11. A 0.64 M solution of the weak hase hydrazine (NH) is found to be 0.16% ionized at equilibrium. What is the value of K for hydrazine? a. 1.0x10 d. 6.7x10 10x10¹ b. 1.6x10 c. 5.77 e
11. A 0.64 M solution of the weak hase hydrazine (NH) is found to be 0.16% ionized at equilibrium. What is the value of K for hydrazine? a. 1.0x10 d. 6.7x10 10x10¹ b. 1.6x10 c. 5.77 e
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...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
Question 11. THIS IS NOT FOR A GRADE!
**It's a practice exam with the answer posted with it!**
I just need help with the concept please explain
![6. The following equilibrium is established in a sealed container. Which of the following changes would increase
the partial pressure of SO:(g) at equilibrium?
SO,Cl₂(g) SO₂(g) + Cl₂(g)
Adding an inert gas (such as helium).
a.
b. Increasing the temperature.
C. Removing SOCI(g)
d. Adding Cl(g).
C. Decreasing the volume of the reaction vessel.
7. Which of the following is not a conjugate acid-base pair?
a. HF. II
b. HCN, CN
9. What is the pH of a solution with [OH]- 1.8x10¹?
a. 4.75
b. 9.25
c. 7.00
AH +67
c. H₂SO, HSO d. H.PO. HPO e HCL CI
8. Which of the following pairs lists the weaker acid first?
a. HCL, HCIO b. IIBRO, HBrO; c. H₂O, NaOH d. HCIO, HBO, e. HBr. HI
10. What is the pH of a solution that is 0.40 M in HCN?
b. 9.40
a. 0.40
c. 9.80
kJ
mol
d. 4.76
e. 8.25
The K, for HCN is 4.0x10".
d. 4.90
e. 9.10
11. A 0.64 M solution of the weak base hydrazine (NH₂) is found to be 0.16% ionized at equilibrium. What is the
value of K for hydrazine?
a. 1.0x10
b. 1.6x10
d. 6.7x10
b. 1.06
c. 5.77
e. 1.0x10¹¹
12. Which of the following substances produces a basic solution when dissolved in water?
a. CaBrz
d. Co(NO): e. NaCN
b. NHƯ
LICI
13. A sample of 0.050 mol of NaOH is added to a solution containing 0.100 mol of acetic acid (K,-1.8x10³). After
mixing, is the solution a buffer?
a. Yes, because the solution contains a weak acid and its conjugate base.
b. Yes, because the solution contains acetate ions and hydroxide ions.
C. No, because the solution contains acetate ions and hydroxide ions.
d. No, because we don't know the volume.
e. No, because we have too much acid.
14. A sample of 0.45 mol of the weak acid HCIO (pK, = 7.54) and 0.15 mol of NaClO are dissolved in enough water to
make 0.750 L. of solution. What is the pH of the solution?
a. 7.06
b. 8.02
c. 3.88
C.
e. 0.398
d. 10.42
15. When 15.0 mL of a 0.20 M HCl solution is mixed with 20.0 mL of 0.15 M NaOH solution, what is the pH of the
resulting solution?
a. 7.00
C. 12.93
d. 6.93
e. 7.25](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F43965b80-42e8-41df-9b51-2c2200725cfe%2F3bd1b3cb-e1f9-46d8-8820-8895c30682b5%2F0395w1b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:6. The following equilibrium is established in a sealed container. Which of the following changes would increase
the partial pressure of SO:(g) at equilibrium?
SO,Cl₂(g) SO₂(g) + Cl₂(g)
Adding an inert gas (such as helium).
a.
b. Increasing the temperature.
C. Removing SOCI(g)
d. Adding Cl(g).
C. Decreasing the volume of the reaction vessel.
7. Which of the following is not a conjugate acid-base pair?
a. HF. II
b. HCN, CN
9. What is the pH of a solution with [OH]- 1.8x10¹?
a. 4.75
b. 9.25
c. 7.00
AH +67
c. H₂SO, HSO d. H.PO. HPO e HCL CI
8. Which of the following pairs lists the weaker acid first?
a. HCL, HCIO b. IIBRO, HBrO; c. H₂O, NaOH d. HCIO, HBO, e. HBr. HI
10. What is the pH of a solution that is 0.40 M in HCN?
b. 9.40
a. 0.40
c. 9.80
kJ
mol
d. 4.76
e. 8.25
The K, for HCN is 4.0x10".
d. 4.90
e. 9.10
11. A 0.64 M solution of the weak base hydrazine (NH₂) is found to be 0.16% ionized at equilibrium. What is the
value of K for hydrazine?
a. 1.0x10
b. 1.6x10
d. 6.7x10
b. 1.06
c. 5.77
e. 1.0x10¹¹
12. Which of the following substances produces a basic solution when dissolved in water?
a. CaBrz
d. Co(NO): e. NaCN
b. NHƯ
LICI
13. A sample of 0.050 mol of NaOH is added to a solution containing 0.100 mol of acetic acid (K,-1.8x10³). After
mixing, is the solution a buffer?
a. Yes, because the solution contains a weak acid and its conjugate base.
b. Yes, because the solution contains acetate ions and hydroxide ions.
C. No, because the solution contains acetate ions and hydroxide ions.
d. No, because we don't know the volume.
e. No, because we have too much acid.
14. A sample of 0.45 mol of the weak acid HCIO (pK, = 7.54) and 0.15 mol of NaClO are dissolved in enough water to
make 0.750 L. of solution. What is the pH of the solution?
a. 7.06
b. 8.02
c. 3.88
C.
e. 0.398
d. 10.42
15. When 15.0 mL of a 0.20 M HCl solution is mixed with 20.0 mL of 0.15 M NaOH solution, what is the pH of the
resulting solution?
a. 7.00
C. 12.93
d. 6.93
e. 7.25
Transcribed Image Text:Answer Section
MULTIPLE CHOICE
1.
ANS: E
2.
ANS: E
3.
ANS: B
4.
ANS: A
5.
ANS: D
6.
ANS: B
7.
ANS: A
8.
ANS: E
9.
ANS: B
10. ANS: D
11. ANS: B
12. ANS: E
13. ANS: A
14. ANS: A
15. ANS: A
16. ANS: D
17. ANS: A
18. ANS: E
19. ANS: B
20. ANS: B
21. ANS: A
22. ANS: C
23. ANS: C
24. ANS: C
25. ANS: C
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!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 1 images
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY