Copper_LabProtocol

The formation constant of a silver cyano complex is 5.6 x 10-8 Ag+ + 2 CN Ag(CN), If a certain solution have the equilibrium concentrations of 5.0 x 10 M and 0.20 M for Agt and CN, respectively, then what is the equilibrium concentration for the silver cyano complex? O1.1 x 1015 05.6 x 1015 O2.8 x 1016 O2.4 x 109

2. (a) When there are extra chloride ions in solution, [CoCl4]2– complex ions can form, which are a different color than the Co2+ ions. Suppose 20% of the Co2+ ions form the complex ions when a student uses aqueous NaCl solution instead of deionized water (he/she picked up the wrong bottle by mistake). How would the presence of [CoCl4]2– complex ions affect the % transmittance values the student reads from the spectrophotometer? Explain. (b) How are the absorbance values changed?

You need 6 grams of copper ammine complex. The general formula for the copper ammine complex is [Cu(NH3)x]SO4*H2O. Calculate the formula weight for several values of x, x=2 through x=6.

4. Copper (II) sulfate pentahydrate is reacted with potassium oxalate monohydrate to form solid potassium bis(oxalato)cuprate(II) dihydrate. Considering the yield of reaction is 70% and ligand is used 10% excess, how many grams of copper (II) sulfate pentahydrate and potassium oxalate monohydrate should be used to produce 1.54 g of the complex? CUSO4.5H,O (aq) K,SO4(aq) + 2 K,C,04.H,0 (aq) + 3H,O → K,Cu(C,O,)2.2H,O

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

In photography, unexposed silver bromide was removed from film by soaking the film in a solution of sodium thiosulfate, Na2S2O3. Silver ion, Ag+, forms a soluble complex with the thiosulfate ion, S2O3-2, that has a formula of Ag(S2O3)2-3, and the formation of the complex causes the AgBr in the film to dissolve. The formation of the complex has a Kf of 2.0 x 10^13 while the Ksp of AgBr is 5.0 x 10^-13. How many grams of AgBr will dissolve in 125 mL of 1.20 M Na2S2O3 solution?

For the aqueous complex at Fe (CN)6]4-complex Kf= 1.0 x 10^35 Suppose equal volumes of 0.0062M Fe(NO2) solution and 0.10M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe^2+ ion. Round your answer to 2 significant digits.

3) The complex pentamminecarbonatocobalt(III) nitrate was prepared using the starting materials: 5g of cobalt(II) nitrate hexahydrate, excess concentrated ammonia, 12g of ammonium carbonate, and excess hydrogen peroxide. If the reaction gave 3g of actual product, calculate the percentage yield of the complex? Write equation for the reaction. Answer:

4. Continuing on with the analysis of the Ni-en complex as found in question #3, 40 mL of dimethylglyoxime, DMG, solution was added to the titrated nickel-en complex solution. The resulting beautiful red complex, Ni(DMG), was collected by filtration and found to weigh 0.232 g. What is the mass (in grams) of Ni in the Ni-en complex analyzed? 5. Determine the empirical formula of the complex synthesized in questions #3 and #4 above. 6. Assuming 0.900 g of NISO, 6 H,O was used to synthesize the Ni-complex in question 5 and 1.000 g of the Ni-complex formed caleulated the theoretical and percent yield. Refer to the pre-lab videos for information and examples of these calculations.

In the Inorganic laboratory, you made a dark red complex ion when you mixed potassium thiocyanate solution (KSCN) with iron(III) nitrate solution. The formula for this complex ion is [Fe(SCN)(H₂O)5]* where x is the charge of the ion. i) Write the chemical formula for iron(III) nitrate. ii) Determine overall charge and co-ordination number of iron in this complex ion. iii) Draw an energy level diagram for the crystal field splitting of high-spin iron(III). Place the electrons and label the orbitals. iv) Briefly explain why these iron complexes are colored.

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?

1. Why the copper (II) aspirinate complex can be precipitated in water? 2. What is the coordination and geometry of the copper (II) aspirinate complex? 3. How do we purify the copper (II) aspirinate complex from impurities and why we perform these steps? Please help me discuss question 1,2 and 3

The formation of a complex between cobalt (III) cation and six ammonia (NH3) ligands is very favorable (K₁ = 2.3 x 10³3). Given an initial cobalt concentration of 0.0235 M and an initial ammonia concentration of 0.206 M, what will be the concentration of free cobalt ion (Co³+) at equilibrium? 1.4 x 10-28 M 4.3 x 10-34 M 3.3 x 10-41 M 1.2 x 10-27 M 1.6 x 10-34 M

The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration.   increasing the concentration of Fe3+ decreasing the concentration of Fe(SCN)2+ increasing the temperature of the system

The complex ion Cu(NH3), is formed in a solution made of 0.0500 M Cu(NO)2 and 0.300 M NH. What are the concentrations of Cu**, NH3, and Cu(NH3)4t at equilibrium? The formation constant*, Kr, of Cu(NH)t is 1.70 x 10". (Cu = [NH,] = M. |Cu(NH, = M

