(aq) K, = =1.5x 10 [H,Co, (a)] HCO, (aq) + H;O0) co? (aq) + H.O(aq) (aq) 4.69 x 10 [HCo, (n What is the equilibrium constant for this reaction? CO.(aq) + 2H,0(1) HCO, (aq) + H,O (aq) K-? (A) K x Ki (B) Kux K: (C) Ku/Ka (D) Ku/ K. . Which equation represents the charge balance equation for the dissolution of CaCO, in aqueous solution. (A) (Ca']- [HCO, 1+[CO1 (B) 2(Ca] + [H')-[OH ]+ 2[CO, ) (C) [Ca"] + [H']= [OH ]+ [HCO, 1+[CO? ] (D) 2(Ca"] + (H")- [OH ]+ (HCO; 1+ 2[CO) ). In the dissociation of a monoprotic weak acid in aqueous solutions, HA, which leads to the assumption that (H']= (A? (A) The autoprotolysis of water is the dominant source of (H'). (B) The concentration of the acid is sufficiently high such that the dissociation of the acid is the dominant source of (H"). (C) The concentration of the acid has no effect on the approximation; [H'] is always approximately equal to (A). (D) The anion, A is also a weak base. 1. The pK, value for formic acid (HCOOH) is 3.74. Calculate the pH of a 0.25 M solution of sodium formate, the conjugate base of formic acid. Assume the activity coefficients are equal to 1.00. (A) 2.18 (B) 5.43 (C) 8.57 (D) 11.82
(aq) K, = =1.5x 10 [H,Co, (a)] HCO, (aq) + H;O0) co? (aq) + H.O(aq) (aq) 4.69 x 10 [HCo, (n What is the equilibrium constant for this reaction? CO.(aq) + 2H,0(1) HCO, (aq) + H,O (aq) K-? (A) K x Ki (B) Kux K: (C) Ku/Ka (D) Ku/ K. . Which equation represents the charge balance equation for the dissolution of CaCO, in aqueous solution. (A) (Ca']- [HCO, 1+[CO1 (B) 2(Ca] + [H')-[OH ]+ 2[CO, ) (C) [Ca"] + [H']= [OH ]+ [HCO, 1+[CO? ] (D) 2(Ca"] + (H")- [OH ]+ (HCO; 1+ 2[CO) ). In the dissociation of a monoprotic weak acid in aqueous solutions, HA, which leads to the assumption that (H']= (A? (A) The autoprotolysis of water is the dominant source of (H'). (B) The concentration of the acid is sufficiently high such that the dissociation of the acid is the dominant source of (H"). (C) The concentration of the acid has no effect on the approximation; [H'] is always approximately equal to (A). (D) The anion, A is also a weak base. 1. The pK, value for formic acid (HCOOH) is 3.74. Calculate the pH of a 0.25 M solution of sodium formate, the conjugate base of formic acid. Assume the activity coefficients are equal to 1.00. (A) 2.18 (B) 5.43 (C) 8.57 (D) 11.82
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 44PS
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Question
18. Given these equilibrium expressions for the dissolution of CO2 gas in water: CO2(aq)+H2O(1) H2CO3(aq) H2CO3(aq)+ H2O(1)HCO3(aq) + H3O*(aq)
![(ag)
K, =
=1.5x 10
HCO: (aq) + H,O(I) co? (aq) + H:0 (aq)
2
(aq)
(aq)
-4.69 x 10
[HCo, (na]
What is the equilibrium constant for this reaction?
CO.(aq) + 2H;0(1) HCO, (aq) + H;O (aq) K=?
(A) K x Ki
(B) K x K2
(C) Ku/K.
(D) Kn/ K.
19. Which equation represents the charge balance equation
for the dissolution of CaCO, in aqueous solution.
(A) [Ca] = [HCO,1+ [CO 1
(B) 2[Ca*]+ [H'] =[OH]+ 2[CO;)
(C) [Ca]+ [H']= [OH 1 + [HCO,]+ [CO? ]
(D) 2[Ca*]+ [H']= [0H ]+ [HCO; ]+ 2[CO; ]
20. In the dissociation of a monoprotic weak acid in aqueous
solutions, HA, which leads to the assumption that
[H]= [A]?
(A) The autoprotolysis of water is the dominant source
of (H').
(B) The concentration of the acid is sufficiently high
such that the dissociation of the acid is the dominant
source of [H'].
(C) The concentration of the acid has no effect on the
approximation; [H'] is always approximately equal
to [A).
(D) The anion, A is also a weak base.
21. The pK, value for formic acid (HCOOH) is 3.74.
Calculate the pH of a 0.25 M solution of sodium formate,
the conjugate base of formic acid. Assume the activity
coefficients are equal to 1.00.
(A) 2.18
(B) 5.43
(C) 8.57
(D) 11.82
2007 ACS DIVCHED Examinations Institute](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F924eceec-b61f-4e0e-ac19-069b52d93b97%2Fd603b85a-1c15-4ebe-8e7f-ed1c5f39112c%2Fhbi0nh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(ag)
K, =
=1.5x 10
HCO: (aq) + H,O(I) co? (aq) + H:0 (aq)
2
(aq)
(aq)
-4.69 x 10
[HCo, (na]
What is the equilibrium constant for this reaction?
CO.(aq) + 2H;0(1) HCO, (aq) + H;O (aq) K=?
(A) K x Ki
(B) K x K2
(C) Ku/K.
(D) Kn/ K.
19. Which equation represents the charge balance equation
for the dissolution of CaCO, in aqueous solution.
(A) [Ca] = [HCO,1+ [CO 1
(B) 2[Ca*]+ [H'] =[OH]+ 2[CO;)
(C) [Ca]+ [H']= [OH 1 + [HCO,]+ [CO? ]
(D) 2[Ca*]+ [H']= [0H ]+ [HCO; ]+ 2[CO; ]
20. In the dissociation of a monoprotic weak acid in aqueous
solutions, HA, which leads to the assumption that
[H]= [A]?
(A) The autoprotolysis of water is the dominant source
of (H').
(B) The concentration of the acid is sufficiently high
such that the dissociation of the acid is the dominant
source of [H'].
(C) The concentration of the acid has no effect on the
approximation; [H'] is always approximately equal
to [A).
(D) The anion, A is also a weak base.
21. The pK, value for formic acid (HCOOH) is 3.74.
Calculate the pH of a 0.25 M solution of sodium formate,
the conjugate base of formic acid. Assume the activity
coefficients are equal to 1.00.
(A) 2.18
(B) 5.43
(C) 8.57
(D) 11.82
2007 ACS DIVCHED Examinations Institute
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