Please help with question 5 Topic4. 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 acidA6. Complete the following table. Show all calculations in the open space, clearly labeled.SolutionPHPOH[H+][OH-]BCleb. CH3COOH + NH3 CH3COO + NH4+D7.b. CO32- as a base9.631.22b. CH3COOH and KCH3COO0.027M3.9x10-6MSolution A has a pH of 4.00. Solution B has a pH of 1.00. Which one is more acidic? How many timesmore acidic?c. H₂S and NaHSAcidic,Basic, orneutral8. Which of the following combinations would act as buffered solutions (look at ions individually)?JUSTIFY why.a. HCI and NaCl

5. Acid : An acid is a chemical species that can donate a proton, H+ in aqueous solution .…

Answered: 5. Write a chemical equation showing…

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 b. CO32- as a base

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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Question

Please help with question 5

Topic
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
6. Complete the following table. Show all calculations in the open space, clearly labeled.
Solution
PH
POH
[H+]
[OH-]
B
C
le
b. CH3COOH + NH3 CH3COO + NH4+
D
7.
b. CO32- as a base
9.63
1.22
b. CH3COOH and KCH3COO
0.027M
3.9x10-6M
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?
c. H₂S and NaHS
Acidic,
Basic, or
neutral
8. Which of the following combinations would act as buffered solutions (look at ions individually)?
JUSTIFY why.
a. HCI and NaCl

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