Copy of Project 5 Rock Candy Report

5. Suppose you have a mixture of water and your 2-chloro-2-methylbutane product in a separatory funnel. Use densities to predict which phase will be the top layer in the funnel. a. 2-chloro-2-methylbutane (organic phase) b. water (aqueous phase) c. there would only be one phase since the substances are miscible

Calculations are based off of my data table.  I'm not sure how to answer the questions. 1.Based on the results of your experiment, do you have hard or soft water? Does this match the data for your area? Briefly explain your answer. 2.How much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations. 3.What percentage of the recommended daily dose of calcium (1,150 mg/day) does 1.0 L of your water provide? Show all calculations. 4. A complexometric titration can also be used to determine the amount of calcium in milk. The calcium concentration in milk is typically 1,200 mg/L. How would you alter the procedure used in this experiment to determine milk’s calcium content?

B assignment Booklet Unit A Review 6. A 400-g sample of water contains 4.50 x 10 g of arsenic. a. Calculate the concentration of arsenic in the water sample in parts per million. Show your work. b. Use the table on page 42 of the textbook to determine whether this sample of water is safe to drink.

Directions Through the given situations below, answer the following questions 1 A mixture of monosodium glutamate, white sugar, salt and benzoic acid is to be melted by a group of Grade 7 students to determine the behavior of the mother during melting Predict how the mixture will look like as it is being heated. Explain your answer SUBSTANCE Sali White sugar Monosodium glutamate Benzoic acid MELTING POINT 801 C 186 C 232 C 122 C 2. Theo wants to observe what will happen to substance X (melting point is at 78 C) after heating it on an evaporating dish. After heating for a few minutes, substance X starts

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out of Express your answer with three significant digits. Do not include units! g/mol A sample solution has a concentration of 12.4% by mass. What mass of solute (in g) is present in 50.0 g of this sample solution? Express your answer with three significant digits. Do not include units! g + Chemistry 20 Final Exam Equation Sheet (click to open) page 1 11

2. In case of an accident in the classroom, who should be notified immediately? 3. Why is it a safety procedure to tie back long hair in the laboratory? 4. Why should a student not eat or drink in the laboratory? 5. Why should any spills be reported and cleaned immediately? 6. Why should you wash your hands after every laboratory period? 7. Why is rough play in the laboratory dangerous? 8. When would the wearing of safety goggles be a proper procedure? 7

Mary are trying to increase the rate at which she can dissolve a large amount of sodium chloride into water to make a solution to use in lab. Which of the following would be the BEST method of doing this?     A heat the water and use small pieces of sodium chloride     B heat the water and use a large piece of sodium chloride     C stir and heat the mixture and use small pieces of sodium chloride     D stir and heat the mixture and use a large piece of sodium chloride

A student peeled the skins from grapes, exposing cells with membranes that are only permeable to water and small diffusible solutes. The student measured the mass of the peeled grapes. The student then placed each peeled grape into one of five solutions. After 24 hours, the student removed the peeled grapes from the solutions, measured their final mass, and calculated the percent change in mass (Table 1). TABLE 1. PERCENT CHANGE IN MASS OF PEELED GRAPES IN SOLUTIONS Concentration of Solution Solution Percent Change in Mass (weight/volume) Distilled water 0% 13.48% Naci 20% -23.39% Tap water 0.8% 9.46% Grape juice 2.1% 2.8% Grape soda 13% -15.00% In a second experiment (Table 2), the student placed a peeled grape into a solution containing both small diffusible solutes and solutes to which the membrane is impermeable (nondiffusible solutes).

12. The unknown liquids you will use in this experiment are the three compounds below. Draw Lewis structures of each of these compounds. (A Google search for these structures might be helpful.) Isopropyl alcohol Water Hexane

Professor X mixed two solutions in a test tube and observed that the mixture was warm. He also tried to mix 50-ml each of the solutions in a 100-ml volumetric flask and found out that the total volume was less than 100 ml. He only has water, methanol, ethanol, and acetone in his table. From the following choices, what solutions did Professor X mix?   a.acetone and water b.water and methanol c.acetone and ethanol d.methanol and ethanol

Which of these will NOT dissolve in water?    a.table salt b.sugar c.vinegar d.bacon fat

Subparts 4-6

Can you help me understand how to get the dilution factors for each tube, please?

Pre-lab question #4: Distinguish between volatile and nonvolatile substance. The word "volatile" refers to a substance that vaporizes readily. Volatility is a measure of how readily a substance vaporizes or transitions from a liquid phase to a gas phase. A A (volatile/nonvolatile) substance refers to a substance that does not readily evaporate into a gas under existing conditions. A AA (volatile/nonvolatile) substance is one that evaporates or sublimates at room temperature or below.

