6. HOCI is an acid in aqueous solution with Ka = 3.49 x 10-8 at 25.0 °C a. Write the chemical equation for the ionization equilibrium of HOCI in water. Include physical states and appropriate charges. b. 0.35 mol of HOCI is added to 1L of water at 25.0 °C, calculate the pH of the resulting solution. c. Write the chemical equation for the ionization equilibrium of CIO™ in water. Include physical states.

6. HOCI is an acid in aqueous solution with Ka = 3.49 x 10-8 at 25.0 °C a. Write the chemical equation for the ionization equilibrium of HOCI in water. Include physical states and appropriate charges. b. 0.35 mol of HOCI is added to 1L of water at 25.0 °C, calculate the pH of the resulting solution. c. Write the chemical equation for the ionization equilibrium of CIO™ in water. Include physical states.

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...

See similar textbooks

Similar questions

Calculate the pH for each case in the titration of 50.0 mL of 0.120 M HC10(aq) with 0.120 M KOH(aq). Use the ionization constant for HC1O. What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH What is the pH after addition of 40.0 mL KOH? pH What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of 60.0 mL KOH? pH :
In the laboratory, a general chemistry student measured the pH of a 0.386 M aqueous solution of nitrous acid to be 1.865. Use the information she obtained to determine the Ka for this acid. Ka(experiment) = In the laboratory, a general chemistry student measured the pH of a 0.431 M aqueous solution of hydrofluoric acid to be 1.741. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
2. Dr. Dahm has prepared 250 mL of a acetate buffer which contains 0.1 mol of acetic acid (CH₂COOH) and 0.15 moles of acetate (CH₂COO). Determine the initial pH. If he then adds 0.025 moles of H* calculate the new pH. Ka = 1.8 × 10³ CH₂COOH(aq) + H₂O CH₂COO (aq) + HO (aq) 3. Dr. Dahm makes a second acetate buffer exactly the same way as in #2, but he then adds 15 mL of 0.50 M NaOH calculate the new pH.
8. A student conducts an acid-base titration to investigate the change in pH during a reaction between hydrochloric acid and ammonia solution. a. Name a piece of equipment that could be used to provide an accurate measurement of pH during the titration and explain how it would be calibrated. The student transfers 50cm3 of 1.0moldm3 ammonia solution acid into a beaker. During the titration the student adds 50cm3 1.00moldm³ hydrochloric acid from a burette into the beaker and records the pH throughout. b. Sketch the pH curve produced during this titration.
6. Consider the following equilibria: 1 Ca²+ (aq) + 2 OH- (aq) 2 ¹2 H₂O(1) H₂O*(aq) + OH-(aq) Ca(OH)₂(s) K=1.5 x 105 K = 1.0 x 10-14 Given these equilibria, what is the equilibrium constant, K, for the following reaction? 3: Ca(OH)2 (s) + 2 H3O*(aq) ≤ Ca²+ (aq) + 2 H₂O(1)
HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M
2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH COOH with 9.00 mL of 0.080 M NaOH. a. Calculate the moles of CH COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH₂COOH and CH COO present in the buffer solution. c. Calculate the concentration of CH COOH and CH COO in the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH COOH K₂ = 1.8 x 10.
Calculate the pH at 25 °C of a 0.44M solution of potassium butanoate (KC,H,CO,). Note that butanoic acid (HC,H,CO,) is a weak acid with a p K, of 4.82. Round your answer to 1 decimal place. pH = 0
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…
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B C D H₂O H₂O, NaOH H₂O H₂O, NaOH initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic оо 00 neutral change add HCl add Na Br add K Cl add H Br effect of change on pH (check one) pH higher pH lower ο ο1ο ο ο ο ο ο pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same
You are given a 0.250 M NO21 solution. a. Write the balanced chemical reaction of NO21 with water, including phase labels and correct charges. b. Using an ICE table, calculate the pH of this weak base solution. The Kb of NO21 is 2.16 · 10-11.