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). а. 0.0704 М СНЗСОСООН b.0.0704 M CH3NH3CI С. 0.0704 М 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). а. 0.0704 М СНЗСОСООН b.0.0704 M CH3NH3CI С. 0.0704 М 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)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.33QAP

See similar textbooks

Similar questions

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)?
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.
Calculate the pH of a solution prepared by mixing 49.0 mL of butyric acid, HC4H7O2, with 6.15 g of KOH in water. The following data about butyric acid may be helpful: density=0.9595g/mL;K a =1.54105
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
Calculate the pH of a solution made up from 2.0 g of potassium hydroxide dissolved in 115 mL of 0.19 M perchloric acid. Assume the change in volume due to adding potassium hydroxide is negligible.
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?
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.