Describe the preparation of a) 500 ml of 0.0550 M silver nitrate solution from solid silver nitrate b) 5.00 L of a solution that is 0.0800M in K* starting with solid K3FE(CN), c) 2.00 L of 0.135 M perchloric acid from the commercial reagent [60% perchloric acid (w/w), specific gravity 1.60] d) 9.50 L of a solution that is 60.0 ppm in Na*starting with solid Na2sO4.
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- One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?Perform the necessary calculations for the preparation of: a) 200 mL of AgNO3 0.50 M from the solid reagent b) 1 L of HCl 0.25 M and N, consider the purity and density of the acid to perform the calculations c) 100 mL of potassium dichromate K2Cr2O7 (294.185 g/mol) 0.2 NAlthough 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 0.2182g sample of NaCl was assayed by the Volhard Method using 50mL of 0.0985N AgNO3 and 11.75mL of 0.1340N NH4SCN. Calculate the %NaCl in the sampledescribe how you can prepare 500mL of 0.10 M Fe2O3 (159.69g/mol) from the primary-standard-grade solid.1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.
- M is a cation which exists as a nitrate compound in an aqueous solution. Part of this solution is separated andH2S gas is sent. Then a black precipitate is given. Next, another part of this M's nitrate solution is separated.When NaOH is added, white precipitate is given. With excess NaOH, white precipitate dissolve and givecolourless solution. What could be the cation?Calculate the solubility of BaSO4 with the Ksp = 1.08 x 10-10 ,in an aqueous solution with I = 0.0010 mol kg-1Describe the solution's preparation: i) 250 mL of 0.0750 M AgNO3 from the solidreagent ii) 500 mL of 4.75 % (w/v) aqueous ethanol iii) 250 mL solution of 25 ppm of Na+ from solid sodium sulfate (Na2SO4)
- 50.0 mL of a 0.60 M solution of pyridine in ethanol is to be prepared by measuring out a known volume of pure liquid pyridine and diluting to 500 mL with ethanol. The molar mass of pyridine is 79.1 g/mol, and its density at room temperature is 0.982 g/mL. What volume of pyridine is required for this solution?The solubility of Ag2SO3 is 5.5x10-3 g/L. Determine the Ksp. (MW of Ag2SO3=295.8 g/mole)One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?