Suppose a particular water sample is known to have pH = 8.34 and [HCO3-] = 183 mg/L. (a) Estimate or calculate the molar concentrations of HCO3-, H+, OH-, H2CO3, and CO3²-. Hint: yes, you have enough information to do these calculations. (b) Suppose that the only other ion present in the water is sodium, Na+. Estimate or calculate the molar concentration of Na+ that would be required to ensure charge neutrality in the water: [Na+] + [H+] = [OH-] + [HC03-] + 2[CO3²-]. (c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity as normality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinity in the text book if we don't get to it in class. (d) Repeat parts (a)–(c) if the pH is 8.34 (as it was before), but now the concentration
Suppose a particular water sample is known to have pH = 8.34 and [HCO3-] = 183 mg/L. (a) Estimate or calculate the molar concentrations of HCO3-, H+, OH-, H2CO3, and CO3²-. Hint: yes, you have enough information to do these calculations. (b) Suppose that the only other ion present in the water is sodium, Na+. Estimate or calculate the molar concentration of Na+ that would be required to ensure charge neutrality in the water: [Na+] + [H+] = [OH-] + [HC03-] + 2[CO3²-]. (c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity as normality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinity in the text book if we don't get to it in class. (d) Repeat parts (a)–(c) if the pH is 8.34 (as it was before), but now the concentration
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter15: Acids And Bases
Section: Chapter Questions
Problem 15.20QP: Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq)...
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
![8.34 and [HCO3-] = 183
Suppose a particular water sample is known to have pH
mg/L.
(a) Estimate or calculate the molar concentrations of HCO3¬, H+, OH-, H,CO3, and
CO32-. Hint: yes, you have enough information to do these calculations.
(b) Suppose that the only other ion present in the water is sodium, Na+. Estimate or
calculate the molar concentration of Na+ that would be required to ensure charge
neutrality in the water: [Na+] + [H+] = [OH-] + [HCO3-] + 2[CO32-].
(c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity as
normality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinity
in the text book if we don't get to it in class.
(d) Repeat parts (a)-(c) if the pH is 8.34 (as it was before), but now the concentration
of bicarbonate is [HCO3-] = 30 mg/L.
(e) Now suppose you have two beakers. In the first beaker, you put 99 mL of the first
water sample (183 mg/L bicarbonate) and you add 1 mL of hydrochloric acid (HCI).
The concentration of the HCl (before addition to the water sample) is 0.1 M, which
is also equal to 0.1 N. In the second beaker, you put 99 mL of the second water
sample (30 mg/L bicarbonate) and you add 1 mL of HCl. You allow both mixtures
to equilibrate, and then you measure the pH in both beakers. What do
you think
you will see? Why? Hint: it is possible to actually calculate the pH in each beaker,
but that is a pretty complicated calculation, and it is beyond the scope of ENV 4001;
try for a qualitative answer here. Will the pH go up or down in the first beaker? By
a little or by a lot? Why? What about in the second beaker? Why?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff966c414-4cbd-409b-9db4-c8010e535c33%2Ff8015601-33cc-4db0-ab6b-76cd52daf07f%2Fxwgbc41_processed.png&w=3840&q=75)
Transcribed Image Text:8.34 and [HCO3-] = 183
Suppose a particular water sample is known to have pH
mg/L.
(a) Estimate or calculate the molar concentrations of HCO3¬, H+, OH-, H,CO3, and
CO32-. Hint: yes, you have enough information to do these calculations.
(b) Suppose that the only other ion present in the water is sodium, Na+. Estimate or
calculate the molar concentration of Na+ that would be required to ensure charge
neutrality in the water: [Na+] + [H+] = [OH-] + [HCO3-] + 2[CO32-].
(c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity as
normality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinity
in the text book if we don't get to it in class.
(d) Repeat parts (a)-(c) if the pH is 8.34 (as it was before), but now the concentration
of bicarbonate is [HCO3-] = 30 mg/L.
(e) Now suppose you have two beakers. In the first beaker, you put 99 mL of the first
water sample (183 mg/L bicarbonate) and you add 1 mL of hydrochloric acid (HCI).
The concentration of the HCl (before addition to the water sample) is 0.1 M, which
is also equal to 0.1 N. In the second beaker, you put 99 mL of the second water
sample (30 mg/L bicarbonate) and you add 1 mL of HCl. You allow both mixtures
to equilibrate, and then you measure the pH in both beakers. What do
you think
you will see? Why? Hint: it is possible to actually calculate the pH in each beaker,
but that is a pretty complicated calculation, and it is beyond the scope of ENV 4001;
try for a qualitative answer here. Will the pH go up or down in the first beaker? By
a little or by a lot? Why? What about in the second beaker? Why?
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 5 images
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
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
