Question

Calculate the quotient [H3PO4]/[H2PO4] in 0.05 M K2HPO4. K1= 7.11x10^-3, K2= 6.32x10^-8, K3=4.17x10^-3​

Calculate the quotient [H3PO4]/[H2PO4] in 0.05 M K2HPO4. K1= 7.11x10^-3, K2= 6.32x10^-8, K3=4.17x10^-3​

Homework Answers

Answer #1

HPO42-   ---------------> H+   +   PO43-

0.05                                0            0

0.05 - x                            x             x

ka3 = x^2 / 0.05 - x

4.17 x 10^-13 = x^2 / 0.05 - x

x = 1.44 x 10^-7

[H+] = 1.44 x 10^-7 M

H3PO4   -------------> H+ + H2PO4-

Ka1 = [H+][H2PO4-] / [H3PO4]

7.11 x 10^-3 = [H2PO4-] x 1.44 x 10^-7 / [H3PO4]

[H2PO4-] / [H3PO4] = 49241.6

[H3PO4] / [H2PO4-] = 2.03 x 10^-5

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
(a) Calculate the quotient [H3PO4]/[H2PO4− ] in 0.0463 M KH2PO4. (Assume Kw = 1.01 ✕ 10−14,...
(a) Calculate the quotient [H3PO4]/[H2PO4− ] in 0.0463 M KH2PO4. (Assume Kw = 1.01 ✕ 10−14, Ka1 = 7.11 ✕ 10−3, Ka2 = 6.34 ✕ 10−8, and Ka3 = 4.22 ✕ 10−13.)  
Question 2.  Calculate the F-obtained value using the below table K1 K2 K3 K4 X X-squared X...
Question 2.  Calculate the F-obtained value using the below table K1 K2 K3 K4 X X-squared X X-squared X X-squared X X-squared 6 8 12 18 6 10 12 18 8 10 16 22 8 12 16 22 12 18 Total Total Total Total Total Total Total Total X̅1= X̅2= X̅3= X̅4=
Calculate the pH and the equilibrium concentrations of H2PO4-, HPO42- and PO43- in a 0.0353 M...
Calculate the pH and the equilibrium concentrations of H2PO4-, HPO42- and PO43- in a 0.0353 M aqueous phosphoric acid solution. For H3PO4, Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13 pH = ? [H2PO4-] = ?M [HPO42-] = ?M [PO43-] = ?M
What is the [H2PO4-] of a solution labeled "0.10 M Phosphoric Acid (H3PO4)"? [Ka1 = 7.1x10-3;...
What is the [H2PO4-] of a solution labeled "0.10 M Phosphoric Acid (H3PO4)"? [Ka1 = 7.1x10-3; Ka2 = 6.3x10-8; Ka3 = 4.2x10-13] A. 4.2x10-13 M B. 2.7x10-2 M C. 7.1x10-3 M D. 1.6x10-9 M E. 1.6x10-16 M
The formal composition of an aqueous solution is 0.12 M K2HPO4 + 0.08 KH2PO4. The pKa's...
The formal composition of an aqueous solution is 0.12 M K2HPO4 + 0.08 KH2PO4. The pKa's for triprotic phosphoric acid are 2.12, 7.21, and 12.32. Show the three equilibriums in solution and calculate the pH of the solution. Find concentrations of K+, H3PO4, H2PO4^-, HPO4^2-, PO4^3-, H+, and OH^- in the mixture.
Given the following Ka values: H3PO4 <--> H2PO4- + H+, Ka = 7.11*10-3 H2PO4- <--> HPO42-...
Given the following Ka values: H3PO4 <--> H2PO4- + H+, Ka = 7.11*10-3 H2PO4- <--> HPO42- + H+, Ka = 6.34*10-8 HPO42- <--> PO43- + H+, Ka = 4.22*10-13, a) please calculate the pH of the solution at the first equivalence point for the above titration. b) In the same titration as described above, what's the pH of the solution after 15.00 mL of NaOH was added?
4. Consider the following sequence of first order reactions: k1 k2 O → M → G...
4. Consider the following sequence of first order reactions: k1 k2 O → M → G Where k1 = 2.50 × 1011 s -1 and k2 = 5.20 × 1010 s -1 a. At what time in seconds will the maximum concentration of M occur? (3 points) b. If [O]0 = 2.00 M, what will [G] be 9.50 × 10-12 s after the reaction is initiated? (4 points)
Determine the pH of a 0.0520 M solution of the following salts. A table of pertinent...
Determine the pH of a 0.0520 M solution of the following salts. A table of pertinent K values is found to the right. a) NaHCO3 b) NaH2PO4 acid formula K1 k2 k3 arsenic acid H3AsO4 5.8e-3 1.1e-7 3.2e-12 carbonic acid H2CO3 4.45e-7 4.69e-11 hydrogen sulfide H2S 9.6e-8 1.3e-14 phosphoric acid H3PO4 7.11e-3 6.32e-8 4.5e-13
Part A: Given the two reactions H2S⇌HS−+H+,   K1 = 9.51×10−8, and HS−⇌S2−+H+,   K2 = 1.33×10−19, what is the...
Part A: Given the two reactions H2S⇌HS−+H+,   K1 = 9.51×10−8, and HS−⇌S2−+H+,   K2 = 1.33×10−19, what is the equilibrium constant Kfinal for the following reaction? S2−+2H+⇌H2S Part B: Given the two reactions PbCl2⇌Pb2++2Cl−,   K3 = 1.83×10−10, and AgCl⇌Ag++Cl−,   K4 = 1.20×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2+2Ag+⇌2AgCl+Pb2+
Calculate the concentrations of all species in a 0.180-M solution of H2X if K1 = 5.01E-05...
Calculate the concentrations of all species in a 0.180-M solution of H2X if K1 = 5.01E-05 and K2 = 2.82E-08 [H2X] = M [H3O1+] = M [HX1-] = M [X2-] = M