Question

Malonic acid, H2C3H2O4, is a diprotic acid, with the following acid dissociation constants. Ka1 = 1.4...

Malonic acid, H2C3H2O4, is a diprotic acid, with the following acid dissociation constants. Ka1 = 1.4 × 10–3Ka2 = 2.0 × 10–6 Calculate the amount of HC3H2O4‒ present in a 0.80 M H2C3H2O4(aq) solution.

A.3.3 × 10‒2M

B.1.3 × 10‒3M

C.2.6 × 10‒4M

D.2.0 × 10‒6M

When I solved this problem I found that K1=3.3x10^-2, and K2=1.3x10^-3. My question is how can you tell which Ka is correct? How can you pick when both answers are listed?

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
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
For which .10M diprotic acid would the 2nd dissociation affect the pH significantly? Explain. H2A: Ka1=4.2*10^-2...
For which .10M diprotic acid would the 2nd dissociation affect the pH significantly? Explain. H2A: Ka1=4.2*10^-2 Ka2=1.8*10^-7 H2B: Ka1=2.4*10^-4 Ka2= 6.1*10^-8 H2C: Ka1=1.3*10^-4 Ka2=5.2*10^-9 H2D: Ka1=1.8*10-3 Ka2=9.3*10^-4
Oxalic acid is a diprotic acid that occurs naturally in some plants. Calculate the pH and...
Oxalic acid is a diprotic acid that occurs naturally in some plants. Calculate the pH and the concentrations of all species present in a 0.96-M solution. The acid dissociation constants are K1 = 5.9 10-2 and K2 = 6.4 10-5. I have part A but i cannot get part B,C or D a.) [C2O4H2] .71 correct b.) [C2O4H − ] C.)[C2O42-] D.) pH
given a diprotic acid, H2A, with two ionization constants of Ka1 = 1.6×10^-4 and Ka2 =...
given a diprotic acid, H2A, with two ionization constants of Ka1 = 1.6×10^-4 and Ka2 = 5.2×10^-11, calculate the ph for a .206 M solution of NaHA
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.
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1 10-3 and Ka2 =...
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1 10-3 and Ka2 = 2.5 10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHA? NaHA/H2A Na2A/NaHA pKa of the acid component
4. Give a brief explanation for each of the following. (a) For the diprotic acid H2S,...
4. Give a brief explanation for each of the following. (a) For the diprotic acid H2S, the first dissociation constant is larger than the second dissociation constant by about 105 (K1 ~ 105 K2). (b) In water, KOH is a base, but HOCl is an acid. (c) When each is dissolved in water, HCl is a much stronger acid than HF.
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).
Ascorbic acid has two dissociation constants, Ka1=7.9 x 10-5 and Ka2=1.6 x 10-12. What reactions do...
Ascorbic acid has two dissociation constants, Ka1=7.9 x 10-5 and Ka2=1.6 x 10-12. What reactions do these constants refer to? Why is one of sthem so much larger than the other? Which one should you use to calculate the theoretical pH of a 0.50 M solution of ascorbic acid, and why?
For the compound H2XO2, the acid dissociation constants are given as K1 = 8.09 x 10^-7...
For the compound H2XO2, the acid dissociation constants are given as K1 = 8.09 x 10^-7 and K2 = 8.09 x 10^-11. A) For a 0.040 M H2XO2 solution, calculate the concentrations of H+, HXO2-, and XO2 2-. B) Calculate the pH of a solution made from 0.100 moles of Na2XO2 in 1.00 L of water. C) Sketch the titration curve which is expected when a solution contains 0.0100 moles of Na2XO2 and 0.0100 moles of NaHXO2 is titrated with...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT