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![In generally Saturated solution equilibria given as AB = A +6 Solubility product of AB = Ksp = [A40] solubility product is th](http://img.homeworklib.com/questions/dc3a2530-07bf-11ea-88b4-f3966fed5aea.png?x-oss-process=image/resize,w_560)
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2. Thorium fluoride (ThF) is not very soluble in water (K = 5 x 1029). What is the concen- tration (molarity) of fl...
2. Thorium fluoride (ThF) is not very soluble in water (Kop=5 1029). What is the concen-...
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)
Thorium fluoride (ThF4) is not very soluble in water (Ksp = 5 × 1029). What is...
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)
For the reaction MgF2(s) <=> Mg2+(aq) + 2 F-(aq), at a given temperature, K = 7.4...
For the reaction MgF2(s) <=> Mg2+(aq) + 2 F-(aq), at a given temperature, K = 7.4 x 10-11. What MASS (you’ll need to calculate molarity!) of MgF2 could be added to 2L of water, such that ALL the MgF2 dissolves? How soluble is MgF2 in water (qualitative answer…ie, VERY, NOT VERY, etc).
Copper(II) carbonate is very poorly soluble in water, but better soluble in NH3(aq) due to the...
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.]
2. The equilibrium constant for the following reaction is called the "solubility product" of calcium fluoride:...
2. The equilibrium constant for the following reaction is called the "solubility product" of calcium fluoride: CaF2(s) - Cal(aq) + 2F-(ay) K = Kp = 3.2 x 10-11 (a) Write an expression for the equilibrium constant of this reaction in terms of concentrations. Why do you suppose we call this a solubility product instead of a solubility quotient or ratio? (b) Calculate the equilibrium concentrations of Ca2+ and F if excess solid CaF is placed in water. (c) in which...
ID03/2 hul the lune strength is due solely to the O 0.562 7.5 x 10-3 O 5.2 x 10-3 4.2 x 10-3 4. Magnesium fluorid...
ID03/2 hul the lune strength is due solely to the O 0.562 7.5 x 10-3 O 5.2 x 10-3 4.2 x 10-3 4. Magnesium fluoride (MgF2) is a sparingly soluble salt. It has Kp = 7.4x10-9. Calculate the concentration of fluoride ion in a saturated solution of MgF,. O 1.2 x 10-3 M O 2.5 x 10-3 O 7.4 x 10-9 O 6.3 x 10-5 5. Consider the reaction Sr(s) + FeOH(aq) + H2O + (aq) Sr2+ (aq) + Fe(s)...
Part B please. Part A Silver chloride is only slightly soluble in pure water at 25...
Part B please.
Part A Silver chloride is only slightly soluble in pure water at 25 C AgCI(s) Ag (ag)+CI (aq) K-1.8 x 10 1 Calculate the concentration of Ag and Cl in a solution that is saturated with AgCl e, the system is at equilibrium and there is still solid AgCl visible). Express your answers using two significant figures, separate your answers by a comma. [Ag+],[Cl-)- 1.3×10-5 1.3×10-5 mol Li Previous An Correct Part B The addition of ammonia...
Solid Fe(OH)2 is slightly soluble in water. The Ksp = 1.6 x 10-14. What is the...
Solid Fe(OH)2 is slightly soluble in water. The Ksp = 1.6 x 10-14. What is the pH of a solution made from 0.2 mole of Fe(OH)2 (s) added added to 1.0 L solution of 0.039 M Fe(NO3)2(aq)? Note this is a review from chapter 15. There will be a problem like this on the exam. (A) 7.51 (B) 7.36 (C) 4.50 o (D) 7.81 (E) 4.99 Submit
6 6. Zinc hydroxide, Zn(OH)2. is practically insoluble in pure water. (Kap 3.0 x 10-16) a) Determine the pH of a saturated aqueous solution of Zn(O1H)2. (You should assume that all hydroxide ions...
6 6. Zinc hydroxide, Zn(OH)2. is practically insoluble in pure water. (Kap 3.0 x 10-16) a) Determine the pH of a saturated aqueous solution of Zn(O1H)2. (You should assume that all hydroxide ions in the solution come from the Zn(OH)2: you can ignore the autoionization of water.) (4 pts) b) Zn(OH)2 is less soluble in even very dilute solutions of Zn(NOs)2 due to the common ion effect. Determine the molar solubility of zine hydroxide in a 1.0 x 10-4 M...
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(a...
all 5&6
5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
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. The equilibrium constant for the following reaction is called the "solubility product" of calcium fluoride: CaF2(s) - Cal(aq) + 2F-(ay) K = Kp = 3.2 x 10-11 (a) Write an expression for the equilibrium constant of this reaction in terms of concentrations. Why do you suppose we call this a solubility product instead of a solubility quotient or ratio? (b) Calculate the equilibrium concentrations of Ca2+ and F if excess solid CaF is placed in water. (c) in which...
ID03/2 hul the lune strength is due solely to the O 0.562 7.5 x 10-3 O 5.2 x 10-3 4.2 x 10-3 4. Magnesium fluoride (MgF2) is a sparingly soluble salt. It has Kp = 7.4x10-9. Calculate the concentration of fluoride ion in a saturated solution of MgF,. O 1.2 x 10-3 M O 2.5 x 10-3 O 7.4 x 10-9 O 6.3 x 10-5 5. Consider the reaction Sr(s) + FeOH(aq) + H2O + (aq) Sr2+ (aq) + Fe(s)...
Part B please.
Part A Silver chloride is only slightly soluble in pure water at 25 C AgCI(s) Ag (ag)+CI (aq) K-1.8 x 10 1 Calculate the concentration of Ag and Cl in a solution that is saturated with AgCl e, the system is at equilibrium and there is still solid AgCl visible). Express your answers using two significant figures, separate your answers by a comma. [Ag+],[Cl-)- 1.3×10-5 1.3×10-5 mol Li Previous An Correct Part B The addition of ammonia...
Solid Fe(OH)2 is slightly soluble in water. The Ksp = 1.6 x 10-14. What is the pH of a solution made from 0.2 mole of Fe(OH)2 (s) added added to 1.0 L solution of 0.039 M Fe(NO3)2(aq)? Note this is a review from chapter 15. There will be a problem like this on the exam. (A) 7.51 (B) 7.36 (C) 4.50 o (D) 7.81 (E) 4.99 Submit
6 6. Zinc hydroxide, Zn(OH)2. is practically insoluble in pure water. (Kap 3.0 x 10-16) a) Determine the pH of a saturated aqueous solution of Zn(O1H)2. (You should assume that all hydroxide ions in the solution come from the Zn(OH)2: you can ignore the autoionization of water.) (4 pts) b) Zn(OH)2 is less soluble in even very dilute solutions of Zn(NOs)2 due to the common ion effect. Determine the molar solubility of zine hydroxide in a 1.0 x 10-4 M...
all 5&6
5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
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