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
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...
Related questions
Question
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
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.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY