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2.27 g 6- If 15.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO concentration of HNO3 in ppm is: [M.wt. of HNO3= 63 g/mol] a) 9.45×10³ ppm b) 14.70 x10³ ppm c) 7.30 × 10³ ppm 010 M solution of a weak acid, HX? a- d) 18.77 × 10³ ppm

2.27 g 6- If 15.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO concentration of HNO3 in ppm is: [M.wt. of HNO3= 63 g/mol] a) 9.45×10³ ppm b) 14.70 x10³ ppm c) 7.30 × 10³ ppm 010 M solution of a weak acid, HX? a- d) 18.77 × 10³ ppm

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Q1:Chose the correct answer from the following 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 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 M 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=9.74×106 ).? a. 5.10 c. 8.49 4- A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate K, for the acid. a) 3.8 x 10 b) 6.5 x 10-7 c) 7.0 x 10-6 d) 4.2 x 10-6 e) 3.5 x 10-8 b. 4.92 a- e) none of the above d. 9.08 5- How many grams of sodium acetate will adde to sufficient amount of 0.1 M solution of acetic acid to makin 100 ml of buffer solution with pH= 4.1 (Mw of sodium acetate is 82 g/mole and Ka acetic acid is 1.75×10) 2.27 g b- 0.34 g c- 0.180 g d- 4.76 g 6- If 15.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in ppm is: [M.wt. of HNO,= 63 g/mol] c) 7.30 × 10³ ppm d) 18.77 × 10³ ppm b) 14.70 x10³ ppm a) 9.45×10³ ppm a) 3.64 7. Which of the following is true about a 0.10 M solution of a weak acid, HX? a) [X] = 0.10 M b) pH = 1 c) [HX] > [H] d) [H] = 0.10 M 8-. What is the pH of 0.060 M NH4CI? (NH3 Kb = 3.98 x10-¹0) b) 5.12 a) 5.06 c) 5.18 d) 5.24 c) 4.58 e. 8.72 e) 5.35 9- 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 water b) 3.11 d) 3.39 10-What is the pH of a buffer solution where [HA] = [A-]? a. pH = 1 b. pH = pOH c. pH = Ka e) both b and d e) 4.20 d. pH = 7.0 e. pH = pk a
Transcribed Image Text:Q1:Chose the correct answer from the following 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 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 M 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=9.74×106 ).? a. 5.10 c. 8.49 4- A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate K, for the acid. a) 3.8 x 10 b) 6.5 x 10-7 c) 7.0 x 10-6 d) 4.2 x 10-6 e) 3.5 x 10-8 b. 4.92 a- e) none of the above d. 9.08 5- How many grams of sodium acetate will adde to sufficient amount of 0.1 M solution of acetic acid to makin 100 ml of buffer solution with pH= 4.1 (Mw of sodium acetate is 82 g/mole and Ka acetic acid is 1.75×10) 2.27 g b- 0.34 g c- 0.180 g d- 4.76 g 6- If 15.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in ppm is: [M.wt. of HNO,= 63 g/mol] c) 7.30 × 10³ ppm d) 18.77 × 10³ ppm b) 14.70 x10³ ppm a) 9.45×10³ ppm a) 3.64 7. Which of the following is true about a 0.10 M solution of a weak acid, HX? a) [X] = 0.10 M b) pH = 1 c) [HX] > [H] d) [H] = 0.10 M 8-. What is the pH of 0.060 M NH4CI? (NH3 Kb = 3.98 x10-¹0) b) 5.12 a) 5.06 c) 5.18 d) 5.24 c) 4.58 e. 8.72 e) 5.35 9- 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 water b) 3.11 d) 3.39 10-What is the pH of a buffer solution where [HA] = [A-]? a. pH = 1 b. pH = pOH c. pH = Ka e) both b and d e) 4.20 d. pH = 7.0 e. pH = pk a
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