Calculate the concentration of H+ in a 0.250 M solution of
oxalic acid. Consider only [H+] from the first ionization. (Ka =
5.37 x 10^-2) Then calculate [H+] of the same solution, including
the H+ ions resulting from the second ionization. (Ka = 5.37 x
10^-5)
Calculate the equilibrium concentration of carbonate in a 0.067 M
solution of carbonic acid. Do not enter units as part of your
answer. Use “E” for scientific notation.
Ascorbic acid (Vitamin C, CHO) is a weak diprotic acid, with K
= 6.8x10 and K = 2.7x10. What is the pH of a solution that contains
10.0 mg of vitamin C per 1.0 mL of solution?
Calculate the concentration of all species in a 0.155 M solution
of H2CO3.
Express your answer using two significant figures.
[H2CO3], [HCO−3], [CO2−3], [H3O+], [OH−] =
M
Calculate the pH and the equilibrium
concentration of Se2- in a
8.75×10-2 M hydroselenic
acid solution, H2Se
(aq).
For H2Se, Ka1 =
1.3×10-4 and Ka2 =
1.0×10-11
pH =
[Se2-] =
M
Calculate the pH and the equilibrium concentrations of HS- and
S2- in a 0.0425 M hydrosulfuric acid solution, H2S (aq).
For H2S, Ka1 = 1.0×10-7 and Ka2 = 1.0×10-19
pH =
[HS-] =
M
[S2-] =
M
Calculate the equilibrium concentration of undissociated in a
glycolic acid solution with an analytical glycolic acid
concentration of 0.0824 and a pH of 3.180.
Part A: Calculate the [H3O+] of the following polyprotic acid
solution: 0.370 M H3PO4. Express your answer using two significant
figures.
Part B: Calculate the pH of this solution.
Express your answer using one decimal place.
Part C: Calculate the [H3O+] and pH of the following polyprotic
acid solution: 0.360 M H2C2O4. Express your answer using two
significant figures.
Part D: Calculate the pH of this solution.
Express your answer using two decimal places.
Thank you so much!!
Calculate the fraction of nitrous acid deprotonated if the solution
concentration is 0.241 M. The acid dissociation constant of nitrous
acid is 3.0 x 10^-8.
How do you solve for x?