9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? a. 3.2 x 10² M d. 3.2 x 10³ M b. 3.2 x 10³ M c. 3.2 x 104 M 10. A 2.5 M solution of which of the following weak acids would be the most acidic? a. formic acid b. hydrofluoric acid c. hydrocyanic acid d. hydrosulfuric acid 11. A solution made from the dissolving of which of the following salts in water would a. potassium carbonate (K₂CO3) be acidic? b. sodium nitrate (NaNO3) c. calcium fluoride (CaF₂) d. ammonium chloride (NH4Cl) 12. Of the four fluorate oxyacids, which would have the lowest K, value? d. HFO4 b. HFO₂ c. HFO3 a. HFO

9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? a. 3.2 x 10² M d. 3.2 x 10³ M b. 3.2 x 10³ M c. 3.2 x 104 M 10. A 2.5 M solution of which of the following weak acids would be the most acidic? a. formic acid b. hydrofluoric acid c. hydrocyanic acid d. hydrosulfuric acid 11. A solution made from the dissolving of which of the following salts in water would a. potassium carbonate (K₂CO3) be acidic? b. sodium nitrate (NaNO3) c. calcium fluoride (CaF₂) d. ammonium chloride (NH4Cl) 12. Of the four fluorate oxyacids, which would have the lowest K, value? d. HFO4 b. HFO₂ c. HFO3 a. HFO

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 191MP

See similar textbooks

Similar questions

Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
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.
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH], and the pH for this solution. [Hint: Concentrated HCl is 38% HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO3 is 70.% HNO3 (by mass) and has a density of 1.42 g/mL.
A 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000
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.
Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution of HNO3(d=1.00g/mL). What is the pH of 10.0 mL of the same sample? (b) A solution made up of 1.0 g of HCI dissolved in enough water to make 1.28 L of solution. What is the pH of the solution? If the same mass of HCI is dissolved in enough water to make 128 mL of solution, what would the pH be?