The formation of a complex between cobalt (III) cation and six ammonia (NH3) ligands is very favorable (K₁= 2.3 x 1033). Given an initial cobalt concentration of 0.0235 M and an initial ammonia concentration of 0.206 M, what will be the concentration of free cobalt ion (Co3+) at equilibrium? 1.2 x 10-27 M 1.6 x 10-34 M 3.3 x 10-41 M 4.3 x 10-34 M 1.4 x 10-28 M Cobalt (II) carbonate is slightly soluble in water (Ksp = 1.0 x 10-10). In the presence of an excess of ammonia, Co²+ forms a complex with six ammonia ligands that is somewhat favorable (K₁ = 1.3 x 105). What is the value of the equilibrium constant (Koverall) for the overall reaction that occurs? COCO3 (s) +6 NH3 (aq) → Co(NH)32+ (aq) + CO32- (aq) 1.3 x 10-5 3.6 x 10² 7.7 x 10-16 1.3 x 105 1.0 x 10-10

Consider the reaction: Cu2+(aq) + 4NH3(aq) 2 Cu(NH3)4²*(aq) Kf = 1.7x 1013 %3D What is [Cu2+] remaining in solution after 0.020 mol of CuSO4 is dissolved in 1.00 L of 0.70 M NH3? Assume no change of volume. O 3.8 x 10-14 M. 1.6 x 10-14 M 1.1 x 10-13 M 8.0 x 10-15 M 5.0 x 10-13 M

Consider the following complex ion: [Cu(NH3)4]2+ Calculate the concentration of free, uncomplexed Cu2+ ions in a solution that originally contains a total of 1.0 × 10-3 M copper (II) ions and an equilibrium concentration of 0.10 M NH3. (Kf=4.8 x 1012)

A student set up the reaction with 0.048 M Fe3+ and 1.0x10-4 M SCN. They end up with an equilibrium concentration of [Fe(SCN)]2+ of 4.7x10-5 M. Based on these results, what is the value of the equilibrium constant Ke?

Part A. Colors of the Complex Ions. Identify the color of the ion or complex ion observed. Complex Ion (or Ion) Color Complex Ion (or Ion) Cu(OH)2 [Co(H2O)%]2+ [COC14] [Cu(NH3)4(H₂O)2]+ [CuCl4] [Cu(H₂O)6]2+ Color him and nerturbation For the temperature

Chemistry A lab student analyzed her nickel-en complex for ethylenediamine, en, content. A 0.288 g sample of the synthesized Ni-en complex was dissolved in about 50 mL of water and titrated with 0.154 M HCl (aq). Endpoint required 27.02 mL of the HCl (aq). What is the mass (in grams) of en in the Ni-en complex analyzed?

2+ For the aqueous [Ni(NH3) [Ni(NH3)]²+ complex K₁ = 5.50 × 108 at 25 °C. Suppose equal volumes of 0.0078M Ni(NO3), solution and 0.96M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. Round your answer to 2 significant digits. M 0x₁ x10 X ? Ś

What is the equilibrium constant expression for: 4 NH3(g) + 502(g) = 4 NO(g) + 6 H20(1) [NH313[022 [NO][H20]2 O [ANOJ*(6H2O]6 [4NH3]4[502]5 NO]4 [NH3)4[O2]5 NO]H2] [NH2][O2] [NH3]4[02]5 NO]4

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?

Calculations Given the following data, determine the % by mass of oxalate (C204²) in a sample of an iron oxalate complex with the general formula K2[Fe,(C204)y].WH2O. The reaction between oxalate and permanganate is as follows: 6H* + 5(COOH)2 + 2MnO4 → 10CO2 + 2Mn²* + 8H20 m(iron oxalate complex) used to make up 25.00 mL of solution: 0.25 g Volume of iron oxalate solution used for titration: 2.000 mL C(KMNO4) standard solution = 0.0200 M %3D M(C2042) = 88.02 g mol·1 Titre volume = 2.21 mL Enter your answer to 3 significant figures. Do not enter units. Very large or small numbers can be entered in scientific notation - for example enter 1.23E- 4 to represent 1.23x104. Answer:

The equilibrium-constant expression for the reaction Ti (s) + 2CI 2 (g) TICI 4 (1) is given by O [Ti (s)] [Cl2 (g)F [TIC14(1}] [TIC14 (1)] [Ti (s)] [Cl2( g))? [TIC14 (1)] [Ti (s)] [Cl2 (g)] O [TIC14 (1)] [Cl2 (g))? O [Cl2 (g)]2

Solid BaF2 is added to a solution of 1.0 M KF. What is the equilibrium concentration of the barium ion? 5.8 x 10-10 M 4.9 x 10¹3 M 1.2 x 10¹5 M 24 x 10¹5 M

1. What is the balanced net ionic equation for the equilibrium involving complex ions, CoCL42- and [Co(H2O)6]2+. 2. When heating the mixture the color was blue and when cooled it was pink. Based on this, is the forward reaction endothermic or exothermic and why? What is the balanced net ionic equation when heat is included?  3. How could an alcohol solution of CoCL2 beused to predict rain?