2. Would you expect a solution of ammonium chloride (NHCI) to be acidic or basic when added to water? (K NH = 1.8 x 10-5) 3. 4. What is the pH of a 1.15 M solution of methanoic acid? K = 1.8 × 10-4 What is the pH of a 0.350 M solution of lithium citrate? (K. Citric Acid = 7.4 x 10-) Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved. 5. SCH4U Unit 3 Assessment A 50.0 mL solution of 0.150 M acetic acid (CH COOH) is titrated with 0.150 M NaOH. What is the pH after 20.0 mL of base has been added? K. CH COOH = 1.8 x 10-5 4. Explain why the conjugate base of a strong acid can't react with water. Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved. 3 5. Why are some salts acidic when others are neutral? SCH4U Unit 3 Assessment Curriculum Expectation E2. investigate the qualitative and quantitative nature of chemical systems at equilibrium, and solve related problems. 1. Consider the following reaction: PCI (g)+ Cl₂ (g) PCI (g) K = 4.30 x 10-6 Initially, 2.50 M PCI, and 1.40 M Cl₂ are placed into a container and allowed to reach equilibrium. Determine the equilibrium concentrations of all the species.
2. Would you expect a solution of ammonium chloride (NHCI) to be acidic or basic when added to water? (K NH = 1.8 x 10-5) 3. 4. What is the pH of a 1.15 M solution of methanoic acid? K = 1.8 × 10-4 What is the pH of a 0.350 M solution of lithium citrate? (K. Citric Acid = 7.4 x 10-) Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved. 5. SCH4U Unit 3 Assessment A 50.0 mL solution of 0.150 M acetic acid (CH COOH) is titrated with 0.150 M NaOH. What is the pH after 20.0 mL of base has been added? K. CH COOH = 1.8 x 10-5 4. Explain why the conjugate base of a strong acid can't react with water. Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved. 3 5. Why are some salts acidic when others are neutral? SCH4U Unit 3 Assessment Curriculum Expectation E2. investigate the qualitative and quantitative nature of chemical systems at equilibrium, and solve related problems. 1. Consider the following reaction: PCI (g)+ Cl₂ (g) PCI (g) K = 4.30 x 10-6 Initially, 2.50 M PCI, and 1.40 M Cl₂ are placed into a container and allowed to reach equilibrium. Determine the equilibrium concentrations of all the species.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 87SCQ: Most naturally occurring acids are weak acids. Lactic acid is one example....
Related questions
Question
![2.
Would you expect a solution of ammonium chloride (NHCI) to be acidic or basic
when added to water? (K NH = 1.8 x 10-5)
3.
4.
What is the pH of a 1.15 M solution of methanoic acid? K = 1.8 × 10-4
What is the pH of a 0.350 M solution of lithium citrate? (K. Citric Acid = 7.4 x 10-)
Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved.
5.
SCH4U
Unit 3 Assessment
A 50.0 mL solution of 0.150 M acetic acid (CH COOH) is titrated with 0.150 M NaOH.
What is the pH after 20.0 mL of base has been added? K. CH COOH = 1.8 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F633dc666-1c4e-4222-82a0-1d910c7662c5%2F0fd1627e-4f3e-4f74-bd21-5cb86fcb0d17%2Fk73mdsi_processed.png&w=3840&q=75)
Transcribed Image Text:2.
Would you expect a solution of ammonium chloride (NHCI) to be acidic or basic
when added to water? (K NH = 1.8 x 10-5)
3.
4.
What is the pH of a 1.15 M solution of methanoic acid? K = 1.8 × 10-4
What is the pH of a 0.350 M solution of lithium citrate? (K. Citric Acid = 7.4 x 10-)
Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved.
5.
SCH4U
Unit 3 Assessment
A 50.0 mL solution of 0.150 M acetic acid (CH COOH) is titrated with 0.150 M NaOH.
What is the pH after 20.0 mL of base has been added? K. CH COOH = 1.8 x 10-5
![4.
Explain why the conjugate base of a strong acid can't react with water.
Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved.
3
5. Why are some salts acidic when others are neutral?
SCH4U
Unit 3 Assessment
Curriculum Expectation E2. investigate the qualitative and quantitative nature of chemical
systems at equilibrium, and solve related problems.
1.
Consider the following reaction:
PCI (g)+ Cl₂ (g)
PCI (g)
K = 4.30 x 10-6
Initially, 2.50 M PCI, and 1.40 M Cl₂ are placed into a container and allowed to
reach equilibrium. Determine the equilibrium concentrations of all the species.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F633dc666-1c4e-4222-82a0-1d910c7662c5%2F0fd1627e-4f3e-4f74-bd21-5cb86fcb0d17%2Fvxorqja_processed.png&w=3840&q=75)
Transcribed Image Text:4.
Explain why the conjugate base of a strong acid can't react with water.
Copyright © 2021 The Ontario Educational Communications Authority. All rights reserved.
3
5. Why are some salts acidic when others are neutral?
SCH4U
Unit 3 Assessment
Curriculum Expectation E2. investigate the qualitative and quantitative nature of chemical
systems at equilibrium, and solve related problems.
1.
Consider the following reaction:
PCI (g)+ Cl₂ (g)
PCI (g)
K = 4.30 x 10-6
Initially, 2.50 M PCI, and 1.40 M Cl₂ are placed into a container and allowed to
reach equilibrium. Determine the equilibrium concentrations of all the species.
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