjugate base, benzoate, and adjusted to a pH of 2.2. Which of the following is true of the solution?
- It has a higher concentration of benzoic acid as compared to benzoate
- It has a higher concentration of benzoate as compared to benzoic acid
- It has the same concentration of benzoate and benzoic acid
Correct

Incorrect
Question 15 of 21

15. Question
A buffered solution contains 0.2 M of CHOOH (pKa = 3.7) and 0.002 M of CHOO^–. What will the pH of the buffer be?
- 1.7
- 3.7
- 4.7
- 5.7
Correct

Incorrect
Question 16 of 21

16. Question
A buffered solution contains 0.02 M of CHOOH (pKa = 3.7) and 0.002 M of CHOO^–. What will the pH of the buffer be?
- 1.7
- 2.7
- 3.7
- 4.7
Correct

Incorrect
Question 17 of 21

17. Question
A solution of 0.003M H₂S and 3M HS^– would have a pH of:

(Note: H₂S pKa = 7.01)
- 4.01
- 7.01
- 9.01
- 10.01
Correct

Incorrect
Question 18 of 21

18. Question
A buffered solution of acetic acid (pK_a =4.8) and acetate is adjusted to a pH of 6.8. What is the ratio of acetic acid to acetate in solution?
- 1:2
- 1:100
- 2:1
- 100:1
Correct

Incorrect
Question 19 of 21

19. Question
A buffered solution of carbonic acid (pK_a = 6.4) and bicarbonate was created and adjusted to a pH of 5.4. By what factor is the carbonic acid concentration increased in comparison to bicarbonate concentration in the buffer solution?
- 0.1
- 1
- 10
- 100
Correct

Incorrect
Question 20 of 21

20. Question
A buffered solution containing 0.5 M acetic acid and 0.05 M acetate has a pH of 3.4. What is the pKa of acetic acid?
- 2.4
- 3.4
- 4.4
- 5.4
Correct

Incorrect
Question 21 of 21

21. Question
A solution containing 20mL of 2M carbonic acid (pKa = 6.4) and 40 mL of 1M bicarbonate would have a pH of:
- 5.4
- 6.4
- 7.4
- 8.4
Correct

Incorrect

Login

Accessing this course requires a login. Please enter your credentials below!

Username or Email Address

Password

Remember Me

Lost Your Password?

Register

Don't have an account? Register one!

Register an Account

Username

Email

Registration confirmation will be emailed to you.