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...
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