A.Neglecting activity coefficients, calculate the pH of an
aqueous solution of 5.0 x 10-7 M KOH.
B. What fraction of the total [H+ ] is derived from the
autoionization of water?
a)Consider an aqueous solution of ammonium chloride, NH4Cl.
Neglecting the autoprotolysis of water, calculate the pH of NH4Cl
for formal concentration of 0.10M.
b)Use the systematic treatment of equilibrium to derive an
equation for an aqueous solution of NH4Cl that contains [H+], F, Ka
and Kw. Do not neglect the autoprotolysis of water in this
case.
The pH of a 0.00125 M solution of an aqueous solution of XOH (X
= an unknown element) is 3.55. Is XOH a strong acid, weak acid,
strong base, or weak base? How do you know? Is X a metal or
non-metal? Explain
Calculate the pH of a .215 M aqueous solution of aniline C6H5NH2,
Kb= 7.4x10^-10 and the equilibrium concentrations of the weak base
and it’s conjugate acid
Calculate the pH of a 0.0454 M aqueous solution of
triethelyene C2H5(3)N, Kb= 5.2x10^-4 and the equilibrium
concentrations of the weak base and its conjugate acid
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)