Ksp = 3.2×10-11 for CaF2 at 25 °C. a)Calculate the molar concentration of fluoride ions in...

Ksp = 3.2×10-11 for CaF2 at 25 °C.
a)Calculate the molar concentration of fluoride ions in a saturated calcium fluoride solution at 25 °C using the assumption that the solution is ideal -- i.e. the activity coefficients are 1.

b)Still assuming an ideal solution, what mass of CaF2 would be dissolved in 100. mL of saturated solution at 25 °C?
c)Using activity coefficients γCa2+ = 0.405 and γF− = 0.76, calculate the maximum mass of CaF2 which can dissolve in 100. mL of 0.100 M KF?

Expert Solution

queen_honey_blossom answered 2 years ago

Ksp = 2.6×10-9 for SrF2 at 25 °C. a. Calculate the molar concentration of fluoride ions...

Ksp = 2.6×10-9 for SrF2 at 25 °C. a. Calculate the molar concentration of fluoride ions in a saturated strontium fluoride solution at 25 °C using the assumption that the solution is ideal -- i.e. the activity coefficients are 1. b. Using activity coefficients determine the molar solubility of SrF2 in 0.100-M potassium nitrate solution at 25 °C? c. Using activity coefficients calculate the maximum mass of SrF2 which can dissolve in 100. mL of 0.100 M KF?

Calculate the molar solubility of magnesium phosphate, Mg3(PO4)2 (Ksp = 1.0×10–25) Calculate the concentration of lithium...

Calculate the molar solubility of magnesium phosphate, Mg3(PO4)2 (Ksp = 1.0×10–25) Calculate the concentration of lithium ions in a saturated solution of lithium phosphate, Li3PO4 (Ksp = 3.2×10–9)

Ksp for Ag2SO4 is 1.2×105 at 25°C. Calculate the expected molar solubility of Ag2SO4 at 25°C...

Ksp for Ag2SO4 is 1.2×105 at 25°C. Calculate the expected molar solubility of Ag2SO4 at 25°C a. in 0.20 M Na2SO4 b. in 0.20 M NaNO3

Calculate the molar solubility of barium fluoride in 0.15 M Nag, Ksp for BaF2 is 2.45×10^-5

For a magnesium fluoride, MgF2, Ksp= 6.4x10^-9, calculate the molar solubility in pure water. Calculate the...

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 Ag2CrO4(s) in (Solubility Product Ksp at 25 °C is 9.0 ×...

Calculate the molar solubility of Ag2CrO4(s) in (Solubility Product Ksp at 25 °C is 9.0 × 10−12) A) pure water B) in 0.500 L of a solution containing 0.950 g K2CrO4

Calculate the molar solubility in pure water for the following compound at 25°C, Ag2SO3 Ksp =...

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?

Calculate the molar solubility of CaF2 in a solution containing 0.205 M of Ca(NO3)2. The Ksp...

Calculate the molar solubility of CaF2 in a solution containing 0.205 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10.

3. What is the molar Solubility of CaF2 in 0.250 M Ca(NO3)2? (Ksp of CaF2 =...

3. What is the molar Solubility of CaF2 in 0.250 M Ca(NO3)2? (Ksp of CaF2 = 3.2 x 10-8) 4. How many grams of Ag2SO4 will be soluble in 100 ml of water? (Ksp of Ag2SO4 = 4.1 x 10-7) 5. How many grams of Ag2SO4 will be soluble in 250 ml of 0.100 M Na2SO4? (Ksp of Ag2SO4 = 4.1 x 10-7)

Part A Calculate the molar concentration of OH− ions in a 8.1×10−2 M solution of ethylamine...

Part A Calculate the molar concentration of OH− ions in a 8.1×10−2 M solution of ethylamine (C2H5NH2)(Kb=6.4×10−4). Express your answer using two significant figures. [OH−] = M Part B Calculate the pH of this solution. Express your answer using two decimal places.

Question