What is the Ksp for SrF2, given that 1.1 x 10-1 g/L dissolves in water?
What is the Ksp for SrF2, given that 1.1 x 10-1 g/L dissolves in water?
1) If 1.1 x 10-2 g of SrF2 dissolves per 100 mL of aqueous solution, what is its Ksp? 2) Which of the following is most soluble in water? NiS CaF2 Cu(OH)2 ZnCO3
a) What is the molar solubility of FeF2 in a 0.02M solution of NaF? b) What is the Ksp for SrF2, given that 1.1 x 10-1 g/L dissolves in water? c) What is the molar solubility of Fe(OH)2 in water and in a solution buffered at pH = 10.0, given that the Ksp = 7.9 x 10-16?
Given the concentration of a saturated solution of the following compound, what is the Ksp? SrF2: [Sr2+] = 5.82 × 10–4 mol L–1 ; [F– ] = 1.16 × 10–3 mol L–1
4. Given the Ksp values below: Ksp(BaF2) 2.4 x 10-5 Kappor KspPbF2) = 4.0 x 10-8 KsplSrF2) = 0.8 x 10-10 If I increasingly add NaF to a solution with (Ba2+1=[Pb2')= [Sr2"]=0.01 M, what is the precipitation sequence? a. SrF2 first, then PbF2, and finally BaF2 b. BaF2 first, then PbF2, and finally SrF2 c. Not enough information to tell d. SrF2 first, then BaF2, and finally PbF2
Question 5 10 points Determine the water solubility of Cul(s) (Ksp = 1.1 x 10-12) 1- 1- Ksp - S2, S-(Ksp)1/2, S = 1.05 x 10-6 M 2- 2- Ksp = 453, S = (Ksp/4)1/3, S = 6.5 x 10-5 M 3- 3- Ksp = 25, S = (Ksp/2). S = 5.5 x 10-13 M
What is the solubility of SrF2 (s) in moles per liter (mol/L) in pure water? O 5.3 x 10-5 O 8.9 x 10-4 O 7.0 x 10-10 O 3.7x 105 2.8 x 10 3 pts Question 4 What is the solubility in moles per liter (mol/L) of SrF2 (s) from the previous problem in a.2 M Sr2 (aq) solution? O 5.9 x 10 O 1.2 x 10+ O 7.0 x 10° O 1.4 x 10 O 8.4 x 105
15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a. 1.0 x 10-5 b.2.0 x 10-5 c. 4.0 x 10-5 d. 8.0 x 10-5 o o 15b) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4 in 0.10 M Na2SO4? a. 2.8 x 10-10 b.5.5 x 10-10 c. 1.1 x 10-9 d. 2.2 x 10-9
Question 1 1 pts The Ksp value for BaSO4 Ksp = 1.1 x 10 10. If 50.0 mL of 2.0 x 10-4 M Ba(NO3)2 is mixed with 350.0 mL of 1.0 x 10-5 M Na2SO4, will a precipitate be observed? A precipitate forms because the ion pair product, Q> Ksp A precipitate forms because the ion pair product, Q< Ksp. No precipitate forms because the ion pair product, Q = Ksp No precipitate forms because the ion pair product, Q<Ksp...
What is the correct expression for Ksp when BaSO4(s) dissolves in water
The solubility product, Ksp, of Sn(OH)4(s) is 1.0 x 10-57. What is its solubility (in g/L) in pure water?