Copper(II) ions form a complex ion in the presence of ammonia [Cu(NH3)4 2+] [Cu2*(ag)][NH3]4 Cu²*(aq) + 4NH3(aq) = Cu(NH3)4²*(aq) Kc = 5.0x 1013 If 0.010 mol Cu2+ is added to 1.00 L of a solution that is 1.00 M NH3 what are the concentrations when the system comes to equilibrium?

Copper(II) ions form a complex ion in the presence of ammonia [Cu(NH3)4 2+] [Cu2(ag)][NH3]4 Cu²(aq) + 4NH3(aq) = Cu(NH3)4²*(aq) Kc = 5.0x 1013 If 0.010 mol Cu2+ is added to 1.00 L of a solution that is 1.00 M NH3 what are the concentrations when the system comes to equilibrium?

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

bot 3. Iron(II) ion (Fe°*) reacts with thiocyanate ion (SCN¯) to form a red complex ion with the formula [FESCN]2+. The net ionic equation describing this reaction is given in Equation 10. eH MC () Fe+ (aq, It. yellow) + SCN (aq, colorless)=[FESCN]²+ (aq, red) 12+ (Eq. 10) A student studying this equilibrium begins with an equilibrium mixture that is light pink. (1) What change will the student observe when a solution containing Fe³+ ion is added to this mixture?
The metal ion M2+ in ammonia, NH3 forms the complex ion M(NH3)62+ (Kf = 5.1x108). Calculate the M2+ concentration when the equilibrium concentrations of NH3 and M(NH3)62+ are 0.046 and 0.15 M respectively.
If 21.70 mL of 0.0500 M KMnO4 is required to titrate a 0.450 g sample of K3[Fe(C2O4)3]⋅3H2O ⋅what is the percent C2O2−4 in the complex?
The formation constant of a silver cyano complex is 5.6 x 1018 Ag+ + 2 CN Ag(CN)," If a certain solution have the equilibrium concentrations of 5.0 x 10-3 M and 0.20 M for Ag+ and CN", respectively, then what is the equilibrium concentration for the silver cyano complex? O1.1 x 1015 O5.6 x 1015 02.8 x 1016 02.4 x 109
Please show solution and explain [Co(H2O)6]2+ + 4Cl1- ⇋ [CoCl4]2- + 6H2O
Metallic cadmium is added to 0.350 L of an aqueous solution in which [Cr³+]o is 1.00 mol/L. What is the [Cr³+] eq concentration of the chromium(III) species at equilibrium? Kc=0.288 2Cr3+(ac)+Cd(s)<------->2Cr2+(ac)+Cd2+
Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH", the Al³+ (aq) ion forms a hydroxide complex ion, Al(OH)4. Calculate the concentration of free Al³+ ion when 1.20x10-2 mol AI(CH3COO) 3(S) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.90). For Al(OH)4, Kf = 1.1x1033. [A1³+] = Check & Submit Answer Show Approach M
7.00 grams of Cobalt (II) nitrate are dissolved in 1.00 liter of water. What is the initial concentration of CO (2+) in moles per liter? Then, 0.22 moles of solid KOH are added to this solution. The solution volume remains 1.00 liter. Given that Kf = 5.0 x 10^9 for the complex ion, Co(OH)4 (2-) find the final concentrations of Co (2+), Co(OH)4 (2-), and OH-. Also find the pH of this final solution.
write the reaction for the complex ion Cu(NH2)4SO4
Pl
Please use the values in the resources listed below instead of the textbook values. Sometimes equilibria for complex ions are described in terms of dissociation constants, Ka. For the complex ion Cu(CN)4 3- the dissociation reaction is as follows. [Cu*]• [CN 14 Kd [Cu(CN)43-] Cu(CN)4 3- = Cu+ + 4 CN- = 5.0X10° n-31 = Calculate the value of the formation constant, Kf, for Cu(CN)4°¯. 4.0
A compound formula with brackets is called a coordination complex, and the structure looks like a covalent compound with a transition metal central atom. The bonding that happens is often a hybrid of covalent and metallic bonding. One method of extracting silver from mined ore is by using a complex, K[Ag(CN)2], to make the silver soluble in water. The complex is then isolated to recover the silver using the following chemical equation. 2 K[Ag(CN)2] (aq) + Zn (s) → 2 Ag (s) + Zn(CN)2 (aq) + 2 KCN (aq) a.) 5.00 L of 1.25 M K[Ag(CN)2] is mixed with 215.5 g of zinc. Identify the limiting reactant and determine how many grams of silver are produced. b.) The quality control chemists at the mine record collecting 672.4 g of silver. What is the yield of this reaction?