How to solve no. 2 One key to predicting the relative strength of an acid is to look at its conjugate base and judge its slubility.is the stronger Bronsted-Lowry acid in cach pair?1.With this in mind, which(a) H,0 or H0(b) H20 orOH(c) HIO or HIO(d) HCL or HE(e) H SO, or HSO,2.The active component of aspirin is acetylsalicylic acid, HC,H704, which has a Ka of 3.0 x 10-4.(a) Calculate the pH of a solution made by dissolving 0.500 g (500 mg) of acetylsalicylic acid in water and diluting to s0.0 mL.(b) Repeat the calculation, assuming that the some mass of acetylsalicylic acid is dissolved and diluted to 1000.0 mL of solution.(c) Is the pH lower or higher in the mere dilute solution? Which solution has a higher fraction of its acetylsalicylic acid ionized?3. Papaverine hydrochloride (papHCI), a salt of a weak base and a strong acid, s a drug used as a muscle relaxant. It is a250 C, a 0.205 M solution of papHCI has a pH of 3.31. Compute the K, of papHCL.weak acid. At

2) Given: Ka of HC9C7O4 = 2.0 × 10-4 a) Given: Mass of HC9C7O4 = 0.500 g. And volume of solution =…

2. The active component of aspirin is acetylsalicylic acid, HC,H,0., which has a K. of 3.0 x 10-4 (a) Calculate the pH of a solution made by dissolving 8.500 g (500 mg) of acetylsalicylic acid in water and diluting to se.e mL. (b) Repeat the calculation, assuming that the some mass of acetylsalicylic acid is dissolved and diluted to 1900.e mL of solution. (c) Is the pH lower or higher in the mere dilute solution? Which solution hos a higher fraction of its acetylsalicylic acid ionized?

2. The active component of aspirin is acetylsalicylic acid, HC,H,0., which has a K. of 3.0 x 10-4 (a) Calculate the pH of a solution made by dissolving 8.500 g (500 mg) of acetylsalicylic acid in water and diluting to se.e mL. (b) Repeat the calculation, assuming that the some mass of acetylsalicylic acid is dissolved and diluted to 1900.e mL of solution. (c) Is the pH lower or higher in the mere dilute solution? Which solution hos a higher fraction of its acetylsalicylic acid ionized?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen...

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Similar questions

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
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
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
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?
Codeine, C23H21NO3, is an alkaloid (Kb = 6 2 109) used as a painkiller and cough suppressant. A solution of codeine is acidified with hydrochloric acid to pH 4.50. What is the ratio of the concentration of the conjugate acid of codeine to that of the base codeine?
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
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
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
Is the conjugate base of a weak acid a strong base? Explain. Explain why Cl does not affect the pH of an aqueous solution.
White vinegar is a 5.0% by mass solution of acetic acid in water. If the density of white vinegar is 1.007 g/cm3, what is the pH?