5.A student began with a 3.12 g sample that contained their unknown and charcoal. After recrystallization...
5.A student began with a 3.12 g sample that contained their unknown and charcoal. After recrystallization the mass of dried crystals recovered was 2.61 g. What was the percent recovery?
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5.A
student began with a 3.12 g sample that contained their unknown and
charcoal. After recrystallization...
3 3. A student performs a crystallization on an impure sample of biphenyl. The sample weighs...
3
3. A student performs a crystallization on an impure sample of biphenyl. The sample weighs 0.5 g and contains about 5% impurity. Based on his knowledge of solubility, the student de- cides to use benzene as the solvent. After crystallization, the crystals are dried and the final weight is found to be 0.02 g. Assume that all steps in the crystallization are performed cor- rectly, there are no spills, and the student lost very little solid on any glassware...
The solubility of acetanilide is 12.8 g in 100 mL of ethanol at 0 ∘C, and...
The solubility of acetanilide is 12.8 g in 100 mL of ethanol at 0 ∘C, and 46.4 g in 100 mL of ethanol at 60 ∘C. What is the maximum percent recovery that can be achieved for the recrystallization of acetanilide from ethanol? A student was given a sample of crude acetanilide to recrystallize. The initial mass of the the crude acetanilide was 171 mg.The mass after recrystallization was 125 mg. Calculate the percent recovery from recrystallization.
What is the literature (known) melting point for acetanilide? A student performed a recrystallization to purify...
What is the literature (known) melting point for acetanilide? A student performed a recrystallization to purify a crude sample from a reaction. The amount of crude material collected from the reaction was 13.56 grams. After the purification, the student collected 8.97 grams of extremely pure material. a. What is the percent recovery of the desired material? b. Is it possible to determine how much of the desired material remained in solution after the filtration? The solubility of acetanilide in hot...
Number of Unknown Sample Mass of Beaker #1 and Sample a-b=2,129 52.4779 - 50.348g 2.1299 -B0.35g...
Number of Unknown Sample Mass of Beaker #1 and Sample a-b=2,129 52.4779 - 50.348g 2.1299 -B0.35g 14.7009 DATA SUMMARY 4 52.4719 Mass of Beaker #1 50.341.4 Mass of Sample d Mass of Beaker 2 + NaCl (dried) 14. 1994 e Mass of Beaker #2 \r. 4019 f Mass of NaCl Recovered 2.4519 Mass of Filter Paper and Sio, (dried) 9 h Mass of Filter Paper 0.8129 Mass of Sio, Recovered J f + i=1.998g Total Mass of NaCl + SiO,...
solve 3 and 4 1989 Cengage Learning chlorine ions 5. A student was asked to determine...
solve
3 and 4
1989 Cengage Learning chlorine ions 5. A student was asked to determine the percentage of the components of a mixture of potassium bromide (KBr), magnesium hydroxide, Mg(OH)2, and barium sulfate (BaSOA). The mass of the sa- mple of the mixture used was 3.21 g. The student extracted the KBr from the mixture with water and filtered insoluble Mg(OH)2 and BaSO, from the solution, containing the KBr. After evaporating the filtrate, the student recovered and dried the...
A laboratory group began the recrystallization process with. 0.856-grams of synthesized aspirin. After they carefully completed...
A laboratory group began the recrystallization process with. 0.856-grams of synthesized aspirin. After they carefully completed the necessary steps to purify their sample via recystallization, they were left with 0.581-grams of aspirin. What is the group's percent yield?
A student was asked to determine the percentage of each component in a mixture of sodium...
A student was asked to determine the percentage of each component in a mixture of sodium nitrate (NaNO3) and calcium carbonate (CaCO3). The mass of the sample used was 2.96 g. The student extracted NaNO3 from the mixture with water and separated the insoluble CaCO3 from the solution by filtration. After evaporating the filtrate, the student recovered and dried the NaNO3, and found that it weighted 0.49 g. The student dried the insoluble residue of CaCO3 and found that it...
please answer all 5. Suppose you started with 10 g of impure compound A which was...
please answer all
5. Suppose you started with 10 g of impure compound A which was 80% pure, and after recrystallization you recovered 5 g of pure A. Calculate percent recovery. (5 points) 6. Should recrystallization increase or decrease the melting point range of the product you purified in class? Why? (5 points)
Question 2,3,4 please. ESTIONS: 1. Many students do not recover 100% of the original mixture. Describe...
