What is the pH of a 0.44 M solution of the weak base C6H5NH₂ (aniline)?Kb=4.2 × 10-10a 4.87b. 9.13c. 9.73d. 9.31e. 13.14Which of the following acids is the weakest?a. H₂Se6 HCIc. H₂Od. HFe. H₂SWhich salt would produce an acidic solution when dissolved in water?a. K₂SO4b. NH₂Clc. NaCNa. 2.6 x 10-6b. 5.3 × 10-8c. 0.0024The pH of a solution of a weak monoprotic acid (HA) is 2.96. The acid concentration in aqueoussolution is 0.455 M. What is the acid dissociation constant, K₂?CaCO3KFe.0.1541.1 × 10-3A buffer is made with 1.25 M acetic acid (HC₂H₂O₂) and 1.00 M sodium acetate (NaC₂H₂O₂). Whichstatement correctly describes what happens when 0.15 M KOH is added to the buffer?a. Acetic acid neutralizes the KOH and the pH rises slightly.6.The acetate ion neutralizes the KOH and the pH falls slightly.Acetic acid neutralizes the KOH and the pH falls slightly.d.The acetate ion neutralizes the KOH and the pH rises slightly.e. There is no way to predict what happens.

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What is the pH of a 0.44 M solution of the weak base C6H5NH₂ (aniline)? Kb 4.2 x 10-10 3 4.87 b. 9.13 c. 9.73 d. e. 9.31 13.14

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

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

What is the pH of a 0.44 M solution of the weak base C6H5NH₂ (aniline)?
Kb=4.2 × 10-10
a 4.87
b. 9.13
c. 9.73
d. 9.31
e. 13.14
Which of the following acids is the weakest?
a. H₂Se
6 HCI
c. H₂O
d. HF
e. H₂S
Which salt would produce an acidic solution when dissolved in water?
a. K₂SO4
b. NH₂Cl
c. NaCN
a. 2.6 x 10-6
b. 5.3 × 10-8
c. 0.0024
The pH of a solution of a weak monoprotic acid (HA) is 2.96. The acid concentration in aqueous
solution is 0.455 M. What is the acid dissociation constant, K₂?
CaCO3
KF
e.
0.154
1.1 × 10-3
A buffer is made with 1.25 M acetic acid (HC₂H₂O₂) and 1.00 M sodium acetate (NaC₂H₂O₂). Which
statement correctly describes what happens when 0.15 M KOH is added to the buffer?
a. Acetic acid neutralizes the KOH and the pH rises slightly.
6.
The acetate ion neutralizes the KOH and the pH falls slightly.
Acetic acid neutralizes the KOH and the pH falls slightly.
d.
The acetate ion neutralizes the KOH and the pH rises slightly.
e. There is no way to predict what happens.

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