a Following are three organic acids and the pK, of each: MOPS, 7.20; TRIS, 8.30; and PIPES, 6.80. What is the Ką of each acid? Ką( MOPS ) = K( TRIS ) = Ką( PIPES) = | Which of the three is the strongest acid, and which is the weakest? The strongest is = The weakest is = | b What information do you need to predict which of the three acids would require the most NaOH to reach a phenolphthalein end point? (Select all that apply.) O the basicity of each acid | the amount of each acid | atmosphere pressure | the molarity of NaOH | temperature the amount of phenolphthalein

a Following are three organic acids and the pK, of each: MOPS, 7.20; TRIS, 8.30; and PIPES, 6.80. What is the Ką of each acid? Ką( MOPS ) = K( TRIS ) = Ką( PIPES) = | Which of the three is the strongest acid, and which is the weakest? The strongest is = The weakest is = | b What information do you need to predict which of the three acids would require the most NaOH to reach a phenolphthalein end point? (Select all that apply.) O the basicity of each acid | the amount of each acid | atmosphere pressure | the molarity of NaOH | temperature the amount of phenolphthalein

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

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4. The pH of 1.50 mol/L acid is measured to be 5.75. For this acid, the Ka is 10-5.25 = [H₂₂0] A. 2.1 x 10-¹2 B. 1.8 x 10-6 C. 2.4 x 10-6 D. very large Chatz (H30] = 1.77x10-6 = 1,8x10-6 In the following information to answer the next question.
8. 200 mL of 0.7M LİOH is titrated with 1.0 M CH,COOH. Ka of acetic acid is 1.8 x 10 i. find the final pH of the solution at equivalence point. (ANS: 8.99) ii. The titration process was stopped at equivalence point. 200 mL of 0.5M CH,COOH was further added into the mix. Please calculate the new pH. (ANS: 4.9)
3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts) Reaction of sodium propionate in water: Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq) Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert ka to Kb. You can assume that the sodium propionate dissociates completely from the propionate and is not involved in any other important reactions. a) Is this the conjugate base or an acid that you are adding to solution? b) Write down the Mass-Balance Relations, the Proton Balance Relation and the c) Equilibrium Relation. Calculate the pH using both an analytic method, and by drawing the predominance diagram. *Hint* [OH-]=[HPr].
5.) What is K, for an acid whose pK, is 3.78?
(a) Calculate the percent lonization of 0.00820 M hydrosulfuric acid (K,- 9.5e-08). % lonization - % (b) Calculate the percent lanization of 0.00820 M hydrosulfuric acid in a solution containing 0.0810 M sodium hydrogen sulfate. % lonization = %
A weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?
Calculate the K, value for the following acids. (Enter your answer to three significant figures.) a) Acrylic acid (pK₂ = 4.25): b) Bicarbonate ion (pK, 10.25):
Calculate the concentration of each species present in a 0.025 M solution of phthalic acid, C6H4(CO2H)2. C6HĄ(CO2H),(aq) + H,O(1) = H;0*(aq) +C6H4(CO2H)(CO2)¯(aq) Ką=1.1×10-3 CoH4(CO,H)(CO2)-(aq)+ HzO(1)= H30*(aq) + CgHq(CO2),²-(aq) Ką=3.9x 10-6
The following results were collected for % sodium carbonate in asample: 4.2, 4.4, 4.9, 4.0, 6.4, 4.3 and 4.1%. The result 29.4% seemsquestionable, if the tabulated Q = 0.568, should it be retained orrejected?Select one or more:The value 6.4 should be omitted (rejected)The calculated Q = 0.625The value 6.4 should be retainedthe calculated Q = 1.6
(6) 0.8203 g NaAc (FW=82.03 g/mol) was fully dissolved into 100.00 mL of 0.050 M HAc solution. Calculate th pH of the soolution.
You dissolve 5.3 g of ascorbic acid (MW 176; pk 4.2, 11.6) in 150 mL of water. When the solution comes to equilibrium, what is the pH?