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?
We want to determine the concentrations of Ag+, CN-, and Ag(CN)2- when 10.0 mL of 2.00...
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.
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 +) =
Calculate the equilibrium concentration of Ag+(aq) after 10.0 mL of 0.100 M AgNO3(aq) have been mixed with 10.0 mL of 1.00 M NaCN(aq).
3. When Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6] precipitates, as shown below. 2K [Fe(CN).] (aq) + Cl2(g) = 2K3[Fe(CN).J(8) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant (10 pts) At 25°C: [Fe(CN).]" (aq) + e[Fe(CN).]" (aq) E° = 0.356 V Cl2(9) + 2e → 2Cl(aq) E° = 1.360 V Ksp of K3 [Fe(CN)6] = 106.5 b. When 80.0 mL of 1.00 M KCN is...
3. When C12(g) is added to aqueous K4[Fe(CN).), [Fe(CN)]*- is oxidized to [Fe(CN).]>- and K:[Fe(CN)] precipitates, as shown below. 2K.[Fe(CN),](aq) +Cl2(g) = 2Ks[Fe(CN)2](3) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C [Fe(CN).J” (aq) + € → [Fe(CN).]" (aq) E = 0.356 V Cl2(g) + 2e → 2Cl(aq) E* = 1.360 V Kup of Kj[Fe(CN).] = 106.5 Answer: b. When 80.0 mL of 1.00 M KCN is added to...
10) 2.00 mL ofa 0.0500 M CusO, solution is mixed with 2.00 mL of a 0.0100 M solution of K. Ksp (CuF2) 1.61 x 109 a) (7 pts) What is the concentration of Cu (aq) ion in the solution after equilibrium is established? b) (6 pts) Water is added to bring the volume of the solution to 1.00 L, and the mixture is stirred until equilibrium is reestablished. Calculate Q for this mixture. Is all of the CuF2 dissolved?
A solution is prepared by mixing 47.00 mL of 0.024 M AgNO3 with 11.00 mL of 1.0×10-3M Na2CO3. Assume that volumes are additive. Calculate [Ag+], [CO32–], [Na+], and [NO3–] after equilibrium is established. [Ag+]= [CO32+]= [Na+]= [NO3-]=
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2.. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6]2+ at equilibrium? Kf for [Ni(NH3)6]2+ = 2.0 x 108
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6]2+ at equilibrium? Kf for [Ni(NH3)6]2+ = 2.0 x 10^8
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2.. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6] 2+ at equilibrium? Kf for [Ni(NH3)6] 2+ = 2.0 x 10^8