What minimum concentration of thiosulfate ion, S2O3, should be present in 0.10 M AGNO3(ag) so that AgCls) does not precipitate when the solution is also made 0.010 M in Cl(aq)? For AgCl, Kyp = 1.8 x 10-10; for Ag(S2O3)2, K=1.7 x 1013.

Sodium sulfate is slowly added to a solution containing 0.0500 M Ca²+ (aq) and 0.0300 M Ag+ (aq). What will be the concentration of Ca²+ (aq) when Ag₂SO4(s) begins to precipitate? Solubility-product constants, Ksp, can be found in the chempendix. [Ca²+] = 0.00371 What percentage of the Ca²+ (aq) can be precipitated from the Ag+ (aq) by selective precipitation? 99.99 percentage: Incorrect M

[PBCI,] complex K; = 2.5 x 1015 For the aqueous at 25 °C. Suppose equal volumes of 0.0030M Pb(NO,) solution and 0.38M KCl solution are mixed. Calculate the equilibrium molarity of aqueous Pb- 2+ ion. Round your answer to 2 significant digits. ?

The solubility product, Ksp, for Fe(OH)3 is 1.6 × 10–39. What is the solubility of Fe(OH)3 in a buffer solution with pH = 10, in moles per litre?   A) 1.1 × 10–9 mol.L–1  B) 4.0 × 10–23 mol.L–1 C) 8.8 × 10–11 mol.L–1 D) 1.6 × 10–27 mol.L–1

Calculate the final concentrations of K* (aq), C20,2- (aq), Ba?+ (aq) and Br (ag) in a solution prepared by adding 0.100 L of 0.170 M K2C2O, to 0.280 L of 0.220 M ВаBrz. (For BaC204, Kp = 2.3 x 10-8.) Concentration of K* (aq) M Concentration of C20,2- (aq) M Concentration of Ba?+ (aq) M Concentration of Br (aq) M

Given the following values of equilibrium constants: [Ag(NH,)2]* = Ag* (aq) + 2NH3(aq) K 6.3 x 10-5 Ag,SO3(s) = 2Ag* (ag) + SO?-(aq) K= 1.50 x 10-14 What is the value of the equilibrium constant for the following reaction? Ag, SO3 (s) + 4NH3 (aq) = 2[Ag(NH,)2]+ +SO (aq)

A solution contains 0.036 M Cu2+ and 0.044 M Fe2+. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuS) = 1.3 × 10-36, Ksp(FES) = 6.3 × 10-18 == 3.6 × 10-35 M, FeS 3.6 x 10-35 M, CuS 1.4 x 10-16 M, CUS 1.4 × 10-16 M. FeS No precipitate will form at any concentration of sulfide ion.

The overall K, for the complex ion Ag(NH3)2 is 1.7 x 107. The Rp for Agl is 1.5 x 10-16 What is the molar solubility M in NH3? 8.4 x 10-5 O 1.5×10 9 O1.0 × 10 -4 O 5.8 x 10-12 O 1.3 x 10

Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na₂SO4 (aq) at 25°C. The Ksp of CaSO4 is 4.93 x 10-5. solubility: g/L