Determine the pH of an HNO2 solution of each
of the following concentrations.
A. 0.510M
B. 0.100M
C. 1.00*10^-2
D. In which of these cases can you not make the simplifying
assumption that x is small?
Determine the pH of each solution.
a. 0.155 M HNO2 (for HNO2, Ka=4.6×10^−4)
b. 0.0210 M KOH
c. 0.240 M CH3NH3I (for CH3NH2, Kb=4.4×10^−4)
d. 0.324 M KC6H5O (for HC6H5O, Ka=1.3×10^−10)
Determine the pH of an HF solution of each of
the following concentrations.
Part A: .280 M
PartB : 4.5*10^-2 M
Part C: 2*10^-2
Part D
In which cases can you not make the simplifying assumption that
x is small?
In which cases can you not make the simplifying assumption that
x is small?
only in (a)
only in (b)
in (a) and (b)
in (b) and (c)
Determine the pH of an HF solution of each of the following
concentrations. In which cases can you not make the simplifying
assumption that x is small? (Ka for HF is 6.8×10−4.)
a) 0.260 M
b) 4.80×10−2 M
c) 3.00×10−2 M
Determine the pH of each of the following two-component
solutions.
0.270 M NH4NO3 and 0.100 M HCN
8.0×10−2 M RbOH and 0.120 M NaHCO3
8.2×10−2 M HClO4 and 2.2×10−2 M KOH
0.110 M NaClO and 5.50×10−2 M KI
For a 0.100 M solution of K2HPO4, find each of the following
values: pH, [H+], [HPO42-], [PO43-], and [H2PO4-]. Use the
minimum number of approximations.
Calculate the concentrations of all species in a 0.540 M Na2SO3
(sodium sulfite) solution. The ionization constants for sulfurous
acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.
A 0.100 M solution of nitrous acid has a PH ==2.10 . Determine
the value of the ionization constant for nitrous acid . Determine
the present ionization for this acid.