A. 0.0614 M solution of butyric acid, C₂H,COOH is 0.066% ionized. a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures. [C₂H₂COOH] = [H₂0']=[ (C₂H₂COO] = b) What is the pH of the acidic solution? c) What is K, of the acid? 02.68-10 M M M 06.09-108 pH= 02.57-10 00.0613 01.01-10 0

A. 0.0614 M solution of butyric acid, C₂H,COOH is 0.066% ionized. a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures. [C₂H₂COOH] = [H₂0']=[ (C₂H₂COO] = b) What is the pH of the acidic solution? c) What is K, of the acid? 02.68-10 M M M 06.09-108 pH= 02.57-10 00.0613 01.01-10 0

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.65PAE

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Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
One of the most challenging parts of solving acidbase problems is writing out the correct equation. When a strong acid or a strong base is added to solutions, they are great at what they do, and we always react them first. If a strong acid is added to a buffer, what reacts with the H+ from the strong acid and what are the products? If a strong base is added to a buffer, what reacts with the OH from the strong base and what are the products? Problems involving the reaction of a strong acid or strong base are assumed to be stoichiometry problems and not equilibrium problems. What is assumed when a strong acid or strong base reacts to make it a stoichiometry problem?
Ascorbic acid (H, C,H,0,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and K„2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. 2.49 pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O,] = 0.131 M [HC,H,0G] = 3.22 x10-3 M 7.18 x10 -8 [C,H,O; = M Incorrect
Ascorbic acid (H,C,H,O,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 × 10-5 and Ka2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O] = M [HC,H,0] = M [C,H,0;-] = M
Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH3 CH;NH2 C¿H5NH2 C,H;NH2 C3H;N 1.8 × 10-5 4.38 × 10-4 5.6 × 10-4 3.8 × 10-10 Ammonia Methylamine Ethylamine Aniline Pyridine NH, CH;NH;* C¿H5NH3* C¢H;NH;* C;H;NH+ 1.7 x 10-9 314. Compute the concentration of the weak base in Molarity (round off answer to 4 decimal places).
The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
C3H,NH, COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C;H,NH,C00", in a 5.0 x 10-2 M solution of the acid. The value of K, is 2.2 x 10-. Concentration of hydronium ion = M Concentration of para-aminobenzoate ion = M
Determine the pH of a solution of aspirin (acetylsalicylic acid, HC,H,O4) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of aspirin is 3.3 x 10-4. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) -X NEXT > 652 mg of aspirin (HC9H₂O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 15.3 - x 0 1 HCgH;O4(aq) 2.75 x 10-3+x 0.0153 + x 2.75 x 10-3 2.75 x 10-3-X 0.0153 - x + 2 H₂O(1) 3.62 x 10-³ 3.62 x 10-3+x = 1.53 x 10-5 3.62 x 10-3-x 3 H3O+ (aq) 15.3 1.53 x 10-5 + x 0.0153 + 1.53 x 10-5-x C9H₂O4 (aq) RESET +X 15.3 + x
Ascorbic acid (H,C, H,0,) is a diprotic acid. The acid dissocation constants for H,C. H,O, are K - 800 x 10 and Ka- 1.60 x 10-1 Determine the pH of a 0.138 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. (H,C,H,0, = M |HC, H,0;] - C,H,O-
ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 ml of 0.20 M HXp with 19.3 mlL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 uS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30, and Xp 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. K, 8. Ao
A solution is made by mixing exactly 500 mL of 0.156 M NaOH with exactly 500 mL of 0.100 MCH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8×10−5 [H+] M Enter your answer in scientific notation. [OH−] M [CH3COOH] M Enter your answer in scientific notation. [Na+] M [CH3COO−] M

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