ZuoTi.Pro
Question

The acid dissociation constant Ka equals 1.26 x 10-2 for HSO4- and is 5.6 x 10-10...

The acid dissociation constant Ka equals 1.26 x 10-2 for HSO4- and is 5.6 x 10-10 for NH4+. Which statement about the following equilibrium is correct?
HSO4-(aq) + NH3(aq) = SO4 2-(aq)+ NH4+(aq)
a. The reactants will be favored because ammonia is a stronger base than the sulfate anion.
b. The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion.
c. Neither reactants nor products will be favored because all of the species are weak acids or bases.
d. The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made.
e. This reaction is impossible to predic, since the strong acid and the weak base appear on the sma eside of the equation.
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1
answer is b. The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion.
0 0
Add a comment
Answer #2

The answer is:

b. The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion.

Stronger acid has higher tendency to donate H+ than weaker acid

=> reaction will shift to right

=> products favored

0 0
Add a comment
Know the answer?
Add Answer to:
The acid dissociation constant Ka equals 1.26 x 10-2 for HSO4- and is 5.6 x 10-10...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • which acid is the strongest ? Hydrogen sulfate ion HS04– (Ka = 1.2 x 10-2 Hydrofluoric...

    which acid is the strongest ? Hydrogen sulfate ion HS04– (Ka = 1.2 x 10-2 Hydrofluoric acid HF (Ka = 7.2 x 10-4) Hydrocyanic acid HCN (Ka = 4.9 10–10, O Ammonium ion NH4" (ka = 5.6 10-10

  • When ammonium sulfate dissolves, both the anion and cation have acid-base reactions: (NH4)2SO4(s) ⇄ 2NH4+ +...

    When ammonium sulfate dissolves, both the anion and cation have acid-base reactions: (NH4)2SO4(s) ⇄ 2NH4+ + SO42- Ksp = 276 NH4+ ⇄ NH3(aq) + H+ Ka = 5.7x10-10 SO42- + H2O ⇄ HSO4- + OH- Kb = 9.8x10-13 a. Write charge balance and mass balances b. Compute the concentration of NH3(aq) if pH is 9.25

  • HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is...

    HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.055 M in A-(aq)? The temperature is 25oC.

  • 17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a...

    17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...

  • 12. Given that Ka = 1.8 x 10- for acetic acid. in order for an acetic...

    12. Given that Ka = 1.8 x 10- for acetic acid. in order for an acetic acid solution to have a pH of 3.50, its molar concentration must be a. 5.7 x 10-3 M b. 5.6 x 10-3M c. 3.2 x 10-4M d. 2.3 x 10-M 13. If enough base is added to a solution to cause the pH to increase from 7.50 to 8.50, this means that А a. [OH-] increases by a factor of 10 b. [H'] increases...

  • (a) HA (aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11....

    (a) HA (aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a 0.061 M solution in A- (aq)? The temperature is 25oC. (b) For the reaction A (g) ⇋ B (g) + C (g), the equilibrium constant is 1.80 at 25.0oC and 4.46 at 75.0oC. Making the approximation that ΔH and ΔS do not change with temperature, calculate the value of the equilibrium constant at 50.0oC as well as the...

  • If the dissociation constant of a weak acid is 6.4 x 10, at what ratio should...

    If the dissociation constant of a weak acid is 6.4 x 10, at what ratio should you adjust the concentration of the weak acid and its conjugate base in ord a) 0.0500 M weak acid with 0.100 M conjugate base b) 0.100 M weak acid with 0.0100 M conjugate base c)0.500 M weak acid with 0.500 M conjugate base d) 0.0500 M weak acid with 0.500 M conjugate base e) 0 200 M weak acid with 0.100 M conjugate base...

  • (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What...

    (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.066 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.36 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.

  • (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What...

    (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.065 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.00 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC

  • (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What...

    (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.068 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.95 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT