Calculate the buffering index in the pH range 4-8 for a 0.0040 M solution of carbonic acid at 25C. (Hint: This problem may be solved using a spreadsheet.) Use only Ka1 for this calculation, you may ignore Ka2
Calculate the buffering index in the pH range 4-8 for a 0.0040 M solution of carbonic...
What is the pH of a 0.10 M solution of carbonic acid? Carbonic acid, H2CO3 has two acidic protons: H2CO3 + H2O7 HCO3 + H30+ Ka1 = 4.3x10-7 HCO3 + H202 CO32- + H30+ Ka2 = 5.6x10-11 a) 1.00 b) 0.70 c) 6.37 d) 3.68 e) I still can't figure this out...
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of CO3 -2. Ka1 = 4.30 x 10-7 Ka2 = 5.59 x 10-11
12. Calculate the pH and the concentration of all species in solution of 0.33 M K2CO3. For carbonic acid Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×10-7 and Ka2 = 5.6 × 10-11.10)A) 10.44 B) 5.50 C) 4.31 D) 11.00 E) 3.56
46. What is the percent ionization of a 0.491 M aqueous solution of carbonic acid? Ka1= 4.2x10^-7; Ka2= 4.8x10^-11 47. What is the percent ionization of a 0.356 M aqueous solution of hydrosulfuric acid? Ka1= 9.5x10^-8; Ka2= 1x10^-19 48. What is the pH of a 0.387 M aqueous solution of acetic acid? Ka (CH3COOH) = 1.8x10^-5 49. What is the pH of a 0.0398 M aqueous solution of benzoic acid? Ka (C6H5COOH) = 6.5x10^-5 50. What is the pH of...
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.
Calculate the pH of a 0.01 M carbonic acid, H2CO3, solution, given Kal = 4.3 x 10-7, and Ka2 = 5.2 x 10-11. Test your approximation.
2. Calculate the pH of a 0.230 M calcium acetate solution if the Ka for acetic acid is 1.8x10-5 . 3. Calculate the pH of a 0.225 M solution of H2CO3. Ka1 = 4.3x10^-7 ; Ka2 = 5.6x10^-11 4. Calculate the pH of a 0.0080 M solution of sulfuric acid. Ka2 = 1.2x10^-2
Calculate the pH of each solution. A solution containing 0.0320 M maleic acid and 0.046 M disodium maleate. The Ka values for maleic acid are 1.20 x 10 (Ka1) and 5.37 x 10-7 (Ka2) 1.8 pH A solution containing 0.0306 M succinic acid and 0.019 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 105 (Kal) and 2.31 x 10 (Ka2) pH