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
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...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
Q 3 please
![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%2Fb4881833-3d80-456d-87d2-40bbfb3f2e68%2Fvv50xjb_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
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY