When 1.24 g of AgNO3 (169.1 g mol-1) is dissolved in 245 mL of 0.150 M NaCN, what are [Ag+], [Ag(CN)2-], and [CN-] at equilibrium? Kf of Ag(CN)2- = 1.0 x 1021.
When 1.24 g of AgNO3 (169.1 g mol-1) is dissolved in 245 mL of 0.150 M...
We want to determine the concentrations of Ag+, CN-, and Ag(CN)2- when 10.0 mL of 2.00 M KCN is mixed with 10.0 mL of 0.0200 M of AgNO3. Kf for Ag(CN)2- = 1.0 x 1021 a) What is the initial concentration of Ag ion (in M) after mixing but before reaction or equilibrium is established? b) What is the initial concentration of Ag ion (in M) after mixing but before reaction or equilibrium is established?
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 +) =
To a 250.0 mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0100 M AgNO3, 0.245 M NaBr, and 0.100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigorously What mass of AgBr would precipitate from this mixture? (Hint: The Ksp of AgBr is 5.4 x 10-13 and the Ky of Ag(CN)2-is 1.0 × 1021) Number g AgBr
A 0.5427 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water. AgNO3 was added to the solution, precipitating all of the CN− in solution as AgCN (MW=133.886 g/mol). The dried precipitate weighed 1.264 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt%= % NaCN wt%=
If 30.0 mL of 0.150 M CaCl2 is added to 31.0 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? ?g
If 30.0 mL of 0.150 M CaCl2is added to 29.5 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? g
4) When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.500 M NH4CI, how many grams of AgCl are formed? (MM AgCI =143.32 g/mol) AgNO3(ag)+ NH4C| (aq) AgCl(s)+ NH4NO3(aq)
A 50 mL sample of 2.2 x 10^-4 M CuNO3 is added to 50 mL of a 4.0 M NaCN. Cu^+ reacts with CN^- to form the complex ion Cu(CN)3^2- according to Cu^+(aq) + 3CN^-(aq) <--> Cu(CN)3^2- , Kf= 1.0 x 10^9 determine the concentrations of CN^-, Cu^+, Cu(CN)3^2- at equilibrium
Determine the concentration of Ag+ in a solution prepared by adding 0.10 mol AgNO3 to 1.0 L of 3.5 M NH3. Ag+(aq) + 2 NH3(aq) left right double arrow Ag(NH3)2+(aq) Kf= 1.7 x 107
What mass of barium sulfate (233 g/mol) is produced when 125 mL of a 0.150 M solution of barium chloride is mixed with 25 mL of a 0.175 M solution of iron(III) sulfate