(References A solution contains 4.4 x 10-5 M Na,PO. What is the minimum concentration of AgNO,...
A solution contains 5.2 x 10-M Na, PO4. What is the minimum concentration of AgNO, that would cause precipitation of solid Ag, PO, (K = 1.8 x 10-18)? Concentration M Submit Answer Try Another Version 6 item attempts remaining
A solution contains 4.1 x 10-5 M Nag PO4. What is the minimum concentration of AgNO, that would cause precipitation of solid Ag, P04 Ksp = 1.8 x 10-18)? Concentration =
A solution contains 7.7 x 10-5 M Na3PO4. What is the minimum concentration of AgNO3 that would cause precipitation of solid Ag3PO4 (Ksp = 1.8 x 10–18)? Concentration =
When 100 mL of 1.0 M Na₃PO₄ is mixed with 100 mL of 1.0 M AgNO₃, a yellow precipitate forms and [Ag⁺] becomes negligibly small. Which of the following is a correct listing of the ions remaining in solution in order of increasing concentration? (A) [PO₄³⁻] < [NO₃⁻] < [Na⁺] (B) [Na⁺] < [NO₃⁻] < [PO₄³⁻] (C) [Na⁺] < [PO₄³⁻] < [NO₃⁻] (D) [PO₄³⁻] < [Na⁺] < [NO₃⁻] (E) [NO₃⁻] < [PO₄³⁻] < [Na⁺]
Consider a solution that is 2.4×10−2 M in Fe2+ and 1.8×10−2 M in Mg2+. [K2CO3] = 1.3×10−9 M is the minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? Express your answer using two significant...
yes or no? (References) If a solution is 6.5 x 10- M in Mn (NO3), and 5.0 x 10 aqueous ammonia, will Mn(OH), precipitate? Min Ksp (Mn(OH)) = 4.6 x 10-14 Kỳ (NH4) =1.8 x 10-5 Yes | Answer Try Another Version tempts remaining No
A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 9.60×10-5 M, is 10,000 times less than that of the PO43– ion at 0.960 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Calculate the minimum Ag+ concentration required to cause precipitation...
Question: A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 9.10×10-5 M, is 10,000 times less than that of the PO43– ion at 0.910 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Part 1. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Part 2. Calculate the minimum Ag+...
Part A A 110.0-mL sample of a solution that is 2.7 x 10- M in AgNO, is mixed with a 230.0-mL sample of a solution that is 0.11 M in NaCN. For Ag(CN)2,Kf = 1.0 x 1021 After the solution reaches equilibrium, what concentration of Ag+ (aq) remains? Express your answer using two significant figures. IVO ACV O O ? [Ag +) =
References Calculate the final concentrations of (For BaC,0., K= 2.3 x 10 ) (aq), C,0,- (aq). Ba?' (aq) and Br" (ag) in a solution prepared by adding 0.100 L of 0.170M K,C,0, to 0.390 L of 0.380M BaBrg. Concentration of K. (aq) = Concentration of C,0,-(ag) - Concentration of Baº (aq) = Concentration of Br" (aq) Submit Answer Try Another Version tomatempts aning