Arsenic acid dissociates to form dihydrogen arsenate and hydronium ion. Arsenic acid has Ka of 5.5 x 10-3.  a.) Write the equation for dissociation of arsenic acid. Express your answer as a chemical equation. Identify all of the phases in your answer. b.) What is the dissociation constant expression for arsenic acid?

12. Carbonated water has a [H+Jeg = 3.2 × 10-4 M; this is the result of the dissociation of carbonic acid: H₂CO3 (ag) H+ (aq) + HCO3- (ag) Kc = 4.4 x 10-7 a. Set up the equilibrium constant expression for this acid dissociation. b. Calculate [H₂CO₂]ea. Hint: An ICE table may be handy. c. Carbonic acid is created by dissolving carbon dioxide in water. Given that the Henry's Law constant of carbon dioxide is 29.76 atm/M, what partial pressure of carbon dioxide is needed to make carbonated water?

Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12

A 1.00 liter solution contains 0.23 M acetic acid and 0.30 M potassium acetate. If 0.150 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) +A. The number of moles of CH3COOH will remain the same. + B. The number of moles of CH3COO" will remain the same. C. The equilibrium concentration of H30* will remain the same. + D. The pH will remain the same. E. The ratio of [CH3COOH]/[CH;COO"] will decrease.

← Aktiv Chemistry → C + X app.aktiv.com C The equations below show the x + Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. RbClO 1 + ■ Reset + 2 3 NR Rb U □2 ☐ 3 OC ) 4 0 A Question 20 of 20 O H LO 5 05 + 0²+ 6 7 8 07 = (s) (1) CI 3+ H₂O+ 4+ • x H₂O 9 0 ☐9 口。 (g) (aq) H₂O OH Delete OT Update: Submit

6. Open the bags and add 3 drops of bromothymol blue to each bottle. The indicator turns yellow if vinegar is still present and is blue-green when vinegar is not present. Record the color of each solution in the table provided. Data Table 1: Reaction Data Sample 7. Add a 4 teaspoon of baking soda to each bag. Effervescence of CO₂ occurs if excess vinegar is present. Record your observations in the table provided. Moles of vinegar (mol) Moles of baking soda (mol) mistry Relative size of bag Was excess vinegar present? Color with indicator? Reacts with additional baking soda? Moles of gas produced (mol) Watch the limiting reagent! #1 0.042 0.014 чем yes yellow #2 0.042 0.028 #3 yes yellow 0.042 0.042 Experiment 11 yes yellow #4 Stoichiometry 0.042 0.88 more small big bigger bigger No 0.071 #5 NO Geen 0.042 Blue Calculations 1. Use Table 1 to determine which reactant was limiting in each trial. Use the amount of limiting reactant to calculate the moles of carbon dioxide gas that were…

13a.

Show all pertinent computations A. The solubility of ferric hydroxide is 4.8 x 10° g/100 ml at room temperature. Calculate its solubility product constant.

Material from chapters 13, 14, 15 A saturated aqueous solution of Ca(OH)2 is prepared (Ksp=4.68 x 10). a. Classify Ca(OH)2 as strong acid, weak acid, strong base, or weak base. b. Is the boiling point of this solution greater than, less than, or the same as pure water? C. Write the solubility product equilibrium constant expression and determine the equilibrium concentration of the (OH-]. d. What is the pH of this solution? e. This solution is used in a titration of HCO2H. Wha is the conjugate of HCO2H formed? f. 150. mL of HCO2H solution of unknown concentration is titrated with 650. mL of the Ca(OH)2 solution when endpoint is reached. What is the original concentration of HCO2H? Material from chapter 12, 15 2 NO2 (g) → N½O4 (g) a. Is this endothermic or exothermic? 6. AH = -57.23 kJ/mol b. If 5 mols of NO2 react, what is the amount of energy absorbed? c. What intermolecular forces are present in NO2 (g)? d. Write the equilibrium constant expression. e. How does the equilibrium shift…

Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)