(a) Interpretation:
Examine for the following given equations and answer the questions
The value of K1 and K2
Concept Introduction: Equilibrium mass action expression is the ratio of the concentration of product and reactant when equilibrium is attained. Let us consider a general equation:-
Answer to Problem 12.27PAE
Solution:
Explanation of Solution
Using the formula
we can calculate the values of equilibrium constants for both the reactions:-
For the second reaction:
(b) Interpretation:
Examine for the following given equations and answer the questions
The equation by adding the given two equations
Concept Introduction: Equilibrium mass action expression is the ratio of the concentration of product and reactant when equilibrium is attained. Let us consider a general equation:-
Answer to Problem 12.27PAE
Solution:
The overall reaction is
Explanation of Solution
Overall reaction (Sum of both reactions) is given below:-
Hence, this is the result.
This is the overall reaction.
(c) Interpretation:
Examine for the following given equations and answer the questions
The equilibrium constant for the overall equation.
Concept Introduction: Equilibrium mass action expression is the ratio of the concentration of product and reactant when equilibrium is attained. Let us consider a general equation:-
Answer to Problem 12.27PAE
Solution:
Explanation of Solution
The new equilibrium constant for the overall equation is:-
Want to see more full solutions like this?
Chapter 12 Solutions
Chemistry for Engineering Students
- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forwardMost naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.arrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forward
- At 25 oC, Ammonia is a weak base that reacts with water according to this equation: NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq) Briefly explain how the equilibrium will shift (to get back to equilibrium) if the following perturbations are made to the system: (a) Addition of HCl (b) Addition of NaOH (c) Addition of NH4Clarrow_forwardA weak acid, HA, is a monoprotic acid. A solution that is 0.140 Min HA has a pH of 1.800 at 25°C. HA(aq) + H,0(1) 2 H;0"(aq) + A (aq) What is the acid-ionization constant, K, for this acid? What is the degree of ionization of the acid in this solution? Ka- Degree of ionization =arrow_forwarda) What is the equilibrium constant for HF(aq) ⇌ H+ (aq) + F– (aq)?, b) is it Homogenous or Heterogenous?arrow_forward
- Write the equilibrium constant expression for this reaction: CH;Cl(aq)+OH (aq) → CH;OH(aq)+Cl (aq)arrow_forwardGiven 0.01 M solutions of each of the following acids, which solution would have the lowest pH? -117 Hypoiodous acid (HOI), K = 2.3 x 10 Hypobromous acid (HOBr), K = 2.5 x 10 Lactic acid (HC₂H₂O₂), K = 1.3 x 10 Chlorous acid (HClO₂), K = 1.1 x 10²arrow_forwardWrite the concentration equilibrium constant expression for this reaction. HCN(aq)+OH (aq)→CN (aq)+H,O(1)arrow_forward
- A chemical system is set up by placing some solid ammonium chloride in an ammonia solution. The equilibrium established can be represented as follows: NH4*(aq) + H2O(e) 2 H30*(aq) + NH3(aq) The pH of the solution is taken, then a small amount of NaOH(aq) is added and the pH is taken again. What can be said about the change in pH for the solution? The pH significantly increases because a strong base has been added to the solution. The pH significantly decreases because a strong base has been added to the solution. There is very little change to the pH of the solution. If anything the pH of the solution decreases slightly. There is very little change to the pH of the solution. If anything the pH of the solution increases slightly.arrow_forwardhelp pleasearrow_forward7arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning