Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid?  (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .

At 50 °C, the ion-product constant for H2O has the valueKw = 5.48 x 10-14. (a) What is the pH of pure water at50 °C? (b) Based on the change in Kw with temperature,predict whether ΔH is positive, negative, or zero for theautoionization reaction of water:2 H2O(l) ⇌ H3O+(aq) + OH-(aq)

Even though both NH3 and C6H5NH2 are weak bases, NH3 is a much stronger acid than C6H5NH2. Which of the following is correct at equilibrium for a solution that is initially 0.10 M in NH3 and 0.10 M in C6H5NH2?(a) [OH−] = [NH4+](b) [NH4+] = [C6 H5 NH3+](c) [OH−] = [C6 H5 NH3+](d) [NH3] = [C6H5NH2](e) both a and b are correct

Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. CH:NH:CI(aq) + NaOH(aq) 4- 2+ | ]3+ 1 3 4 6 7 8 D4 15 Do ) (s) (1) (g) (aq) Na H C CI Reset • x H2O Delete 1L 2. +

Draw the structures of the conjugate bases of the following acids: (a) COO I CH || HC (c) I COOH COO™ I H-C-H NH (b) (d) COOH H-C-H NH COO™ H-C-CH₂-COOH NH

The Ka of a weak acid is 5.42 x 10-5. What is the pKb of its conjugate base?

Give the conjugate acid of the following Bronsted-Lowry bases. (Type your answer using the format [OH]- for OH.) (a) F HF (b) HASO2- (c) H₂PO4 (d) C₂H₂0₂ x X X

ANALYTICAL CHEMISTRY MIDTERM ASSIGNMENT NO. 3 (BY GROUP) A. Identify the acid (acid1) on the left side and conjugate base (basel) on the right side. (a) HOCI + H,O=H,0* + OCI¯ (b) HONH, + H,0 HONH + OH (c) NH + H,0NH3 + H;O* (d) 2HCO, H,CO, + CO (e) PO + H,PO, 2HPO} B. Identify the base (base2) on the left side and conjugate acid ( acid2) on the right side. (a) HOCI + H,0=H,0* + OCI (b) HONH2 + H0 HONH + OH- (c) NH + H,0=NH, + H;O* (d) 2HCO, =H,CO, + CO (e) PO + H,PO, 2HPO} C. Calculations: 1. What is the concentration of hydronium ion in a 0.100 M solution of HCl? 2. What is the hydroxide concentration in the solution described in item 1? 3. What is the value of pH described in item 1? 4. Is the solution acidic or basic (refer to #3)? 5. Calculate the pH of water at 75 °C. Kw of water at 75 °C is 19.9 x 1014.

Calculate the pH of a solution containing 0.20 M CH3COOH and 0.30 M CH;COONA. [Ka CH3COOH = 1.8 x 1051 8. (a) 4.9 (b) Calculate the pH of the 0.20 M CH3COOH solution if there is no salt present. [Ka CH3COOH = 1.8×10-°] 2.7 (c) Explain the change in pH the solution in (a) when i. a small amount of strong acid is added. ii. a small amount of strong base is added.

6. Draw two graphs for weak acid HA: (a) percent dissociation for HA versus the initial concentration of HA ([HA]o) (hint: assume [HA], as x and [H*]/[HA], as y). (b) the equilibrium concentration of H+ versus [HA]o. Explain both.