Question：use the mass% ethanol to calculate how much ethanol is in each fraction. Fraction 1 ：Totol mass is 15.87g.（mass percent：79%） Fraction 2 ：10.71g. （mass percent：43.75）
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A: Given: Mass of chloroform = 49 g Mass of acetyl bromide = 53 g Mass of acetone = 29 g.
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Q: Best Value for % Purity How did you arrive at the best value?
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A: D5 1/4 NS solution means D5 0.45 NS => 5% Dextrose in 0.225% Saline (D5 1/4NS)
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- Calculate the molarity of solutions prepared by dilution or calculate the quantities needed to carry out a dilution to prepare a solution of a specified concentration.Do parts per million denote a concentration that is a mole ratio?Does the concentration of a component in a mixture depend on the amount of the mix-ture?Chemistry A group of students was tasked with synthesizing dibenzalacetone (DBA) in the lab. They used acetone as limiting reagent, calculated their TY to be 8.0 g DBA, obtained 14.0 g crude product (wet) and their % Yield was 65%. What was the actual yield for their final product (recrystallized, dry DBA)? What was the minimum volume (ml) of ethanol they needed to recrystallize their wet crude? What was the amount of impurities (side products, moisture,...) contained in their wet crude?
- A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g /mL. Calculate the % by weight of CaCl2 in the solution described above.1)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain?Express your answer to the correct number of significant figures. 2)Suppose the Na2CO3 solution described in Question 1 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?2) Calculate the %Yield of the 4 fractions based on the following numbers. Compare these numbers with your optical result (inspection of the amount of material on the bottom of each Erlenmeyer flask). Crude fraction from 1 egg 1.28g %Yield Fraction 1 0.3 g Fraction 2 0.42 8 Fraction 3 0.41 8 Fraction 4 0.12 g
- Suppose a student starts with 2.4094 g of a sand mixture and separates the components into 1.3012 g of NaC1, 0.5266 g of SiO2 , and 0.4503 g of CaCO3 . Based on the amount of recovered SiO2, what is the percent of SiO2 in the starting mixture? Type answer:What is the volume of concentrated HCl to make 100 mL of 0.10 M HCl? ( density of concentrated HCl = 1.20 g/ml, mass %=37% by mass)A water solution of sulfuric acid (H2SO4) has a density of 1.864 g/mL and is 73.0% H2SO4 by mass. How many moles of H2SO4 are contained in 562.797 mL of this solution?
- O 3G lI.. CHEM 310 and 312 Homework O... p CHEM 310 and CHEM 312 Homework # 1 Q1) The combustion of an 8.23-mg sample of unknown substance gave 9.62 mg CO: and 3.94 mg H:0. Another sample, weighing 5.32 mg, gave 13.49 mg AgCl in a halogen analysis. Determine the percentage composition and empirical formula for this organic compound.Using (i) a right triangular plot and (ii) an equilateral triangular plot, solve the following problem graphically. The following mixtures are completely mixed to form mixture D: Mixture Mass (kg) % NaCI % KCI % H2O A 50 50 50 В 100 20 80 C 75 40 60 1. Adding first mixtures A and B to yield the resultant mixture F. Then, add mixture F to mixture C to locate mixture D. 2. If 25 kg of H2O was removed from mixture D to produce mixture E, locate E and determine its composition.Limestone is typically 50.0% (w/w) CaCO3. How many grams of CaCO3 are present in a limestone sample weighing 1.2 kg?
