Oxalic acid, H2C2O4 has acid dissociation constants Ka1 = 5.9 �
10^2 and Ka2 = 6.4...
Oxalic acid, H2C2O4 has acid dissociation constants Ka1 = 5.9 �
10^2 and Ka2 = 6.4 � 10^5. What is the pH after 20.00 mL of 0.0500
M NaOH is added to 5.00 mL of 0.2000 M H2C2O4?
The Answer is 2.8 but I don't know how to get there
A diprotic acid, H2A, has acid dissociation constants of Ka1 =
2.40× 10–4 and Ka2 = 2.70× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.
.185M solution of NaHA
.185M solution of Na2A
A diprotic acid, H2A, has acid dissociation constants of Ka1 =
1.63× 10–4 and Ka2 = 4.71× 10–11. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.
(a) a 0.184 M solution of H2A
(b) a 0.184 M solution of NaHA
(c) a 0.184 M solution of Na2A
A diprotic acid, H2A, has acid dissociation constants of Ka1 =
3.66× 10–4 and Ka2 = 4.99× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.
(a) a 0.121 M solution of H2A
pH = ? [H2A]=? [HA-]=? [A2-]=?
(b) a 0.121 M solution of NaHA
pH = ? [H2A]=? [HA-]=? [A2-]=?
(c) a 0.121 M solution of Na2A
pH = ? [H2A]=? [HA-]=? [A2-]=?
A diprotic acid, H2A, has acid dissociation constants of Ka1 =
3.94× 10–4 and Ka2 = 2.17× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.
(a) a 0.147 M solution of H2A
(b) a 0.147 M solution of NaHA
A diprotic acid, H2A, has acid dissociation constants of Ka1 =
3.61× 10–4 and Ka2 = 4.02× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.
(a) a 0.124 M solution of H2A
pH [H2A] [HA-] [A2-]
(b) a 0.124 M solution of NaHA
pH [H2A] [HA-] [A2-]
(c) a 0.124 M solution of Na2A
pH [H2A] [HA-] [A2-]
A diprotic acid, H2A, has acid dissociation constants of Ka1 =
1.56× 10–4 and Ka2 = 2.28× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.
(a) a 0.203 M solution of H2A
(b) a 0.203 M solution of NaHA
(c) a 0.203 M solution of Na2A
Many household cleaning products contain oxalic acid, H2C2O4, a
diprotic acid with the following dissociation constants:
Ka1=5.9×10−2, Ka2=6.4×10−5Calculate the equilibrium concentration
of HC2O4− in a 0.20 mol L−1 solution of oxalic acid.
Determine the pH of 0.055 M oxalic acid
(H2C2O4;
Ka1=5.6x10-2 and
Ka2=5.4x10-5). Note: both steps are important
here, therefore we have to set up two "ICE" boxes. Show work.
The triprotic acid H3A has ionization constants of Ka1 = 1.6×
10–3, Ka2 = 2.4× 10–9, and Ka3 = 6.4× 10–11.
Calculate the following values for a 0.0800 M solution of
NaH2A.
[H+] = M
[H2A-]/[H3A] =
Calculate the following values for a 0.0800M solution of
Na2HA.
[H+] = M
[HA2-]/[H2A-] =
This is all the information this problem comes with
Hint:
Consider H2A– to be the intermediate form of a diprotic acid,
surrounded by H3A and HA2–. Consider...
The triprotic acid H3A has ionization constants of Ka1 = 6.2×
10–3, Ka2 = 9.6× 10–9, and Ka3 = 6.3× 10–12. Calculate the
following values for a 0.0790 M solution of NaH2A
A)Calculate the following values for a 0.0790 M solution of
NaH2A.
H+=?
H2A-/H3A=?
B)Calculate the following values for a 0.0790 M solution of
Na2HA.
H+=?
HA2-/H2A-=?