You are required to prepare 5 L of a solution containing 1.000 x 103 mol/L of Cu2"(aq).Which of the following procedures would produce an appropriate solution?O Dissolve 0.0636 g of copper metal in nitric acid, add to a 5.000 Lvolumetric flask, dilute to themark with deionized water and mix well.O Dissolve 1.248 g of CuSO.5H,0(s) in deionized water, add to a 5.000 L volumetric flask, diluteto the mark with deionized water and mix well.Dissolve 0.250 g of CUSO,.5H,O(s) in deionized water, add to a 5.000 L volumetric flask, diluteto the mark with deionized water and mix well.

The molarity of a solution describes the number of moles of the solute present in one liter of…

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EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter13: Isolation Of Eugenol From Clov

Section: Chapter Questions

Problem 9Q

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When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?
A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.
A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixture
You are required to standardize a dilute solution of sulphuric acid, and undertake the following steps:(i) 4.805 g of solid sodium tetraborate (Na2B4O7) are added to a 250 mL volumetric flask, and the solution made up to the mark with distilled water.(ii) 25.00 mL aliquots of the stock solution from (i) are transferred to conical flasks, for titration against the sulphuric acid solution in the burette.(iii) You perform titrations using two different indicators: bromocresol green, and phenolphthalein.With bromocresol green, the average titre volume is 22.50 cm3, while with phenolphthalein, the average volume is 9.50 cm3.(a) Write the balanced equation for the reaction between Na2B4O7 and sulphuric acid
The aluminum in a 1.200 g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al(OH)3.xH2O. The precipitate was filtered and ignited at 10000C to give anhydrous Al2O3 which weighed 0.1798 g. Express the result of this analysis in terms of % Al2O3.
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It istherefore necessary to periodically determine the purity of the peroxide solutions.This can be done via a redox titration as follows: The density of a particular surgical grade hydrogen peroxide solution is 1.11g.cm-3. Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficientamount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a0.372 M KMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns apersistent bright pink due to the presence of excess permanganate ions. The average titration value is 26.20 mL of the KMnO4 solution 1.Determine the percentage of the hydrogen peroxide in the solution sample.2. Naturally occurring manganese…
1. It is found that 16.34 mL of a solution containing Ni* is required to titrate a sample of pure KCN weighing 0.5024 g. The reaction is Ni* + 4 CN" → Ni(CN),“ . Calculate the molarity of the nickel solution. From the following data calculate the normalities of the acid and base solutions: weight of pure Na2CO3 = 0.2448 g; volume of acid = 43.65 mL ; volume of base used in back titration = %3D 0.84 mL ; 1.000 mL of base = 0.982 mL of acid. Reaction: CO, + 2H* → H2CO3
Toxie chromate can be removed from solution uning the following reaction 2 Cro, lag) + 3SO4H'(ag)- Cry(SOls) + 2HyOA 5o, Is bubbled through 3.0x 10Lofa solution. All of the chromate is removed and 2.94 x 10 kg of the precipitate is formed. Calculate the initial concentration (in units of mM) of chromate in solution. Write only the numerical value below (without units) using the correct number of signihcant hpares. Type your answer Nest

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