11. Which is a Lewis acid-base reaction but not a Bronsted-Lowry acid-base reaction? [a] NH3)+BF%)→ H₂NBF3(g) [b] NHS) + H₂O → NH4+(aq) + OH-(aq) [c] CH3NH2(aq) + HBr(aq) → CH3NH3(aq) + + Br-(aq) [d] CH3COOH(aq) + H₂O)→ CH3COO-(aq) + H3O+ (aq) [e] NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O0) 12. The pH of a 0.100 M solution of a weak acid, HA, is 3.50. Calculate the percent ionization of the acid in 0.100 M solution. a. 0.016% b. 0.078% c. 0.32% d. 0.68% e. 1.6% 13. Calculate the pH of a solution resulting from the addition of 20.0 mL of 0.100 MHCI to 50.0 mL of 0.100 MNH3. a. 9.26 b. 4.91 c. 9.44 d. 4.60 e. 9.08 14. Which of the following formulas represents an alkane? (5 points) A. C₂H4 B. C3H7 C. C4H10 D. C5Hg 15. The half-life of 231 Pa is 3.25 x 104 y. How much of an initial 10.40 microgram sample remains after 3.25 x 105 y? a. 0.0102 µg b. 0.240 µg c. 0.0240 μg d. 1.02 µg e. 1.04 µg 6 E. C6H6 16. A

11. Which is a Lewis acid-base reaction but not a Bronsted-Lowry acid-base reaction? [a] NH3)+BF%)→ H₂NBF3(g) [b] NHS) + H₂O → NH4+(aq) + OH-(aq) [c] CH3NH2(aq) + HBr(aq) → CH3NH3(aq) + + Br-(aq) [d] CH3COOH(aq) + H₂O)→ CH3COO-(aq) + H3O+ (aq) [e] NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O0) 12. The pH of a 0.100 M solution of a weak acid, HA, is 3.50. Calculate the percent ionization of the acid in 0.100 M solution. a. 0.016% b. 0.078% c. 0.32% d. 0.68% e. 1.6% 13. Calculate the pH of a solution resulting from the addition of 20.0 mL of 0.100 MHCI to 50.0 mL of 0.100 MNH3. a. 9.26 b. 4.91 c. 9.44 d. 4.60 e. 9.08 14. Which of the following formulas represents an alkane? (5 points) A. C₂H4 B. C3H7 C. C4H10 D. C5Hg 15. The half-life of 231 Pa is 3.25 x 104 y. How much of an initial 10.40 microgram sample remains after 3.25 x 105 y? a. 0.0102 µg b. 0.240 µg c. 0.0240 μg d. 1.02 µg e. 1.04 µg 6 E. C6H6 16. A

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...

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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

11-15

[a] NH3)+BF%)→ H3NBF3(g)
[b] NHS) + H₂O → NH4+ng)+ OH-(aq)
[c] CH3NH2(aq) + HBr(aq) → CH3NH3(aq) + + Br-(ag)
[d] CH3COOH(aq) + H₂O)→ CH3COO-(aq) + H3O+(ag)
[e] NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O0)
11. Which is a Lewis acid-base reaction but not a Bronsted-Lowry acid-base
reaction?
12. The pH of a 0.100 M solution of a weak acid, HA, is 3.50. Calculate the percent ionization
of the acid in 0.100 M solution.
a.
0.016%
b. 0.078%
c. 0.32%
d. 0.68%
e. 1.6%
13. Calculate the pH of a solution resulting from the addition of 20.0 mL of 0.100 MHCI to
50.0 mL of 0.100 MNH3.
a. 9.26
b. 4.91
c. 9.44
d. 4.60
e. 9.08
14. Which of the following formulas represents an alkane? (5 points)
A. C₂H4
B. C3H7 C. C4H10 D. C5Hg
a. 0.0102 µg
b. 0.240 µg
c. 0.0240 μg
d. 1.02 µg
e. 1.04 µg
15. The half-life of 231 Pa is 3.25 x 104 y. How much of an initial 10.40 microgram sample
remains after 3.25 x 10³ y?
E. C6H6
6
16. A plot of
17. H

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