Thorium fluoride (ThF4) is not very soluble in water (Ksp = 5 × 1029). What is the concen- tration (molarity) of fluoride in a solution saturated with ThF4?
R ThF4(s) Th4+(aq) + F– (aq)
Thorium fluoride (ThF4) is not very soluble in water (Ksp = 5 × 1029). What is...
2. Thorium fluoride (ThF) is not very soluble in water (Kop=5 1029). What is the concen- tration (molarity) of fluoride in a solution saturated with ThF/? ThF.(8) - Th4+ (aq) + F(aq)
2. Thorium fluoride (ThF) is not very soluble in water (K = 5 x 1029). What is the concen- tration (molarity) of fluoride in a solution saturated with ThF,? ThF.(s) – Th'+ (aq) + F (aq)
Copper(II) carbonate is very poorly soluble in water, but better soluble in NH3(aq) due to the formation of the Cu(NH3)4 2+ complex: CuCO3(s) + 4NH3(aq) ⇄ Cu(NH3)4 2+ (aq) + CO3 2- (aq) CuCO3 (Ksp = 2.3·10-10 ) and the formation constant for Cu(NH3)4 2+ (Kf = 5.0·1012) What was the initial concentration of NH3(aq), if 0.010 mol of CuCO3(s) dissolved at equilibrium in 1.00 L of this solution? [Consider the change in the volume of solution negligible.]
Calcium hydroxide is a strong base but is not very soluble ( Ksp = 5.02 X 10-6 ). What is the pH of a saturated solution of Ca(OH)2 ?
Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 567 g NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution. concentration: If 8.67 g of CuNO, is dissolved in water to make a 0.250 M solution, what is the volume of the solution in milliliters? volume: mL
5 pts Question 12 AgCl is sparingly soluble in water as it has Ksp of 1.77 x 1010 at room temperature. Which solution will decrease the solubility of AgCI most effectively when mixed to saturated solution of AgCI? O 0.1 M KCI O 0.1 M CaCl2 00.1 M of AlCl3 O 0.1 M NaCi
10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain 4.28 millimoles (mmol) fluoride. What is the value of Ksp? CaF2(s) -> <- ca2+ (aq) +2 F- (aq) How did Ksp= [Ca2+] [F-]2 become Ksp= [s] [2s]2= 4s3 Cause I thought it was only Ksp= [s] [s]2 = s3 and why 4.28x10-3 have to devide by 10 and why the [F-] = 4.28 x 10-4 have to eqautes to 2 to have s= 2.14x10-4...
The compound silver fluoride, AgF is soluble in water. Write the net ionic equation for the dissociation reaction that occurs when solid silver fluoride dissolves in water: Use the pull-down boxes to specify states such as (aq) or (s).
1. If Ksp = 6.4 x 10-9 for magnesium fluoride, what is the concentration of Mg2+ and Fin equilibrium with solid magnesium fluoride? First write the equilibrium expression for Ksp. 2. The concentration of Ag+ in a solution saturated with Ag2C2O4 is 2.42 x 10-4 M. Calculate Ksp for Ag2C2O4.
5.0 g of barium fluoride is added to 1.0 L of water. After a sufficient amount of time, the saturated solution is filtered and the solid is dried and weighed and found to have a mass of 3.6g. What is the solubility product constant, Ksp Bato Bar + 2 Flag) (BaFz)? Ksp = [B2[F]?