If Ksp Ni(CN)2 = 3.0x10^-23, what concentration of CN- would reduce the equilibrium concentration of Ni+2 to 5.0mg/l? Please show all work, Thankyou.
If Ksp Ni(CN)2 = 3.0x10^-23, what concentration of CN- would reduce the equilibrium concentration of Ni+2...
a Ni(CN)2, nickel cyanide Ksp-3.0 x 10-23 Molar solubility mo/L [Ni2+] . CN Solubility g/L bPbla, lead(lI) odide Ksp8.7 x 10-9 Molar solubility mo/L Solubility g/L We were unable to transcribe this image
Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of the solution is buffered to pH=12.00 (so that the hydroxide ion concentration is 0.010 M). 1. Zn(OH)2(s) A. [Zn2] 3.0x10-12 M B. [Zn2 3.7x10- M C. [Zn23.0x10-10 M D. [Zn2] 9.1x10-3 M E. [Zn2] 1.5x10-13 M Zn2 (aq) + 20H (aq) Ksp 3.0x10-16 2. When silver carbonate, Ag,COs, is mixed with water, it dissolves to some extent to form a saturated solution where the...
What Is The Molar Solubility Of Nickel(II) Sulfide In 0.091 M CN-? For Nis, Ksp = 3.0 10-19; For Ni(CN)4²-, Kf,= 1.0x 10³¹. Show All Equilibrium Equations Involved Here. See the answer
What is the maximum concentration of Ni2+ in a solution of pH 10.00? Ksp (NI(OH)2) = 2.0*10-15 M
ksp= 8x10-12 A 350.0 mL sample of a saturated solution of Zn(CN)2 is at equilibrium at 25C. At equilibrium, the [CN-1) is 2.52 x 10-4 M. What is the molar solubility of Zn(CN)2? Enter your answer with units. If no units are required, write no units after your number.
The concentration of Mg2+ at equilibrium (25oC) is 0.000144 M. What is the value of Ksp at this temperature? In the solubility rules, Mg(OH)2 was listed as an "insoluble" salt. It is actually slightly soluble in an equilibrium reaction: Mg (OH)2 (s) Mg2+ (aq) 20H (aq) The concentration of Mg2+ at equilibrium (25°C) is 0.000144 M. What is the value of Ksp at this temperature? Submit Answer Tries o/99
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide. Ksp =___________ 2) Use solubility to calculate Ksp. The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide. Ksp =______________
calculate the ksp for Ca(IO3)2 if at equilibrium the concentration of IO3 ion is 2.35x10^-2 M.
at must be the equilibrium concentration of Question 1 (5 pts). A. If the equilibrium concentration of Ce is 0.00010 M, what must be the oqu Cod in the solution? K (Ce (CO)) -59% 10%. (Answer: 3.9 x 10M] B. If the concentration of Ca?" of the solution in 1A is in will some CaCO, begin to precipitate? K (Caco) -1.3 x 10". (Hint: What is the the association of Caland Co, at these concentrations and how does that compare...
The solubility of solid nickel hydroxide, Ni(OH)2, is governed by its Ksp= 6x10^-16. a) Write the equation for this dissolution reaction, and the equilibrium expression. b) Nickel ions undergo three complexations with hydroxide in basic solutions. Assume OH concentration to be 0.0010 M and pH to be 11, calculate the concentrations of Ni2+, NiOH+, Ni(OH)2, and Ni(OH)3-. logK1= 4.1 logK2= 3.9 logK3= 3