Please help with question 8 Topic 14 HW4. In each of the following chemical equations, identify the conjugate acid-base pairs.a. CH3NH2 + H₂O CH3NH3+ + OH-5. Write a chemical equation showing how each of the following species can behave as indicated whendissolved in water(this is the other reactant).a. HSO3 as an acidAB6. Complete the following table. Show all calculations in the open space, clearly labeled.SolutionpHPOH[H+][OH-]PUOb. CH3COOH + NH3 CH3COO- + NH4+Cb. CO32- as a baseD9.631.223.9x10-6M7. Solution A has a pH of 4.00. Solution B has a pH of 1.00. Which one is more acidic? How many timesmore acidic?b. CH3COOH and KCH3COO0.027Mc. H₂S and NaHSAcidic,Basic, orneutral8. Whic of the owing combinations would act as buffered solutions (look at the ions individually)?JUSTIFY why.a. HCI and NaCl

Given : compounds Tip : buffer solution contains weak acid or base and their salt.

Answered: 8. Which of the following combinations…

8. Which of the following combinations would act as buffered solutions (look at the ions individually)? JUSTIFY why. a. HCI and NaCl b. CH3COOH and KCH³COO c. H₂S and NaHS

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

Please help with question 8

Topic 14 HW
4. In each of the following chemical equations, identify the conjugate acid-base pairs.
a. CH3NH2 + H₂O CH3NH3+ + OH-
5. Write a chemical equation showing how each of the following species can behave as indicated when
dissolved in water(this is the other reactant).
a. HSO3 as an acid
A
B
6. Complete the following table. Show all calculations in the open space, clearly labeled.
Solution
pH
POH
[H+]
[OH-]
PUO
b. CH3COOH + NH3 CH3COO- + NH4+
C
b. CO32- as a base
D
9.63
1.22
3.9x10-6M
7. Solution A has a pH of 4.00. Solution B has a pH of 1.00. Which one is more acidic? How many times
more acidic?
b. CH3COOH and KCH3COO
0.027M
c. H₂S and NaHS
Acidic,
Basic, or
neutral
8. Whic of the owing combinations would act as buffered solutions (look at the ions individually)?
JUSTIFY why.
a. HCI and NaCl

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