Calculate the pH of a solution that contains the following
analytical concentrations 0.0100 M inH2C2O4 and...
Calculate the pH of a solution that contains the following
analytical concentrations 0.0100 M inH2C2O4 and 0.0610 M in
Na2C2o4. Please show steps so that we can learn from this?
A) Calculate the pH of a 0.0100 M solution of butylamine by
making the assumption that the formal concentration is equal to the
equilibrium molarity of the butylamine in solution.
B) Calculate the percent error incurred by "cutting corners"
with the assumption in part A
C) Solve part A by using the technique of successive
iterations.
D) Solve part A by using the quadratic
Calculate the pH and concentrations of the following species in
a 0.025 M carbonic acid solution. (Given Ka1 = 4.3x10-7 and Ka2 =
5.6x10-11)
a) H2CO3
b) HCO3-
c) CO32-
d) H+
e) OH
Calculate the pH of a 5.0 M H3PO4 solution
and the equilibrium concentrations of the species
H3PO4,
H2PO4-,
HPO42- and PO43- (ka1 =
7.5 x 10-3, ka2 = 6.2 x 10-8, ka3 = 4.8 x
10-13)
Calculate the pH of a buffer solution that contains 0.44 M
NaH2PO4 and 0.29M Na2HPO4
Calculate the change in pH if 0.100 g of solid NaOH is added to
250 mL of the solution in the problem above.
Suppose a solution contains 0.28 M Pb2 and 0.46 M Al3 .
Calculate the pH range that would allow Al(OH)3 to precipitate but
not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found
here.
Suppose a solution contains 0.22 M Pb2 and 0.49 M Al3 .
Calculate the pH range that would allow Al(OH)3 to precipitate but
not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found
here.
Determine the pH of an HNO2 solution of each of the following
concentrations.
0.540 M
0.100 M
1.30×10−2 M
In which cases can you not make the simplifying assumption that
x is small?