Calculate the molar solubility of magnesium fluoride in each of
the following solutions:
a) pure water
b) 0.010 M potassium fluoride solution
c) 0.050 M solution of magnesium nitrate
d) Why are the results of parts (a) thru (c) different?
Calculate the molar solubility in pure water for the following
compound at 25°C, Ag2SO3 Ksp =
1.5x10-14
What is the molar solubility in 0.0010 M sodium
sulfite?
For a magnesium fluoride, MgF2, Ksp= 6.4x10^-9, calculate the
molar solubility in pure water.
Calculate the molar solubility in 0.050 M NaF solution.
Please show step by step instructions, thank you!
Calculate the molar solubility of MX(Ksp=1.27×10−36)
in:
Part A
pure water
Express your answer using three significant figures.
Part B
0.28 M MCl2
Express your answer using two significant figures.
Part C
0.22 M Na2X
Express your answer using two significant figures.
Part A
Use the molar solubility 1.08×10−5M in pure water to
calculate Ksp for BaCrO4.
Ksp =
Part B
Use the molar solubility 1.55×10−5M in pure water to
calculate Ksp for Ag2SO3.
Ksp =
Part C
Use the molar solubility 2.22×10−8M in pure water to
calculate Ksp for Pd(SCN)2.
Ksp =
Molar solubility of copper hydroxide in pure water, taken into
account that water is adding hydroxide into the solution.
Ksp=[Cu^2+][OH^-]^2 = 4.8x10^-20
(x) (1.0x10^-7 +2x)^2 = 4.8x10^-20
Calculate the molar concentration of OH negative in water
solutions with the following H3O positive molar concentrations:
a) 0.044
b) 1.3 * 10 to the negative 4 power
c) 0.0087
d) 7.9 * 10 to the negative 10 power
e) 3.3 * 10 to the negative 2 power
(Please show clear handwriting and step by step) Thank you!!
Calculate the molar solubility of HgBr2
(Ksp= 5.6 x 10-23) in the following
solutions. Be sure to state and justify any assumption you make in
solving the problems. Be sure to correct for ionic strength.
a saturated solution of HgBr2
0.025 M Hg(NO3)2 saturated with
HgBr2
0.050 M NaBr saturated with HgBr2
Explain how ionic strength affects the solubility of
HgBr2