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 =
Calculate the molar solubility of magnesium fluoride in each of
the following solutions: (MgF2 Ksp = 7.4*10^-9)
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?
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