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 e) none of the above
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 e) none of the above
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46ef3182-b77b-4d5e-aa39-bd37ce4fcd02%2Ffcd82a95-78fa-40f7-8d3e-92e5d8616528%2Fh0z9ikec_processed.jpeg&w=3840&q=75)
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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