MasteringChemistry: CHE154 X + session.masteringchemistry.com/myct/itemView?assignmentProbiemID=14296684 CHE154-H Gen Chem I CHE154 S20 Ch17 Sec5-6 chapter 17 Multiple Choice Question 42 Part A Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10°. 4.52 9.48 5.48 11.74 2.26 Submit Request Answer Provide Feedback II

MasteringChemistry: CHE154 X + session.masteringchemistry.com/myct/itemView?assignmentProbiemID=14296684 CHE154-H Gen Chem I CHE154 S20 Ch17 Sec5-6 chapter 17 Multiple Choice Question 42 Part A Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10°. 4.52 9.48 5.48 11.74 2.26 Submit Request Answer Provide Feedback II

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 34Q: Which of the following statements is(are) true? Correct the false statements. a. When a base is...

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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.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Consider the process H2O H+(aq)+OH(aq)H=55.8kJ (a) Will the pH of pure water at body temperature (37C) be 7.0? (b) If not, calculate the pH of pure water at 37C.
The indicator dinitrophenol is an acid with a Ka of 1.1104. In a 1.0104 -M solution, it is colorless in acid and yellow in base. Calculate the pH range over which it goes from 10% ionized (colorless) to 90% ionized (yellow).
Which of the following statements is(are) true? Correct the false statements. a. When a base is dissolved in water, the lowest possible pH of the solution is 7.0. b. When an acid is dissolved in water, the lowest possible pH is 0. c. A strong acid solution will have a lower pH than a weak acid solution. d. A 0.0010-M Ba(OH)2 solution has a pOH that is twice the pOH value of a 0.0010-M KOH solution.
You mix a solution of a strong acid with a pH = 4.0 and an equal volume of another strong acid solution having a pH = 6.0. Is the final pH less than 4.0, equal to 4.0, between 4.0 and 5.0, equal to 5.0, between 5.0 and 6.0, equal to 6.0, or greater than 6.0? Explain.
Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the ratio [C5H5N]/[C5H5NH+] if the solution has the following pH values: a. pH = 4.50 b. pH = 5.00 c. pH = 5.23 d. pH = 5.50
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)?
Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30
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