3 4 You are studying coordination compounds of Cu(II with carbonate and other ligands. You add excess aqueous Na₂CO to 20.5 mL of 0.505 M aqueous CuSO. You observe a color change from deep blue to teal and the formation of 0.229 g CO₂. You isolate and dry a precipitate, with a mass of 1.163 grams. You hypothesize that the new compound is made up of copper(II) ligated to HO, and CO₂². How many grams of copper are contained in 8.15 grams of the compound? 2- 3

3 4 You are studying coordination compounds of Cu(II with carbonate and other ligands. You add excess aqueous Na₂CO to 20.5 mL of 0.505 M aqueous CuSO. You observe a color change from deep blue to teal and the formation of 0.229 g CO₂. You isolate and dry a precipitate, with a mass of 1.163 grams. You hypothesize that the new compound is made up of copper(II) ligated to HO, and CO₂². How many grams of copper are contained in 8.15 grams of the compound? 2- 3

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

Draw an example of an ionization isomer for [Pt(NH3)4] Cl2Draw an example of a coordination isomer for [Ag(NH3)2][Co(H2O)4(Cl)4] Draw an example of a linkage isomer for [Cr(NH3)5(SCN)] (NO3)2
4. Consider the following reaction: [ZnCl4]² +4 OH → [Zn(OH)4]² +4 CI If the reaction is spontaneous, then which of the following is true? (A) Chloride is a more labile ligand than hydroxide in zinc complexes (B) Hydroxide is a more labile ligand than chloride in zinc complexes (C) Chloride is a more inert ligand than hydroxide in zinc complexes (D) Hydroxide and chloride are equally labile in zinc complexes
What is the charge on each of the following complex ions? hexaaquairon(II), [Fe(H2O)6]? tris(carbonato)ferrate(III), [Fe(CO3)3]? diaquatetrachlorovanadate(III), [V(H2O)2Cl4]? Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).
The maximum absorption for the complex ion [Co(NH3)6]3+ is located at 470 nm. A)Predict the color of the complex and B) calculate the crystal field splitting inkJ/mol and cm-1.
The complex ion Fe(CN)6³ is paramagnetic with one unpaired electron. The complex ion Fe(SCN)6³ has five unpaired electrons. Draw the crystal field diagrams of two complex ions. Which compound absorbs light with the shorter wavelength? Where does SCN- lie in the spectrochemical series relative to CN-? (hint: stronger or weaker 4. (a) (b) (c) field)
1. Give the electron configuration (in t2g and eg forms) for Ti(III), Mn(II), and Ni(II) ions in: a) Octahedral (high spin) b) Tetrahedral crystal fields
When oxalate (chemical formula: C₂04²; ligand abbreviation: ox) is added to an aqueous solution of nickel(II), the octahedral complex [Ni(ox)3]4 is produced. Given that complex formation is sequential, which reaction corresponds to the stability constant, B₂? O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) = [Ni(ox)₂]4- (aq) + 6 H₂0 (1) O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) = [Ni(0x)2(H₂O)4]² (aq) + 2 H₂O(1) O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) ⇒ [Ni(ox)₂(H₂O)2]² (aq) + 4H₂O(1) O [Ni(H₂0)6]²+ (aq) + 2 OX(aq) = [Ni(ox)₂]² (aq) + 6 H₂0 (1)
You are synthesizing a coordination complex using the following reaction: FeCl3 + 3K2C2O4 H₂O → K3Fe(C₂O4)3 3 H₂O + KCl To do this you have weighed out 11.113 g of K₂C₂O4 · H₂O (molar mass is 184.24 g/mol, dissolved it in 20 mL of warm DI water, and added 10.00 mL of a solution containing 0.400 g/mL of FeCl3, with a molar mass of 162.20 g/mol. 1. How many moles of K₂C₂O4 H₂O are present? 2. How many moles of FeCl3 are present? 3. Calculate the theoretical yield in grams. The molar mass of the product is 491.2 g/mol.
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?
The pentacarbonyl metal, M(CO)5 complex, has two geometrical structures: trigonal bipyramidal or square pyramidal. Experimentally, it was found that the Ru(CO)5 complex show two stretching CO bands in the IR and three bands in the Raman region. According to these information, what would be the expected structure for Ru(CO)5?
Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a) [Ag(NH3)2]+ (b) square planar [Cu(NH3)4]2+
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?