Question

What are the concentrations of HSO4−, SO42−, and H+ in a 0.21 M KHSO4 solution? (Hint:...

What are the concentrations of HSO4−, SO42−, and H+ in a 0.21 M KHSO4 solution? (Hint: H2SO4 is a strong acid; Ka for HSO4− = 1.3 × 10−2.)

Homework Answers

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
What are the concentrations of HSO4−, SO42−, and H+ in a 0.25 M KHSO4 solution? (Hint:...
What are the concentrations of HSO4−, SO42−, and H+ in a 0.25 M KHSO4 solution? (Hint: H2SO4 is a strong acid; Ka for HSO4− = 1.3 × 10−2.) [ HSO4− ] = M [ SO42− ] = M [ H+ ] = M
Be sure to answer all parts. Calculate the concentrations of H2SO4, HSO4−, SO42− and H3O+ ions...
Be sure to answer all parts. Calculate the concentrations of H2SO4, HSO4−, SO42− and H3O+ ions in a 0.15 M sulfuric acid solution at 25°C (Ka2 for sulfuric acid is 1.3 × 10−2.) [H2SO4] M [HSO4−] M [SO42−] M [H3O+]
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid....
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as H2SO4?H++HSO4? A HSO4? anion can dissociate further by HSO4??H++SO42? but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as Ka2=[H+][SO42?][HSO4?]=0.012 Part A Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid....
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid....
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as H2SO4?H++HSO4? A HSO4? anion can dissociate further by HSO4??H++SO42? but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as Ka2=[H+][SO42?][HSO4?]=0.012 Part A Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid....
Calculate the concentration of H2SO4, HSO4-, SO4-2 and H+ ions in a 0.17 M sulfuric acid...
Calculate the concentration of H2SO4, HSO4-, SO4-2 and H+ ions in a 0.17 M sulfuric acid solution. Assume H+ and H3O+ to be the same ions. Ka2 = 1.3 x 10^-2.
1. Calculate the [H+]-, [HSO4-]- and [SO 42-] - ion concentrations and the pH of a...
1. Calculate the [H+]-, [HSO4-]- and [SO 42-] - ion concentrations and the pH of a 0.050 M H2SO4. Ka1 is very large and Ka2 is 0.012. 2. Write equations to show how you would make: a) NaHSO4 b) Na2SO4 c) NaHCO3
1) What is the ph of a 0.005 M , solution of h2so4? ka2=1.2x10^-2 of HSo4-
1) What is the ph of a 0.005 M , solution of h2so4? ka2=1.2x10^-2 of HSo4-
What color will the solution be if we add H2SO4 to the K2CrO4 solution? H2SO4 (aq)...
What color will the solution be if we add H2SO4 to the K2CrO4 solution? H2SO4 (aq) ----> H+ (aq) + HSO4- (aq) HSO4- (aq) ---> H+(aq) + SO42- (aq) How does increasing the concentration of H+ affect the chromate/dichromate equilibrium? What color will the solution be? What if we add NaOH to the solution? How does it affect the equillibrium? What does OH- react with in the solution? What color will the solution be?
Weak acids partially dissociate in solution and establish equilibrium with H+ HA ⇌ H+ + A-...
Weak acids partially dissociate in solution and establish equilibrium with H+ HA ⇌ H+ + A- The equilibrium constant, called Ka, is a measure of the extent of the dissociation and the strength of the weak acid.                               Calculate the concentration of H+, [H+], in the following acid solutions. 1.      0.2 M HF, Ka = 7.2 × 10-4 2.      0.2 M CH3COOH, Ka = 1.8 × 10-5 3.      0.2 M HCN, Ka = 6.2 × 10-10 4.      0.2 M HCl...
Determine the concentrations of K2SO4, K+ , and SO42– in a solution prepared by dissolving 1.71...
Determine the concentrations of K2SO4, K+ , and SO42– in a solution prepared by dissolving 1.71 × 10–4 g K2SO4 in 2.50 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). [Note: Determine the formal concentration of SO42–. Ignore any reactions with water.] [K2SO4] = ________M [K+] = ________M        = ________ppm [SO42–] = ________M              = ________ppm