Question

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.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
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
Similar Questions
Given that the stepwise dissociation constants for phosphoric acid are: Ka1 = 7.5×10-3; Ka2 = 6.2×10-8;...
Given that the stepwise dissociation constants for phosphoric acid are: Ka1 = 7.5×10-3; Ka2 = 6.2×10-8; Ka3 = 4.8×10-13 To prepare 1.20 L of a buffer solution having an ionic strength of 0.150 and a pH of 7.50 would require: Answer to 3 sig figs. a) (mass) of Na2HPO4(anhydrous) and b) (mass) of NaH2PO4(anhydrous).
Calculate the pH of 0.103 M phosphoric acid (H3PO4, a triprotic acid). Ka1 = 7.5 x...
Calculate the pH of 0.103 M phosphoric acid (H3PO4, a triprotic acid). Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13. Hint, if you are doing much work, you are making the problem harder than it needs to be.
a.) Phosphoric acid is a triprotic acid: H3PO4(aq) +H2O(l) ↔ H3O+(aq) + H2PO4-(aq) Ka1 = 7.5...
a.) Phosphoric acid is a triprotic acid: H3PO4(aq) +H2O(l) ↔ H3O+(aq) + H2PO4-(aq) Ka1 = 7.5 x 10-3 H2PO4-(aq) +H2O(l) ↔ H3O+(aq) + HPO42-(aq) Ka2 = 6.2 x 10-8 HPO42-(aq) +H2O(l) ↔ H3O+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Determine whether sodium monohydrogen phosphate (Na2HPO4) is neutral, basic, or acidic. First, what is its Ka when it acts as an acid? b.) Second, what is its Kb when it acts as a base? c.) Finally, indicate whether the HPO42-...
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
Phosphoric acid is a triprotic acid (Ka1 = 6.9× 10–3, Ka2 = 6.2× 10–8, and Ka3...
Phosphoric acid is a triprotic acid (Ka1 = 6.9× 10–3, Ka2 = 6.2× 10–8, and Ka3 = 4.8× 10–13). To find the pH of a buffer composed of H2PO4–(aq) and HPO42–(aq), which pKa value would you use in the Henderson-Hasselbalch equation? A) pKa1= 2.16 B) pKa2=7.21 C) pKa3= 12.32 Calculate the pH of a buffer solution obtained by dissolving 24.0 g of KH2PO4(s) and 43.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.
phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of acid has 3 acidic...
phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of acid has 3 acidic protons. estimate the pH and concentration of all species in a .200 M phosphoric acid solution Ka1=6.9x10^-3, Ka2=602x10^-8, Ka3=4.8x10^-13
A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.48× 10–4 and Ka2 =...
A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.48× 10–4 and Ka2 = 3.21× 10–12. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below.(a) a 0.153 M solution of H2A.(b) a 0.153 M solution of NaHA.(c) a 0.153 M solution of Na2A
Which is the most prevalent species in a 0.25M aq solution of phosphoric acid, H3PO4? Ka1...
Which is the most prevalent species in a 0.25M aq solution of phosphoric acid, H3PO4? Ka1 = 7.5x10-3  , Ka2 = 6.2x10-8 , Ka3 = 4.2x10-13 a) H3PO4 b) H2PO4- c) HPO42- d) H3O+ The answer is A, can you explain why?
3. Show how phosphoric, H3PO4, dissociates in water and calculate the pH of a 0.030 M...
3. 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
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT