**Formation Constant and Equilibrium Concentration Problem** The formation constant (\(K_f\)) of \([M(\text{CN})_2]^{-}\) is \(5.30 \times 10^{18}\), where \(M\) is a generic metal. A 0.160 mole quantity of \(M(\text{NO}_3)\) is added to a liter of 0.550 M NaCN solution. **Question:** What is the concentration of \(M^+\) ions at equilibrium? \[ [M^+] = \underline{\hspace{2cm}} \text{ M} \] *Note: There are no graphs or diagrams associated with this content.*

Formation Constant and Equilibrium Concentration Problem The formation constant (\(K_f\)) of \([M(\text{CN})_2]^{-}\) is \(5.30 \times 10^{18}\), where \(M\) is a generic metal. A 0.160 mole quantity of \(M(\text{NO}_3)\) is added to a liter of 0.550 M NaCN solution. Question: What is the concentration of \(M^+\) ions at equilibrium? \[ [M^+] = \underline{\hspace{2cm}} \text{ M} \] Note: There are no graphs or diagrams associated with this content.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Solve this question
To 200.0 ml of a solution of Al(NO3)3 with concentration (2.000x10^-3) mol L-1, (3.0x10^2) ml of (1.00x10^-1) mol L-1 NaF is added. Determine the concentration of free aluminum ions after equilibrium has been established.(K+(AIF63-) = 7.0 x 1019) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units
Calculate the concentration of cobalt(III) ions in a solution formed by mixing 150 mL of 0.200 M Co(NO,), with 250 mL of 5.00 M NH, solution given K, of [Co(NH₂) 13+ is 4.5×1033. [Co³+]= M
The solubility product of Mg(OH)2 is 1.2x10-11. Predict whether a precipitate will beformed or not if 20.0 mL of 0.01 M MgCl2 solution is mixed with 30.0 mL of 1x10-3 MNaOH solution. Show supporting calculations
35 For the aqueous [Fe(CN), complex K₁=1.00 × 10³5 2+ Suppose equal volumes of 0.0078 M Fe(NO3), solution and 0.76M NaCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe²+ ion. Round your answer to 2 significant digits. []м 2 x10 Ś
If Ks (Ksp) refers to the dissolved solution at equilibrium and Q refers to the dissolved solution in general which of the following is true? Q, > Kg [Ag*] Q, = Kg Qg Ks the solution is supersaturated thus crystals will form. O a, b and c O b only O a only O b and c equilibium states
Determine if precipitation of Cu2O (s) will occur when 120.0mL of 4.00 x 10^-9 M (NH4)2O is added to 70.0mL of 5.00 x 10 ^-9 M Cu2SO4. Assume that both dissolve 100% in water. Ksp Cu2O=2.00 x 10^-28 Cu2O in Equilibrium with 2Cu+ and O2-
What happens when equal volumes of 2x104 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF, are combined? The K of calcium fluoride, CaF 2, is 4.0x10-11, sp O a. Q K; no precipitate forms c. Q K; a precipitate forms
2b
R456
11. The Kf for [AIF6]³- is 7.0 x 101⁹ and the corresponding equilibrium is shown below. Calculate the concentration of Al³+ ions in a solution that is initially 0.83 M in [AlF6]³-. Al³+ (aq) + 6 F-(aq) [AIF6]³(aq)
Q1) In titration of the solution containing 0.1 Molar of I'and 0.1 Molar of Cro,", with the solution of 0.1 molar of Ag+ , what is the titration error in first step? if the end point of first titration will be taken on the precipitation of Ag.Cro. KSP(Ag.Cro.)=10112 KSP(Agl) = 10.1