Q 3 please Q1:Chose the correct answer from the following1- the [H] concentration for the solution that result from addition of 40.0 ml of 0.10 M KOH to 50ml of 0.3 M of HCI.a) 0.0667 M. b) 1.00 x 10-7c) 0.12 Md) 1.50 x 10-13 M2-What is the pH of 500 mL of solution containing 0.0124 grams of Ca(OH)₂?c) 2.96d) 3.17a) 11.04 b) 9.68e) 10.83M3- What was the pH of the solution that result from addition of 30 ml of 0.1 M hydrochloric acid to25.0 ml of 0.5 M solution of weak base (Kb=9.74×106 ).?a. 5.10c. 8.494- A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate K, for the acid.a) 3.8 x 10b) 6.5 x 10-7c) 7.0 x 10-6d) 4.2 x 10-6e) 3.5 x 10-8b. 4.92a-e) none of the aboved. 9.085- How many grams of sodium acetate will adde to sufficient amount of 0.1 M solution of acetic acidto makin 100 ml of buffer solution with pH= 4.1(Mw of sodium acetate is 82 g/mole andKa acetic acid is 1.75×10)2.27 gb- 0.34 gc- 0.180 gd- 4.76 g6- If 15.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then theconcentration of HNO3 in ppm is: [M.wt. of HNO,= 63 g/mol]c) 7.30 × 10³ ppmd) 18.77 × 10³ ppmb) 14.70 x10³ ppma) 9.45×10³ppma) 3.647. Which of the following is true about a 0.10 M solution of a weak acid, HX?a) [X] = 0.10 Mb) pH = 1c) [HX] > [H]d) [H] = 0.10 M8-. What is the pH of 0.060 M NH4CI? (NH3 Kb = 3.98 x10-¹0)b) 5.12a) 5.06c) 5.18d) 5.24c) 4.58e. 8.72e) 5.359- Calculate the pH that results when the following solutions are mixed.( Ka of formic acid is 3 x10¹)(1) 35 mL of 0.20 M formic acid(2) 55 mL of 0.10 M sodium formate(3) 110 mL of waterb) 3.11d) 3.3910-What is the pH of a buffer solution where [HA] = [A-]?a. pH = 1b. pH = pOHc. pH = Kae) both b and de) 4.20d. pH = 7.0e. pH = pk a

Given, Volume of HCl = 30 ml Molarity of HCl = 0.1 M The volume of a solution of weak base = 25.0 ml…

Q1:Chose the correct answer from the 1- the [H] concentration for the solution that result from addition of 40.0 ml of 0.10 M KOH to 50 ml of 0.3 M of HCI. a) 0.0667 M b) 1.00 x 10-7 M c) 0.12 M d) 1.50 x 10-13 M 2-What is the pH of 500 mL of solution containing 0.0124 grams of Ca(OH)₂? c) 2.96 d) 3.17 a) 11.04 b) 9.68 e) 10.83 e) none of the above 3- What was the pH of the solution that result from addition of 30 ml of 0.1 M hydrochloric acid to 25.0 ml of 0.5 M solution of weak base (Kb = 9.74×10% ).? b. 4.92 c. 8.49 d. 9.08 e. 8.72

Q1:Chose the correct answer from the 1- the [H] concentration for the solution that result from addition of 40.0 ml of 0.10 M KOH to 50 ml of 0.3 M of HCI. a) 0.0667 M b) 1.00 x 10-7 M c) 0.12 M d) 1.50 x 10-13 M 2-What is the pH of 500 mL of solution containing 0.0124 grams of Ca(OH)₂? c) 2.96 d) 3.17 a) 11.04 b) 9.68 e) 10.83 e) none of the above 3- What was the pH of the solution that result from addition of 30 ml of 0.1 M hydrochloric acid to 25.0 ml of 0.5 M solution of weak base (Kb = 9.74×10% ).? b. 4.92 c. 8.49 d. 9.08 e. 8.72

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.36QE

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