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Cul has a Ksp = 1.1 x 10-12 Select any and all of the true statements...
Question 7 Determine the solubility of Cul(s) (Ksp = 1.1 x 10-12) in 0.15 M Cu(NO3)2(aq) solution 1- 1- Ksp = (S+ 0.15). (25)?. S = (Ksp/0.6) 1/2, S = 1.35 x 10-6 M 2- 2- Ksp = S . (S + 0.30). S = (Ksp/0.30), S = 3.67 x 10-12 M 3- 3- Ksp = (S + 0.15).S. S = (Ksp/0.15). S = 7.33 x 10-12 M
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
Question 1 10 poi Determine the solubility of Cul(s) (Ksp = 1.1 x 10-12) in 0.15 M Srl2(aq) solution 1- 1- Ksp = (s). (S + 0.30), S = (Ksp/0.30), S = 3.67 x 10-12M 2- 2- Ksp = (S). (S + 0.15)2. S = (Ksp/0.023), S = 4.78 x 10-11 M 3- 3- Ksp = (s). (S + 0.30)2 S = (Ksp/0.09), S = 1.22 x 10-11 m.
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x 10-19), however, it is highly soluble in an ammonia solution due to the formation of the complex ion [Ag(NH3)21 (Kr" 1.7 X 10) Given this information, calculate the molar solubility of AgCl in 2.25 M ammonia. 2. Calculate the molar solubility of Cul in 0.92 M KCN. (Ksp of Cul is 1.1 x 10-12, Kp of [Cu(CN)2] is 1.0 x 1016).
a) The solubility product, Ksp, of Cd3(PO4)2 is 2.5 x 10-33. What is the solubility (in g/L) of Cd3(PO4)2 in pure water? b) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.38 and is saturated in Cu(OH)2. c) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to...
AgBr is sparingly soluble in water and has a Ksp of 5.0 x 10-13. What will be the effect of adding solid NaBr to an aqueous solution of in equilibrium with solid AgBr? Some additional AgBr will precipitate. The Ksp of AgBr will increase. The Agt concentration will remain constant. Additional AgBr will dissolve.
The solubility of Ce(IO3)3 in a 0.14-M KIO3 solution is 1.3 x 10-7 mol/L. Calculate Ksp for Ce(IO3)3 - Ksp = Submit Answer Try Another Version 10 item attempts remaining Which of the following two compounds is expected to be more soluble in acidic solution than in pure water? a. Agi AgNO2 b. Mn(NO3) Mn(CN)2 Submit Answer Try Another Version 10 item attempts remaining Calculate the solubility of solid Ca3(PO4)2 (Ksp = 1.3x10-32) in a 0.16 M Na3PO4 solution. S...
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Question 3 A Solution pH 7.00 8.00 9.00 Ag... 1.41 x 10-4 1.41 x 10-4 1.37 x 10-4 1.00 x 10-4 1.96 x 100 2.00 x 10- 2.00 x 10-7 Submit 10.00 11.00 12.00 13.00 A student investigates the effects of pH on the solubility of AgOH(3), which dissolves in water according to the equation AgOH(3) Ag' (aq) + OH(aq). The value for Kp for AgOH is 2.0 x 10 at 298 K. The student places the...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except that they have the following pH values: Hint: Common ion effect. Which two ions dictate acidity and basicity? a. 3 b. 7 c. 9 d. 11 2. Potassium perchlorate has a solubility product constant of 10-2. Which is true about the following solution of KClO4: [K+] = 0.01 M, [ClO4 −] = 0.01 M a. Ksp < Q and no precipitation occurs b....
Solubility Product Constants (Ksp at 25 °C) Type Formula Кsp Bromides PbBr2 6.3 x 10-6 AgBr 3.3 * 10-13 Carbonates BaCO3 8.1 x 10-9 CaCO3 3.8 x 10-9 COCO3 8.0 × 10-13 CuCO3 2.5 10-10 FeCO3 3.5 x 10-11 PbCO3 1.5 10-13 MgCO3 4.0 x 10-5 MnCO3 1.8 10-11 NiCO3 6.6 x 10-9 Ag2CO3 8.1 x 10-12 ZnCO3 1.5 x 10-11 Chlorides PbCl2 1.7 x 10-5 AgC1 1.8 10-10 Chromates BaCrO4 2.0 x 10-10 CaCrO4 7.1 x 10-4 PbCr04 1.8...