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30 solutions

Formation Constant

Q. The average human body contains 5.20 L of blood with a Fe^2+ concentration of 2.30x10^-5 M. If a person ingests 12.0 mL of 24.0 mM NaCN, what percentage of iron (II) in the blood would be sequestered by the cyanide ion? Express the percentage numerically.

Solved • Feb 26, 2020

Formation Constant

Q. From the value of Kf listed in Table 17.1, calculate the concentration of Ni2+(aq) and Ni(NH3)62+ that are present at equilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of 0.20 M NH3(aq)

Solved • Mar 16, 2020

Formation Constant

Q. 9. What is the pH of a solution of 0.1 M Ba(OH)2 and excess Zn(OH)2 (s)? The Ksp of Zn(OH)2 is 3.0X10^-15 and the Kf of [Zn(OH)4]^2- is 2.0X10^15

Solved • Mar 5, 2020

Formation Constant

Q. 10. What is the molarity of NH3 remaining in solution when 0.400 mol of Cu(NO3)2 is mixed with 0.600 mol NH3 in 0.650 L of solution? The Kf of [Cu(NH3)4] 2+ is 1.1 X 10^13. Assume for this problem that NH3 does not react with water.

Solved • Mar 4, 2020

Formation Constant

Q. 9. What is the pH of a solution of 0.10 M Ba(OH)2 and excess Zn(OH)2(s)? The Ksp of Zn(OH)2 is 3.0 X 10-15 and the Kf of [Zn(OH)4]2- is 2.0 X 10^15.

Solved • Mar 3, 2020

Formation Constant

Q. Ni(OH)2(s) + 4CN(aq) ,<--> Ni(CN)4 2-(aq) + 2OH- (aq). knet = 2.8 x 10^14. If ksp for Ni(OH)2 is 2.8 x 10^-16, what is the value of the formation constant K form for the reaction below Ni+2(aq) +4CN-(aq) <--> Ni(CN)4 2- (aq)

Solved • Dec 17, 2019

Formation Constant

Q. For the aqueous [Cu(NH3)4]^2+ complex Kf = 5.6 x 10^11 at 25 °C. Suppose equal volumes of 0.0062 M Cu(NO3)2 solution and 0.88 M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Cu^2+ ion. Round our answer to 2 significant digits.

Solved • Dec 10, 2019