12. Carbonated water has a [H+Jeg = 3.2 × 10-4 M; this is the result of thedissociation of carbonic acid:H₂CO3 (ag)H+ (aq) + HCO3- (ag)Kc = 4.4 x 10-7a. Set up the equilibrium constant expression for this acid dissociation.b. Calculate [H₂CO₂]ea. Hint: An ICE table may be handy.c. Carbonic acid is created by dissolving carbon dioxide in water. Given that theHenry's Law constant of carbon dioxide is 29.76 atm/M, what partial pressureof carbon dioxide is needed to make carbonated water?

a. The equilibrium constant expression for the acid dissociation reaction of carbonic acid is: Kc =…

12. Carbonated water has a [H+Jeg = 3.2 × 10-4 M; this is the result of the dissociation of carbonic acid: H₂CO3 (ag) H+ (aq) + HCO3- (aq) Kc = 4.4 x 10-7 a. Set up the equilibrium constant expression for this acid dissociation. b. Calculate [H₂CO3]ea. Hint: An ICE table may be handy. c. Carbonic acid is created by dissolving carbon dioxide in water. Given that the Henry's Law constant of carbon dioxide is 29.76 atm/M, what partial pressure of carbon dioxide is needed to make carbonated water?

12. Carbonated water has a [H+Jeg = 3.2 × 10-4 M; this is the result of the dissociation of carbonic acid: H₂CO3 (ag) H+ (aq) + HCO3- (aq) Kc = 4.4 x 10-7 a. Set up the equilibrium constant expression for this acid dissociation. b. Calculate [H₂CO3]ea. Hint: An ICE table may be handy. c. Carbonic acid is created by dissolving carbon dioxide in water. Given that the Henry's Law constant of carbon dioxide is 29.76 atm/M, what partial pressure of carbon dioxide is needed to make carbonated water?

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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Calculate [CO32] in a 0.010-M solution of CO2 in water (usually written as H2CO3). If all the CO32 in this solution comes from the reaction HCO3(aq)H+(aq)+CO32(aq) what percentage of the H+ ions in the solution is a result of the dissociation of HCO3? When acid is added to a solution of sodium hydrogen carbonate (NaHCO3), vigorous bubbling occurs. How is this reaction related to the existence of carbonic acid (H2CO3) molecules in aqueous solution?
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
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.
Composition diagrams, commonly known as alpha plots, are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown here. The plot shows how the fraction [alpha ()] of acetic acid in solution, =[CH3CO2H][CH3CO2H]+[CH3CO2] changes as the pH increases (blue curve). (The red curve shows how the fraction of acetate ion, CH3CO2, changes as the pH increases.) Alpha plots are another way of viewing the relative concentrations of acetic acid and acetate ion as a strong base is added to a solution of acetic acid in the course of a titration. (a) Explain why the fraction of acetic acid declines and that of acetate ion increases as the pH increases. (b) Which species predominates at a pH of 4, acetic acid or acetate ion? What is the situation at a pH of 6? (c) Consider the point where the two lines cross. The fraction of acetic acid in the solution is 0.5, and so is that of acetate ion. That is, the solution is half acid and half conjugate base; their concentrations are equal. At this point, the graph shows the pH is 4.74. Explain why the pH at this point is 4 74.
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