Question 2,3,4 please.
ESTIONS: 1. Many students do not recover 100% of the original mixture. Describe at least two possible problems that could cause less than 100% recovery of the mixture. 2. A student received a mixture that actually contained 50.0% salt and 50.0% sand. At the end of the experiment, this student calculated that his sample was composed of 45.2% salt and 54.8% sand. What might he have done (or not done correctly) during the experiment to cause this...
Question 4 2 pts In lab, a student weighed out 1.576 g of unknown in a beaker. The student added ...
Question 4 2 pts In lab, a student weighed out 1.576 g of unknown in a beaker. The student added 58 mL DI water and followed the protocol in the lab to filter and dry the product, which had a final mass of 0.616 g. The filtrate was tested, and the student determined that CaCl2 2H2O was the limiting reactant. Determine the percent by mass composition of CaCl2 2H20 in the original unknown sample. Note: These numbers ate for calculation...
3
3. A student performs a crystallization on an impure sample of biphenyl. The sample weighs 0.5 g and contains about 5% impurity. Based on his knowledge of solubility, the student de- cides to use benzene as the solvent. After crystallization, the crystals are dried and the final weight is found to be 0.02 g. Assume that all steps in the crystallization are performed cor- rectly, there are no spills, and the student lost very little solid on any glassware...
What is the literature (known) melting point for acetanilide? A student performed a recrystallization to purify a crude sample from a reaction. The amount of crude material collected from the reaction was 13.56 grams. After the purification, the student collected 8.97 grams of extremely pure material. a. What is the percent recovery of the desired material? b. Is it possible to determine how much of the desired material remained in solution after the filtration? The solubility of acetanilide in hot...
Number of Unknown Sample Mass of Beaker #1 and Sample a-b=2,129 52.4779 - 50.348g 2.1299 -B0.35g 14.7009 DATA SUMMARY 4 52.4719 Mass of Beaker #1 50.341.4 Mass of Sample d Mass of Beaker 2 + NaCl (dried) 14. 1994 e Mass of Beaker #2 \r. 4019 f Mass of NaCl Recovered 2.4519 Mass of Filter Paper and Sio, (dried) 9 h Mass of Filter Paper 0.8129 Mass of Sio, Recovered J f + i=1.998g Total Mass of NaCl + SiO,...
solve
3 and 4
1989 Cengage Learning chlorine ions 5. A student was asked to determine the percentage of the components of a mixture of potassium bromide (KBr), magnesium hydroxide, Mg(OH)2, and barium sulfate (BaSOA). The mass of the sa- mple of the mixture used was 3.21 g. The student extracted the KBr from the mixture with water and filtered insoluble Mg(OH)2 and BaSO, from the solution, containing the KBr. After evaporating the filtrate, the student recovered and dried the...
please answer all
5. Suppose you started with 10 g of impure compound A which was 80% pure, and after recrystallization you recovered 5 g of pure A. Calculate percent recovery. (5 points) 6. Should recrystallization increase or decrease the melting point range of the product you purified in class? Why? (5 points)
Question 2,3,4 please.
ESTIONS: 1. Many students do not recover 100% of the original mixture. Describe at least two possible problems that could cause less than 100% recovery of the mixture. 2. A student received a mixture that actually contained 50.0% salt and 50.0% sand. At the end of the experiment, this student calculated that his sample was composed of 45.2% salt and 54.8% sand. What might he have done (or not done correctly) during the experiment to cause this...
Question 4 2 pts In lab, a student weighed out 1.576 g of unknown in a beaker. The student added 58 mL DI water and followed the protocol in the lab to filter and dry the product, which had a final mass of 0.616 g. The filtrate was tested, and the student determined that CaCl2 2H2O was the limiting reactant. Determine the percent by mass composition of CaCl2 2H20 in the original unknown sample. Note: These numbers ate for calculation...
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