25. Which of the following is usually considered to be a weak acid?A) HCIB) HBrC) HID) HF26. Which of the following acids is generally considered to be a strong acid?A) CH3COOHB) HNO3C) H2CO3D) HCO301.0 027. A solution has [H*] = 1.2 X 104. What is the pH of this solution?A) 3.92B) 8.3 X 10-11PHOOC) 10.08D) 1.0 X 10-1428. A solution has a pH = 4.50. What is its pOH?A) 4.50B) 9.50C) 3.2 X 105D) 3.1 X 1010 29. A solution of 0.0050 M HF would be expected to have a pH that is:A) lower than a solution of 0.0050 M HCI.B) the same as a solution of 0.0050 M HCl.C) higher than a solution of 0.0050 M HCI.D) impossible to compare to a solution of 0.0050 M HCIQuestions 30 and 31 both involve a 0.22 M solution of acetic acid (CH3COOH). TheKa of CH3COOH is 1.8 X 10S.30. What is the pH of 0.22 M CH3COOH?A) 0.66B) 4.74C) 0.10D) 2.7231. What is the percent ionization of 0.22 M CH3COOH?A) 0.20 %B) 0.75 %C) 0.86 %D) 100 %

Given: HCl, HI, HBr,HF To find: Weak acid among the given acids. Since you have asked multiple…

25. Which of the following is usually considered to be a weak acid? A) HCI B) HBr C) HI D) HF 26. Which of the following acids is generally considered to be a strong acid? A) CH3COOH B) HNO3 C) H2CO3 D) HCO3 27. A solution has [H*] = 1.2 X 104. What is the pH of this solution? A) 3.92 B) 8.3 X 10-11 PHO C) 10.08 5.0 (A D) 1.0 X 1014 28. A solution has a pH = 4.50. What is its pOH? A) 4.50 B) 9.50 CL 11X10:5

25. Which of the following is usually considered to be a weak acid? A) HCI B) HBr C) HI D) HF 26. Which of the following acids is generally considered to be a strong acid? A) CH3COOH B) HNO3 C) H2CO3 D) HCO3 27. A solution has [H*] = 1.2 X 104. What is the pH of this solution? A) 3.92 B) 8.3 X 10-11 PHO C) 10.08 5.0 (A D) 1.0 X 1014 28. A solution has a pH = 4.50. What is its pOH? A) 4.50 B) 9.50 CL 11X10:5

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 50A

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Similar questions

Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.
Compare the percent ionization of the base in Exercise 22a with the percent ionization of the base in Exercise 22d. Explain any differences.
For the following, mix equal volumes of one solution from Group I with one solution from Group II to achieve the indicated pH. Calculate the pH of each solution. Group I: 0.20 M NH4Cl, 0.20 M HCl, 0.20 M C6H5NH3Cl, 0.20 M (C2H5)3NHCl Group II: 0.20 M KOI, 0.20 M NaCN, 0.20 M KOCl, 0.20 M NaNO2 a. the solution with the lowest pH b. the solution with the highest pH c. the solution with the pH closest to 7.00
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.
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.