Homework Help is Here – Start Your Trial Now!
Science
Chemistry
1. The four chemical reactions which occur in sequence when gaseous carbon dioxide dissolves in water is represented as follows: (1) In the first reaction, CO2 dissolves in water to give carbonic acid, represented as follows: CO2 + H2O → H2CO3 (carbonic acid) This is a reversible reaction, so that a state of equilibrium is achieved where some CO, and water molecules combine to form H2CO3, while at the same time, an equal number of H2CO3 molecules split into CO2 and water. (ii) In the second reaction, H2CO3 is a weak acid, some of its molecules dissociate into bicarbonate ion and hydrogen ion and the reaction is reversible: H2CO, → H* + HCO;- (bicarbonate) (iii) Third reaction is the dissociation of bicarbonate ion to carbonate ion: HCO;- → H* + CO;²- (carbonate) (iv) The carbonate ion reacts with excess hydrogen ions to produce bicarbonate: Co,?- + 2H* → 2HCO;- (bicarbonate) 2. Carbon dioxide is not an acid by itself since it does not contain H+ ions but become acidic when carbon dioxide dissolves in water. This is because, carbonic acid (weak acid) is formed from which hydrogen ions dissociate, increasing the acidity of the carbon dioxide solution. The reaction is represented as follows: CO2 + H2O → H2CO3 (carbonic acid) If OH- (from a strong base such as sodium hydroxide) is added to a solution of carbon dioxide, what happens to the OH- and what effect will this have on the equilibria you wrote above?

1. The four chemical reactions which occur in sequence when gaseous carbon dioxide dissolves in water is represented as follows: (1) In the first reaction, CO2 dissolves in water to give carbonic acid, represented as follows: CO2 + H2O → H2CO3 (carbonic acid) This is a reversible reaction, so that a state of equilibrium is achieved where some CO, and water molecules combine to form H2CO3, while at the same time, an equal number of H2CO3 molecules split into CO2 and water. (ii) In the second reaction, H2CO3 is a weak acid, some of its molecules dissociate into bicarbonate ion and hydrogen ion and the reaction is reversible: H2CO, → H* + HCO;- (bicarbonate) (iii) Third reaction is the dissociation of bicarbonate ion to carbonate ion: HCO;- → H* + CO;²- (carbonate) (iv) The carbonate ion reacts with excess hydrogen ions to produce bicarbonate: Co,?- + 2H* → 2HCO;- (bicarbonate) 2. Carbon dioxide is not an acid by itself since it does not contain H+ ions but become acidic when carbon dioxide dissolves in water. This is because, carbonic acid (weak acid) is formed from which hydrogen ions dissociate, increasing the acidity of the carbon dioxide solution. The reaction is represented as follows: CO2 + H2O → H2CO3 (carbonic acid) If OH- (from a strong base such as sodium hydroxide) is added to a solution of carbon dioxide, what happens to the OH- and what effect will this have on the equilibria you wrote above?

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...
See similar textbooks
icon
Related questions
Question
1. The four chemical reactions which occur in sequence when gaseous carbon dioxide dissolves in water is represented as follows: (i) In the first reaction, CO, dissolves in water to give carbonic acid, represented as follows: CO2 + H20 → H2CO3 (carbonic acid) This is a reversible reaction, so that a state of equilibrium is achieved where some CO, and water molecules combine to form H2CO3, while at the same time, an equal number of H2CO3 molecules split into CO2 and water. (ii) In the second reaction, H2CO3 is a weak acid, some of its molecules dissociate into bicarbonate ion and hydrogen ion and the reaction is reversible: H2CO3 + H+ + HCO3- (bicarbonate) (iii) Third reaction is the dissociation of bicarbonate ion to carbonate ion: НСО-- + н* + со)3- (сarbonate) (iv) The carbonate ion reacts with excess hydrogen ions to produce bicarbonate: CO,?- + 2H+ → 2HСО,-- (bicarbonate) 2. Carbon dioxide is not an acid by itself since it does not contain H+ ions but become acidic when carbon dioxide dissolves in water. This is because, carbonic acid (weak acid) is formed from which hydrogen ions dissociate, increasing the acidity of the carbon dioxide solution. The reaction is represented as follows: CO2 + H20 → H2CO3 (carbonic acid) If OH (from a strong base such as sodium hydroxide) is added to a solution of carbon dioxide, what happens to the OH- and what effect will this have on the equilibria you wrote above?
Transcribed Image Text:1. The four chemical reactions which occur in sequence when gaseous carbon dioxide dissolves in water is represented as follows: (i) In the first reaction, CO, dissolves in water to give carbonic acid, represented as follows: CO2 + H20 → H2CO3 (carbonic acid) This is a reversible reaction, so that a state of equilibrium is achieved where some CO, and water molecules combine to form H2CO3, while at the same time, an equal number of H2CO3 molecules split into CO2 and water. (ii) In the second reaction, H2CO3 is a weak acid, some of its molecules dissociate into bicarbonate ion and hydrogen ion and the reaction is reversible: H2CO3 + H+ + HCO3- (bicarbonate) (iii) Third reaction is the dissociation of bicarbonate ion to carbonate ion: НСО-- + н* + со)3- (сarbonate) (iv) The carbonate ion reacts with excess hydrogen ions to produce bicarbonate: CO,?- + 2H+ → 2HСО,-- (bicarbonate) 2. Carbon dioxide is not an acid by itself since it does not contain H+ ions but become acidic when carbon dioxide dissolves in water. This is because, carbonic acid (weak acid) is formed from which hydrogen ions dissociate, increasing the acidity of the carbon dioxide solution. The reaction is represented as follows: CO2 + H20 → H2CO3 (carbonic acid) If OH (from a strong base such as sodium hydroxide) is added to a solution of carbon dioxide, what happens to the OH- and what effect will this have on the equilibria you wrote above?
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Chemical Equilibrium
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.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS