How do you prepare 500 ml 5% (v/v) ethanol/water mixture? Select one: a. Adding 25 ml ethanol and 475 ml water to 500 ml volumetric flask b. Adding 25 gr ethanol to 500 ml volumetric flask and making up the mark with water O c. Adding 25 ml ethanol to 500 ml volumetric flask and making up the mark with water d. Adding 25 ml ethanol to 500 ml volumetric flask and adding 475 ml water

How do you prepare 500 ml 5% (v/v) ethanol/water mixture? Select one: a. Adding 25 ml ethanol and 475 ml water to 500 ml volumetric flask b. Adding 25 gr ethanol to 500 ml volumetric flask and making up the mark with water O c. Adding 25 ml ethanol to 500 ml volumetric flask and making up the mark with water d. Adding 25 ml ethanol to 500 ml volumetric flask and adding 475 ml water

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.107E

See similar textbooks

Similar questions

You need 300. mL of 0.500-M K2Cr2O7. Which method is best to prepare this solution? Explain your choice. (a) Dilute 250. mL of 0.600-M K2Cr2O7 to 300. mL. (b) Add 50.0 mL water to 250. mL of 0.250-M K2Cr2O7. (c) Dilute 125 mL of 1.00-M K2Cr2O7 to 300. mL. (d) Add 30.0 mL of 1.50-M K2Cr2O7 to 270. mL of water.
6-16 Answer true or false. (a) Solubility is a physical property like melting point and boiling point. (b) All solutions are transparent—that is, you can see through them. (c) Most solutions can be separated into their components by physical methods such as distillation and chromatography.
6-35 Describe how we would prepare the following solutions: (a) 280. mL of a 27% v/v solution of ethanol C2H6O, in water (b) 435 mL of a 1.8% v/v solution of ethyl acetate, C4H8O2 in water (c) 1.65 L of an 8.00% v/v solution of benzene C6H6, in chloroform, CHCI3
6-15 Answer true or false. (a) A solute is the substance dissolved in a solvent to form a solution. (b) A solvent is the medium in which a solute is dissolved to form a solution. (c) Some solutions can be separated into their components by filtration. (d) Acid rain is a solution.
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…
50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution. Information of stock solution - molar mass- 534.3g/mole 0.587g in MilliQ
4. A solution is created by dissolving 74g of NaNO3 into enough water to make 3.50L of solution. Calculate the m/v% concentration of NaNo3 in this solution. Use stoichiometry conversion factors and actually put divider lines in between the numbers. The answer should be 2.1% m/V. 5. A 2.00L bottle of mineral water has a concentration of %0.00162 KCl mass/volume. Calculate the mass inmilligrams (mg) of KCl present in the bottle. Use stoichiometry conversion factors and actually put divider lines in between the numbers. The answer should be 32.4mg Please answer 4 and 5.
Preparation of a standard solution of copper(II) sulfate pentahydrate 1. Weigh out accurately 9.99 g of copper(II) sulfate pentahydrate (CuSO4·5H2O) by taring using a clean and dry empty 250-ml beaker. 2. Add tap water to the beaker to reach the 50-mL mark on the side of the beaker. 3. Dissolve all the crystals of CuSO4·5H2O in the water using a clean glass rod for stirring. 4. Then using a glass funnel transfer all the blue solution to a 100-mL volumetric flask. Rinse the beaker with about 10 mL of water and transfer the solution to the volumetric flask. Repeat the rinsing of the beaker with another 10 mL of water and transfer the solution to the volumetric flask. This is called quantitative transfer of the solution. 5. Then add enough water to reach the calibration mark of the volumetric flask. (You will need to use a dropper to add the last few drops of water to ensure the meniscus is on the calibration mark). Close the volumetric flask with a stopper and mix the solution well (so…
Ben prepared a salicylic acid in pentanol solution by adding 4.77 g of salicylic acid to 91.88 mL of pentanol. Calculate the mole fraction of salicylic acid in this solution. MW of salicylic acid= 138.12 g/mol MW of pentanol= 88.15 g/mol Density of pentanol= 0.8144 g/mL
Part 1. One gram of caffeine dissolves in 55 ml of water; 7 ml of dichloromethane (DCM); 530 ml of diethyl ether; and 100 ml of benzene. Covert the solubility of caffeine in these four solvents into units of mg/ml. a) Solubility of caffeine in mg/ml in water: b) Solubility of caffeine in mg/ml in DCM: c) Solubility of caffeine in mg/ml in Diethyl Ether: d) Solubility of caffeine in mg/ml in Benzene: Which is the optimal solvent to extract caffeine from an aqueous solution? Why? Part 1 Continued: Use intermolecular force (IMF), provide a brief explanation on the solubility of caffeine in water, diethyl ether, observed above. (Hint: draw the skeletal structures for caffeine, DCM and diethyl ether)
Table 1: Temp vs. solubility data of ammonium chloride. Test tube g NH4Cl/10 mL H2O Crystallization temp. (ºC) 1 1.0 g/10 mL H2O 10 oC 2 1.8 g/10 mL H2O 20 oC 3 2.9 g/10 mL H2O 40 oC 4 3.8 g/10 mL H2O 65 oC 5 4.4 g/10 mL H2O 95 oC Use the table to plot a solubility curve for ammonium chloride on the graph provided below. For the best fit line, use a smooth curve. "Mass of Solute per 100 mL of H2O," should be written on the y-axis (use increments of 2g for every box). "Temperature (°C)" should be written on the x-axis (use increments of 10 °C for every 2 boxes).