Posttest Direction. Read the questions carefully. Write the letter of the correct answer. 1. Water exists in three states of matter and continuously moving through a cycle on Earth. At which stage in the water cycle does water transform from a gas to a liquid? a.evaporation c. precipitation b. condensation d. Sublimation 2. Carbon dioxide (CO2) forms when coal burns in the presence of oxygen. Which of the following is the BEST evidence that a chemical reaction occurs when the coal burns? a. Production of mechanical energy c. A new substance is produced b. Production of electricity d. Formation of precipitate 3.Which of these does NOT happen during a chemical change? a. New substances are formed with different chemical properties. b. Attractive force between atoms of molecule formed or break. c. The chemical properties of the substances before and after the reaction are the same d. Energy is always released or absorbed. 4. A granular substance is added to a liquid. Which of the…

Please answer question and give a brief explination why

STANDARD SAMPLE PREPARATIONS FOR ABSORBANCE & CONCENTRATION DATA Concentration of stock nickel sulfate hexahydrate solution = .400 Molarity Sample Volume Absorbance Concentration (In Molarity) a 5 mL .179 10 mL .329 15 mL .588 20 mL .760 25 mL .939 Reference Blank = 0 Please show how to find Molarity, please show steps. Thank you and stay safe.

4. Which mixture(s) can be separated into its components using filtration? A. oil + vinegar B. sand + iron filings C. pure water D. salt + sugar E. sand + water Examine the solubility chart below and answer questions 5-12 KNO le ww

An injectable preparation comes packaged as a 4 g vial and states that you should add 35 mL to achieve a final concentration of 200 mg/2 mL. How much diluent should you add to achieve a final concentration of 125 mg/2 mL? O a. 52 mL O b.59 mL O c. 55 mL O d. 48 mL

1. You have a concentrated stock solution of bacterial LPS in water that has a concentration of 1 mg/ml. What is the concentration of a diluted solution with a dilution factor of 1:2? 2. Your stock solution is 1 mg/ml and your final solution is 1ug/ml. What is your dilution factor? 3. A 1 ug/ml solution is diluted so it is half as concentrated as the stock. What is the concentration of the new solution in ng/ml?

4. Calcium Hydroxide Solution (Lime Water) and olive oil are used because an emulsifying agent is formed in situ when these 2 solutions are agitated together. What is the emulsifying agent that is formed? a. calcium succinate b. calcium oleate c. succinic hydroxide d. palmitic hydroxide

NEED A HELP WITH THIS QUESTION 02

What is the answer of this?

I have 6 tubes with the contents labeled. How can I make a 20% concentration serial dilution? Please show the steps and the final dilutions for the tubes as a fraction.

TRUE OR FALSE __________ 6. Glassware is clean when no water droplets cling to the inner wall of the vessel. __________ 7. When smelling the odor of a chemical substance, fan your hand over the substance toward your nose which should be centimeters away from the substance. __________ 8. An accident as simple as breaking a beaker containing distilled water in the sink does not need to be reported to the laboratory instructor. __________ 9. Students should turn off cell phones, iPads, and other electronic devices during the laboratory class. __________ 10. It is a good laboratory protocol to call other students’ attention when they do not practice good laboratory safety procedures.

10. Draw a graph of the concentration of NaCl (x-axis) against the calculated density (y-axis) for the data in section B above. Find the straight line equation. The graph has to be manual on graph paper, and you should draw a best-fit straight line. 11. Calculate the density of 35% NaCl from your graph.

What volume (in mL) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 solution? McVc=MdVd A.10.9 mL B.91.8 mL C.14.4 mL D.72.3 mL E.69.4 mL

These questions are not graded! It is strictly for practice. Do questions 1-5.

Most of us have had a glass of water from a Brita® pitcher. What is inside of a Brita® filter cartridge and what does it filter out? What doesn’t it filter out?

Sam drops a sugar cube into a jar with hot water and a sugar cube into a jar with cold water. Both jars have the same volume of water. He drops the sugar cubes at the same time and then observes how much of them dissolves in two minutes. What will be the result of Sam’s experiment, and which statement should he use as his conclusion? A A greater amount of sugar dissolved in hot water because temperature is directly proportional to the solubility rate of sugar in water.   B Temperature does not affect the solubility rate of the sugar cube in water because sugar dissolves equally in both cold and hot water.   C A greater amount of sugar dissolved in hot water because temperature is inversely proportional to the solubility rate of sugar in water.   D A smaller amount of sugar dissolved in cold water because temperature is inversely proportional to the solubility rate of sugar in water.