2.In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2with 8.000 NiCl2.6H20 to obtain the product Ni(NH2CH2CH½NH2j3Cl2 complex. TheC2H3N2 solution used in this experiment is 25.0% by mass, with a density (d) of0.950 g/mL.(MW NICI2.6H2O= 237.69 g/mole, MW C2HgN2=60.10 g/mole,MW tris(ethylenediamine)nickel(II)chloride = 309.89 g/mole)a. Write down the balanced equation of the synthesis.b. Determine the number of moles of each reactant that you use.c. Determine which reactant is the limiting reactant, giving your reasoning. Show allyour work to get full credit. (5 points)d. Calculate your percent yield if the dry product weighs 7.000 g.

The balanced chemical equation can be written as follows: NiH2O6Cl2 + 3C2H8N2 → NiC2H8N23Cl2 +…

2. In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2 with 8.000 NiCl2.6H2O to obtain the product Ni(NH2CH¿CHNH2y3Cl2 complex. The C2HạN2 solution used in this experiment is 25.0% by mass, with a density (d) of 0.950 g/mL. (MW NICI2.6H2O= 237.69 g/mole, MW C2H&N2=60.10 g/mole, MW tris(ethylenediamine)nickel(I)chloride = 309.89 g/mole) a. Write down the balanced equation of the synthesis. b. Determine the number of moles of each reactant that you use. c. Determine which reactant is the limiting reactant, giving your reasoning. Show all your work to get full credit. (5 points) d. Calculate your percent yield if the dry product weighs 7.000 g.

2. In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2 with 8.000 NiCl2.6H2O to obtain the product Ni(NH2CH¿CHNH2y3Cl2 complex. The C2HạN2 solution used in this experiment is 25.0% by mass, with a density (d) of 0.950 g/mL. (MW NICI2.6H2O= 237.69 g/mole, MW C2H&N2=60.10 g/mole, MW tris(ethylenediamine)nickel(I)chloride = 309.89 g/mole) a. Write down the balanced equation of the synthesis. b. Determine the number of moles of each reactant that you use. c. Determine which reactant is the limiting reactant, giving your reasoning. Show all your work to get full credit. (5 points) d. Calculate your percent yield if the dry product weighs 7.000 g.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter26: Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 26.15QAP

See similar textbooks

Similar questions

A sample of processed meat scrap weighing 4.000 g is digested with concentrated HSO. and Hg(catalyst) until the N present has been converted to NHHSO.. This is treated with excess NaOH, and the liberated NHs is caught in a 100-ml of H.SO. ( Iml 0.01860 g Na:OJ. The excess acid requires 57.60 ml of NaOH ( ImL = 0.12660 g potassium acid phthalate, KHCaH.OJ. Calculate the percentage protein in the meat scrap 4.
Express the equilibrium constant for the following reaction: 2 CH2CI2 (g) + Cl2 (g) =2 CHCI3 + H2 (g) [CHCI3]CH2] k = %3D [CHCI3]°[H2] k = %3D [CHCI,ICI,] [CHCI;]*tC!,] [CHCI;]°[H;] %3D [CHCI,ICI,] k%3D [CHCI;][H2] %3D [CHCI3][H2] k%3D [CHCI2[CI]
1. A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc. (2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample. Calculate the mass percent of NH3 in the product.
. When titrated in neutral solution with 0.05000 N I2, a mixture of As2O3, AS2O5, and inert material requires 20.10 mL. The resulting solution is then acidified, and excess KI is added. The liberated Iz requires 29.92 mL of 0.1500 N Na,S,O3. Calculate the sum of the weights of As2O3 and As2O5 in the sample.
4. If the following values are used... Measure the mass of 0.400 g of cobalt(II) nitrate hexahydrate (Co(NO;)2 -6H2O), and dissolve it in 15.0 mL of distilled or deionized water using a clean beaker. Using a graduated cylinder, measure out 10.0 mL of a prepared 0.10-M sodium phosphate (NazPO4) solution. ... determine which compound, (Na3PO4 or Co(N03)2 ·6H2O) will be the limiting reagent. Then determine the theoretical yield.
(iv) CI. (v) 2x (vi) O 요 CI OMe O NaOMe NaOMe NH3 + H (cat.) J (C5H8O4) K
A 0.8965g ore sample is dissolved in nitric acid and then filtered. The aluminum is present in solution as AP". The solution is made basic with ammonium hydroxide, NH,OH, and the aluminum hydroxide, Al(OH)» (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al;O; (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? Why rinse with ammonium hydroxide solution? What chemical transformation takes place during ignition? (Show the balanced chemical equation) • Why use a desiccator during cooling? Calculate the weight percent Al (AW 26.9815) in the sample. Al(OH)) -> Al;O, + H0
The solubility constant Ksp of Ag2CrO4 is related to its solubility in water (s) as Ksp
0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)
(f) Potassium permanganate (g) Sodium hypochlorite (h) Beryllium bicarbonate (1) Ammonium dichromate (G) Iron (II) chloride
What is the water solubility of BaCO3 (Kep = 2.6 x 10-9) in a solution containing 0.40 M CO, (aq)? %3D
(a) In 20 or less of yourown words define the term “leachate”and describe how it forms. (b) Previous records had shown that to prevent acute toxicity to organisms, the maximum mass of CdSO4 that should be allowed into the landfill was determined to be 0.1 kg. This was calculated using a standard concentration of Cd in mg/L where the volume of the leachate pond was used as 500 000L. (i) Provide the name of the CdSO4 compound. State the oxidation number of Cd in this compound (ii) You need to ensure that the concentration used to determine the mass of Cd allowed in the landfill, meets the current regulatory standard. Assuming that previous calculations determined that all of the CdSO4 would be deposited in the leachate pond, what standard concentration of Cd in mg/L was used to determine the maximum mass of allowable CdSO4?