Question

What is the pH of a 0.20 M solution of disodium hydrogen phosphate? Ka2 ​ =...

What is the pH of a 0.20 M solution of disodium hydrogen phosphate? Ka2 ​ = 6.2 x 10^- 8and Ka3 ​ = 2.2 x 10^-1 3

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
a) What is the pH of 0.10 M NaH2PO4? Ka2 = 6.2 x 10-8 b) What...
a) What is the pH of 0.10 M NaH2PO4? Ka2 = 6.2 x 10-8 b) What is the pH of 0.10 M Na2​HPO4? Ka3 = 2.2 x 10-13
a) A solution containing 0.0267 M maleic acid and 0.038 M disodium maleate. The Ka values...
a) A solution containing 0.0267 M maleic acid and 0.038 M disodium maleate. The Ka values for maleic acid are 1.20 × 10-2 (Ka1) and 5.37 × 10-7 (Ka2). b) A solution containing 0.0345 M succinic acid and 0.021 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 × 10-5 (Ka1) and 2.31 × 10-6 (Ka2).
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
2The acid-dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 × 10-3, Ka2 = 6.2...
2The acid-dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.2 × 10-13 at 25.0 °C. What is the molar concentration of phosphate ion in a 2.5 M aqueous solution of phosphoric acid? A) 0.13 B) 2.5 × 10-5 C) 8.2 × 10-9 D) 9.1 × 10-5 E) 2.0 × 10-19 Can you include the complete steps where Ka2 and Ka3 is used.
Another buffer found in blood is based on the equilibrium between dihydrogen phosphate and monohydrogen phosphate....
Another buffer found in blood is based on the equilibrium between dihydrogen phosphate and monohydrogen phosphate. The reaction is shown below: H2PO4^-(aq) + H2O(l)----> H3O^+(aq) + HPO4^-2(aq) If the pH of a blood sample was 7.10, what would you calculate as the ratio of (H2PO4^-) to (HPO4^-2)? (Ka1 = 7.5*10^-3, Ka2 = 6.2*10^-8, Ka3 = 3.6*10^-13)
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of 0.50 M HCl to 53 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of 0.46 M HCl to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of 0.46 M NaOH to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Show how phosphoric, H3PO4, dissociates in water and calculate the pH of a 0.030 M solution...
Show how phosphoric, H3PO4, dissociates in water and calculate the pH of a 0.030 M solution of the acid. Ka1 = 7.5 x 10-3; K a2 = 6.2 x 10-8; Ka3 = 4.8 x 10-13
Phosphoric acid is a triprotic acid, and the Ka values are given below. Calculate pH, pOH,...
Phosphoric acid is a triprotic acid, and the Ka values are given below. Calculate pH, pOH, [H3PO4], [H2PO4 2-], [HPO4 -], and [PO4 3-] at equilibrium for a 5.00 M phosphoric acid solution. Ka1 = 7.5 x 10^-3 Ka2 = 6.2 x 10^-8 Ka3 = 4.2 x 10^-13
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT