Write appropriate K expressions (including the value of the constant from Harris Appendix A or B) and fill out an ICE table (include chemical formulas in the column headers!). Find the pH to the nearest +0.001 units (3 significant digits). a. 0.0704 М СНЗСОСООН b. 0.0704 M CH3NH3CI c. 0.0704 M HBr d. 24.0 mL 0.0704 M HBr added to 25.0 mL 0.0704 M KOH (dilution) e. 0.0704 M HONH2 f. 0.0704 M NalO3 g. water with excess Co(OH)2(s) (solids don't belong in ice tables) h. water with excess Cu(OH)2(s) (solids don't belong in ice tables)

Write appropriate K expressions (including the value of the constant from Harris Appendix A or B) and fill out an ICE table (include chemical formulas in the column headers!). Find the pH to the nearest +0.001 units (3 significant digits). a. 0.0704 М СНЗСОСООН b. 0.0704 M CH3NH3CI c. 0.0704 M HBr d. 24.0 mL 0.0704 M HBr added to 25.0 mL 0.0704 M KOH (dilution) e. 0.0704 M HONH2 f. 0.0704 M NalO3 g. water with excess Co(OH)2(s) (solids don't belong in ice tables) h. water with excess Cu(OH)2(s) (solids don't belong in ice tables)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 191MP

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Similar questions

Water is accidentally added to 350.00 mL of a stock solution of 6.00 M HCI. A 75.00-mL sample of the diluted solution is titrated to pH 7.00 with 78.8 mL of 4.85 M NaOH. How much water was accidentally added? (Assume that volumes are additive.)
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Consider 1000. mL of a 1.00 104-M solution of a certain acid HA that has a Ka value equal to 1.00 104. How much water was added or removed (by evaporation) so that a solution remains in which 25.0% of HA is dissociated at equilibrium? Assume that HA is nonvolatile.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein