Question

IF HA IS A WEAK ACID, WHICK EQUILIBRIUM CORRESPONDS TO THE ACID EQUILIBRIUM CONSTANT Ka for...

IF HA IS A WEAK ACID, WHICK EQUILIBRIUM CORRESPONDS TO THE ACID EQUILIBRIUM CONSTANT Ka for Ha?

a. HA (aq) + H2O (l)<--->H2A+ (aq) + OH- (aq)

b. A- (aq) + H3O+ (aq)<---> HA (aq) + H2O (l)

c. HA (aq) + OH-(aq)<---> H2O (l) + H+ (aq)

d. A- (aq) +H2 O (l)<---> HA (aq) + OH- (aq)

e. A- (aq) + OH- (aq)<---> HOA2- (aq)

Homework Answers

Answer #1

Given, HA is a weak acid,

The equilibrium reaction for HA is,

HA(aq) + H2O(l) A-(aq) + H3O+(aq)

Since H3O+ species is present in the equilibrium reaction, We write the Acid equilibrium constant(Ka).

If we reverse the reaction,

A-(aq) + H3O+(aq) HA(aq) + H2O(l)

The Acid equilibrium constant value will inverse of the Ka but the value is the acid equilibrium constant.

Thus, Option (B) A-(aq) + H3O+(aq) HA(aq) + H2O(l) is the acid equilibrium constant for HA.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Given that Ka for the weak acid HA is 3.46 × 10–8, calculate K for the...
Given that Ka for the weak acid HA is 3.46 × 10–8, calculate K for the reaction of HA with OH–. HA(aq) + OH−(aq) ↔ A−(aq) + H2O(l)
0.250 moles of a weak acid, HA, is dissolved in pure water to make up 500...
0.250 moles of a weak acid, HA, is dissolved in pure water to make up 500 ml of a solution. As the HA dissolves, the following equilibrium is established: HA(aq) + H2O (l) = H3O+(aq) + A- (aq) K=3.5 * 10-5 (25 C) A). Calculate the concentrations of HA, H3O+, and A- present at equilibrium B). Calculate the pH of the solution at equilibrium.
A solution of a weak acid HA has initial concentration c and acid ionization constant Ka....
A solution of a weak acid HA has initial concentration c and acid ionization constant Ka. To what concentration should the acid be diluted to make [H3O+] half of what it was? Answer in terms of c and Ka.
1.Write the equilibrium constant expression (Ka) for the generic weak acid HA. HA(aq)⇌H+(aq) + A−(aq) 2.Write...
1.Write the equilibrium constant expression (Ka) for the generic weak acid HA. HA(aq)⇌H+(aq) + A−(aq) 2.Write the Henderson-Hasselbalch equation. 3.Given the Henderson-Hasselbalch equation, under what conditions does the pH= pKa? 4.Sketch a pH versus volume of base curve (a titration curve) for the titration of a weak acid with a strong base. On this sketch indicate the equivalence point and the point at which the conditions described in #3 are met. 5.When using a buret, do your results depend on...
The Ka constant of a weak acid always deals with the weak acid dissociating in water...
The Ka constant of a weak acid always deals with the weak acid dissociating in water to form H3O+ and the conjugate base of the weak acid. Write equilibrium reactions of the following weak acids in water and then write the corresponding Ka expressions in terms of concentrations of the weak acid, its conjugate base, and the conjugate acid of water, H3O+. HCN equilibrium Ka reaction____________________________________ Ka= HClO equilibrium Ka reaction____________________________________ Ka= HC2H3O2 equilibrium Ka reaction____________________________________ Ka= HNO2 equilibrium Ka...
Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq)...
Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq) + H3O+(aq) In a 0.200 M aqueous solution of HCNO, the concentration of H3O+ is 6.50 x 10-3M. The equilibrium constant (Kc) for this reaction is
Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq)...
Cyanic acid, HCNO, is a weak acid with the following equilibrium: HCNO(aq) + H2O(l) ⇌ CNO-(aq) + H3O+(aq) In a 0.200 M aqueous solution of HCNO, the concentration of H3O+ is 6.50 x 10-3M. The equilibrium constant (Kc) for this reaction is?
2. If an acid HA has a Ka value of 1.5 x 10-5, what will be...
2. If an acid HA has a Ka value of 1.5 x 10-5, what will be the value of equilibrium constant for the following reaction? Hint: You need to use Rxns 1 and 3 and Eqs 1 and 3 from the Background material. HA(aq) + OH-(aq) ↔ A-(aq) + H2O(l) Will this reaction be reactant favored or product favored? What does this tell you about the “completeness” of the titration reactions used in this laboratory?
The equilibrium constant, Ka, for the reaction below is 6.0*10^-3. Fe(H2O)6 ^3+ (aq) + H2O(l) <-->...
The equilibrium constant, Ka, for the reaction below is 6.0*10^-3. Fe(H2O)6 ^3+ (aq) + H2O(l) <--> Fe(H2O)5 (OH)^2+(aq) + H3O^+ (aq) a)Calculate the pH of the 0.10M solution of Fe(H2O)6^3+. b)Will a 1.0 M solution of iron (II) nitrate have a higher or lower pH than a 1.0 M solution of iron (III) nitrate?
Learning Goal: To understand the relation between the strength of an acid or a base and...
Learning Goal: To understand the relation between the strength of an acid or a base and its pKa and pKb values. The degree to which a weak acid dissociates in solution is given by its acid-ionization constant, Ka. For the generic weak acid, HA, HA(aq)⇌A−(aq)+H+(aq) and the acid-ionization constant is given by Ka=[A−][H+][HA] Similarly, the degree to which a weak base reacts with H2O in solution is given by its base-ionization constant, Kb. For the generic weak base, B, B(aq)+H2O(l)⇌BH+(aq)+OH−(aq)...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT