thank u What is the [CO_3^-2] in seawater (a 0.05 M solution of carbonic acid, K_a1...
One of the buffers to maintain the pH of blood is the carbonic acid, H_2CO_3, buffer. Carbonic acid is diprotic and it's equilibrium constants are K_a1 = 4.2 times 10^-7 and K_a2= 4.8 times 10^-11. How would you prepare 5.0 L a carbonic acid buffer of a pH of 7.2 from 0.250 M H_2CO_3? You have available NaHCO_3 (MW = 84.0) and Na_2CO_3 (MW = 106).
What is the molar concentration of carbonate ion in a 0.10 M solution of carbonic acid? Ka1 = 4.3 × 10–7 ; Ka2 = 5.6 × 10–11 Please report the answer in units of M (do not write unit, only number) Write numbers as 1.23E-5
What is the molar concentration of carbonate ion in a 0.10 M solution of carbonic acid? Ka1 = 4.3 × 10–7 ; Ka2 = 5.6 × 10–11 Please report the answer in units of M (do not write unit, only number) Write numbers as 1.23E-5
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?
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
Calculate the concentration of H^+, HCO_3^- and CO_3^2- in a 0.025 M H_2CO_3 solution. Note that H_2CO_3 is a diprotic acid. First ionization (Ka_1 = 4.2 times 10^-7) Second ionization (Ka_2 = 4.8 times 10^-11)
The next three (3) problems deal with the titration of 431 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.7 M KOH. What is the pH of the solution at the 2nd equivalence point? What will the pH of the solution be when 0.2045 L of 1.7 M KOH are added to the 431 mL of 0.501 M carbonic acid? How many mL of the 1.7 M KOH are needed...
A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L of water. Which statement about the solution is correct? A)The solution is basic. B) The solution is C) The solution is weakly acidic. D) The solution is strongly acidic. E The values for K_a and K_b for the species in solution must be known before a prediction can be made. The pH of blood is 7.35. It is maintained in part by the buffer system...
Determine the [H_3 O^+] in an aqueous solution of hypothetical diprotic acid, H_2 X, that is 0.10 M in H_2 X. (K_a1 = 1.0 times 10^-7, K_a2 = 1.0 times 10^-12) 1.0 times 10^-12 1.0 times 10^-19 1.0 times 10^-18 1.0 times 10^-4 0.10
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.