Question

The formation constant* of [M(CN)44]2− is 7.70×10167.70×1016, where M is a generic metal. A 0.1600.160 mole...

The formation constant* of [M(CN)44]2− is 7.70×10167.70×1016, where M is a generic metal.

A 0.1600.160 mole quantity of M(NO3)2 is added to a liter of 0.8600.860 M NaCN solution.

What is the concentration of M2+ ions at equilibrium?

[M2+]=[M2+]=

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is a generic metal. A...
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is a generic metal. A 0.160-mole quantity of M(NO3)2 is added to a liter of 1.070 M NaCN solution. What is the concentration of M2 ions at equilibrium?
A 0.160-mole quantity of NiCl2 is added to a liter of 1.20 M NH3 solution. What...
A 0.160-mole quantity of NiCl2 is added to a liter of 1.20 M NH3 solution. What is the concentration of Ni2+ ions at equilibrium? Assume the formation constant* of Ni(NH3)6^2 is 5.5 × 10^8
A 0.130-mole quantity of CoCl2 is added to a liter of 1.20 M NH3 solution. What...
A 0.130-mole quantity of CoCl2 is added to a liter of 1.20 M NH3 solution. What is the concentration of Co2 ions at equilibrium? Assume the formation constant* of Co(NH3)62+ is 5.0 × 1031 M–6. The balanced equation is: Co2+ + 6NH3 <==> Co(NH3)62+ The ICE table is: I:    0.13,      1.2,    0 C:      -x,       -6x,   +x E: 0.13-x, 1.2-6x,    x k=[Co(NH3)62+]/[(Co2+)(NH3)6] 5.0x1031=(x)/[(0.13-x)(1.2-6x)6]
Calculate the equilbrium concentration of Zn2 (aq) in a solution that is initially 0.150 M Zn(NO3)2...
Calculate the equilbrium concentration of Zn2 (aq) in a solution that is initially 0.150 M Zn(NO3)2 and 0.800 M NaCN. The formation constant for [Zn(CN)4]2- (aq) is Kf = 2.1 x 1019. Please show all of your work and include any formulas you use! Thank you!
1)Which of the following will be more soluble in an acidic solution than in pure water?...
1)Which of the following will be more soluble in an acidic solution than in pure water? PbSO4, Cd(OH)2,AlPO4, CsClO4, AgCl 2)Which of the following will be more soluble in an acidic solution than in pure water? PbS, AgCl, CsClO4, Zn(OH)2, CaCO3 3)A 0.140-mole quantity of NiCl2 is added to a liter of 1.20 M NH3 solution. What is the concentration of Ni2 ions at equilibrium? Assume the formation constant* of Ni(NH3)62 is 5.5 × 108. ____M
Consider the decomposition of a metal oxide to its elements where M represents a generic metal:...
Consider the decomposition of a metal oxide to its elements where M represents a generic metal: M2O3 (s) -----------------------> 2 M (s) + 3/2 O2 (g) Delta Gf (kj/mol) for M2O, M and O = -8.10, 0, 0 <------------------ 1. What is the standard change in Gibbs energy for the reaction as written in the forward direction? Delta Grxn = ? kj/mol 2. What is the equilibrium constant for this reaction as written in the forward direction at 298 K?...
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(OH)2(s) <--> M2+(aq) + 2OH-(aq)...
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(OH)2(s) <--> M2+(aq) + 2OH-(aq) Ksp= 3x10-16 M(OH)2(s) +2OH-(aq) <--> [M(OH)4]2-(aq) Kf= 0.05 Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.
Consider the decomposition of a metal oxide to its elements where M represents a generic metal:...
Consider the decomposition of a metal oxide to its elements where M represents a generic metal: M2O (s) ⇌ 2 M (s) + 1/2 O2 (g) Substance: ----> ∆G°f (kg/mol): M2O(s) ----------->-7.00 M(s) --------------> 0 O2(g) --------------->0 1. What is the standard change in Gibbs energy for the reaction as written in the forward direction? ∆G°rxn = ? kj/mol 2. What is the equilibrium constant for this reaction as written in the forward direction at 298 K? K = ?...
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations...
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A] = 0.100 M, [C] = 0.0340 M, and [AC5] = 0.100 M. Determine the formation constant, Kf, of AC5. The solubility of AB(s) in a 1.000-M solution of C(aq) is found to be 0.163 M. What is the Ksp of AB?
One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in...
One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108 What is the initial concentration of Ni(NO3)2 in the solution? _____M What is the equilibrium concentration of Ni2+(aq ) in the solution? ______M
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT