Question

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

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 is the (H2PO4-) of a solution labeled "0.10 M Phosphoric Acid"? [Ka1= 7.1 x 10...
What is the (H2PO4-) of a solution labeled "0.10 M Phosphoric Acid"? [Ka1= 7.1 x 10 ^ -3 , Ka2= 6.3 x 10^ -8, Ka3 = 4.2 x 10 ^-13]
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13)...
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after adding 24.16 mL of 0.1000M NaOH.
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?
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13)...
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after adding 33.71 mL of 0.1000M NaOH. ** All volumes should have a minimum of 2 decimal places.
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13)...
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after adding 33.71 mL of 0.1000M NaOH. ** All volumes should have a minimum of 2 decimal places.
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13)...
Calculate the pH during the titration of 50.00 mL of 0.1000M phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after adding 28.79 mL of 0.1000M NaOH. ** All volumes should have a minimum of 2 decimal places.
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.
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
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.
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