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- I need help completing a lab report for chemistry. I attached assignment questions and lab obervations. Important notes: - The salt I worked with was a hydrated CaCl2*(H2O)2 salt. - Density for 1st diluted salt solution was 0.968g/mL, mixed 22mL of salt solution with 6mL of water - Density for 2nd diluted salt solution was 0.944g/mL, mixed 15mL of salt solution with 13mL of water -Density for 3rd diluted salt solution was 0.956g/mL, mixed 8mL of salt solution with 20mL of waterA student trying to determine the Ksp for Calcium hydroxide used 10.15 mL of 0.050 M HCl to neutralize the initial volume of 15.00 mL Ca(OH)2 solution. If the accepted value of the Ksp for Ca(OH)2 is 6.5 x 10-6 calculate the percent error from this experiment.Using recrystallization techniques, a student attempts to purify 0.50 g of compound H. Based on the solubility of H in the chosen solvent at collection temperature, the maximum percent recovery is 82%. The student obtains 0.396 g of purified crystals. What is their percent recovery? Group of answer choices 41% 64% 79% 82% 97% none of these
- The separation and purification processes given below and the method used against them are given. Which or which of these pairings are correct? Brewing the tea - Extraction Purification of water from impurities-Chromatography Separating olive pomace from oil while olive oil is being produced - Decantation Obtaining oil fractions - Ordinary distillation Obtaining essential oils and using them in perfume making - Water-steam distillation A. I, IV, V B. I, II, III, IV, V C. I, II, V D. I, II, III, V E. I, II, III, IVYou are asked to create a 0.35 M solution of calcium chloride (CaCl2) using a 250.0 mL volumetric flask. a.You have two solvents, difluoromethane (CH2F2) and ethanol (C2H5OH) available to dissolve your CaCl2. Which solvent would be more appropriate to use? Justify your response in 2 sentences or less.1. Calculate the mass required to prepare a 250 mL 3 M NaCl in water.Mass = M x MM x V 10002. Calculate how to prepare the following dilutions, ½, ¼, 1/8 and 1/16 of the initial concentration.There is a helpful equation that is used to determine how much stock solution and how much diluent to combine to get the final solution of a desired concentration
- Calculate the solubility of CuCO3 in water at 25C. Ksp = 3.00x10-12. Round the answer to two significant figures.Why do Sedimentation and filtration is important in water treatment?Is a period of timeimportant in water purification?For 0.250 L of aqueous solution with a density of 1.00 g/mL containing 13.7 mg of pesticide, express the concentration of pesticide in ppm and ppb.
- 0.02 M NaOH reagent was standardized using 0.1000 g Potassium hydrogen phthalate (204.22 g/mol) and it required 25.8 mL to reach end point. What is the molar concentration required?You have to make 50 mL of 0.05M HCl from a 10M HCl stock solution, but the only measuring devices available are 100mL graduated cylinders and 10mL serological pipets. How could you accurately make the dilute HCl solution (clearly explain)?A chemist attempts to prepare some very pure crystals of borax by dissolving 100g of Na 2 B 4 O 7 in200 grams of boiling water. He then cools the solution slowly until some borax crystallizes out.Calculate the grams of borax recovered in the crystals per 100 grams of initial solution (Na 2 B 4 O 7plus water), if the residual solution at 55 0 C after the crystals are removed contains 12.4%Na 2 B 4 O 7 . What is the percent yield or percent recovery of Na 2 B 4 O 7 . (MW: Na =23, O =16, B=10.8,H =1) round off up to 4 decimal places