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.

Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the dry texture of certain wines. Tartaric acid, H2C4H4O6, is a diprotic acid with the following Ką values: Ka1 = 1.00 x 10-3; Ka2 = 4.60 x 10-5 a. Write the equation for the 1st jonization of tartaric acid. b. Write the equation for the 2nd ionization of tartaric acid. c. Write the Ką expression for the 1st ionization. d. Write the Ką expression for the 2nd ionization. e. What is the equilibrium concentrations of the reactants and products from the 1st ionization of a 0.250M solution of tartaric acid? f. What is the equilibrium concentrations of the reactants and products from the 2nd ionization? g. What is the total [H30+] and the overall pH of the solution of tartaric acid?

Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the dry texture of certain wines. Tartaric acid, H₂C4H406, is a diprotic acid with the following Ka values: Kal = 1.00 x 10-³; K₁2 = 4.60 x 10-5 a. Write the equation for the 1st ionization of tartaric acid. b. Write the equation for the 2nd ionization of tartaric acid. c. Write the Ka expression for the 1st ionization. d. Write the Ka expression for the 2nd ionization. e. What is the equilibrium concentrations of the reactants and products from the 1st ionization of a 0.250M solution of tartaric acid? f. What is the equilibrium concentrations of the reactants and products from the 2nd ionization? g. What is the total [H3O+] and the overall pH of the solution of tartaric acid?

What is the pH of 0.80 M Hypobromite acid (HBrO) which is a weak acid? The Ka the wesk acid is 4.5 × 10 -8. Hint: [i]. M [C]. M [E]. M HBrO(aq) 0.80 -X 0.80 - X H+ (aq) + BrO - (aq) 0 0 +X +X Ka (X) (X) / 0.80-X = Hint: Solve for (X) = [H*]E X Then : [H+] at Equilibrium then PH = - Log [H* JE A. PH = 3.2 B. PH = 3.4 C.PH = 3.6 D.PH = 3.7 E.PH = 4.2