Question

Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.270 M oxalic acid...

Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.270 M oxalic acid solution (Ka1 = 6.5 × 10−2, Ka2 = 6.1 × 10−5). Be sure to report your answers to the correct number of significant figures. please give details and formulas,

Homework Answers

Answer #1

H2C2O4   ----------------> HC2O4-   + H+

0.270                                   0            0

0.270 - x                             x               x

Ka1 = x^2 / 0.270 - x

6.5 x 10^-2 = x^2 / 0.270 - x

x = 0.1039

[H+] = 0.104 M

[HC2O4-] = 0.104 M

[H2C2O4 ] = 0.166 M

[C2O42-] = 6.1 x 10^-5 M

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
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.210 M oxalic acid...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.210 M oxalic acid solution (Ka1 = 6.5 × 10−2, Ka2 = 6.1 × 10−5). Be sure to report your answers to the correct number of significant figures.
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.370 M oxalic acid...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.370 M oxalic acid solution (Ka1 = 6.5 ×10−2, Ka2 = 6.1 ×10−5). Be sure to report your answers to the correct number of significant figures.
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.290 M oxalic acid...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.290 M oxalic acid solution (Ka1 = 6.5 × 10−2, Ka2 = 6.1 × 10−5). Report your answers to 2 significant figures. [H2C2O4] = M [HC2O4−] = M [C2O42−] = × 10 M Enter your answer in scientific notation. [H+] = M
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ ions in a 0.193 M oxalic acid...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ ions in a 0.193 M oxalic acid solution at 25 °C. (Ka1 = 6.5 × 10−2 and Ka2 = 6.1 ×10−5 for oxalic acid.) (Enter your answer in scientific notation.)
Be sure to answer all parts. Calculate the concentrations of H2C2O4, HC2O4?, C2O42?, and H+ ions...
Be sure to answer all parts. Calculate the concentrations of H2C2O4, HC2O4?, C2O42?, and H+ ions in a 0.227 M oxalic acid solution at 25°C. (Ka1 = 6.5 × 10?2 and Ka2 = 6.1 × 10?5 for oxalic acid.) [H2C2O4] = M [HC2O4?] = M [C2O42?] = M (scientific notation) [H+] = M
Oxalic acid, found in the leaves of rhubarb and other plants, is a diprotic acid. H2C2O4...
Oxalic acid, found in the leaves of rhubarb and other plants, is a diprotic acid. H2C2O4 + H2O ↔ H3O+ + HC2O4- Ka1= ? HC2O4- + H2O ↔ H3O+ + C2O42- Ka2 = ? An aqueous solution that is 1.05 M H2C2O4 has pH = 0.67. The free oxalate ion concentration in this solution is [C2O42-] = 5.3 x 10-5 M. Determine Ka1 and Ka2 for oxalic acid.
Oxalic acid can donate two protons to water in successive reactions: (1) H2C2O4(aq)+H2O(l)⇌H3O+(aq)+HC2O4-(aq) (2) HC2O4-(aq)+H2O(l)⇌H3O+(aq)+C2O42-(aq) If...
Oxalic acid can donate two protons to water in successive reactions: (1) H2C2O4(aq)+H2O(l)⇌H3O+(aq)+HC2O4-(aq) (2) HC2O4-(aq)+H2O(l)⇌H3O+(aq)+C2O42-(aq) If Kc1 = 5.9 × 10-2 andKc2 = 6.4 × 10-5 at 25°C, what is the value of Kc for reaction (3)? (3) H2C2O4(aq)+2H2O(l)⇌2H3O+(aq)+C2O42-(aq) A) 9.2 × 102 B) 1.1 × 10-3 C) 5.9 × 10-2 D) 3.8 × 10-6 Why is C not the right answer? Does Hess's Law not apply in this problem?
Calculate the concentrations of all species in a 1.12 M Na2SO3 (sodium sulfite) solution. The ionization...
Calculate the concentrations of all species in a 1.12 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4� 10�2 and Ka2 = 6.3� 10�8. NA+ = SO32- = HSO3- = H2SO3 = OH- = H+ =
Calculate the concentrations of all species in a 0.470 M Na2SO3 (sodium sulfite) solution. The ionization...
Calculate the concentrations of all species in a 0.470 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. NA+ SO32- HSO3- H2SO3 OH- H+
Oxalic acid, which is formed either as (COOH)2 or H2C2O4, is a diprotic acid. At 25...
Oxalic acid, which is formed either as (COOH)2 or H2C2O4, is a diprotic acid. At 25 degrees celecius ka1= 5.9 x 10^-2 and ka2= 6.4 x 10^-5. Using just sodium oxalate and stock solutions of either 3.00 M HCL (aq), how many grams of sodium oxalate and milliliters of stock solution are needed to prepare 1.00 L of a buffer that has pH= 4.0 and contains 0.16 M oxalate ion?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT