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Q: Question 28
A:
Solubility
How to tell if 0.45% NaCl saline solution is a solvent or solute?
How to tell if 3.0% NaCl saline Solution is a solvent or solute?
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- The literature value of solubility of a substance "A" is 2.5 g/100mL. The value for a different substance "B" is 0.1*10-3 g/100mL. In the lab, you determine the solubilities of this two substances experimentally. Your results are 2.6 g/100mL for substance A and 0.2*10-2 g/100mL for substance B. What deviation between experimental result and literature value is larger by percentage? What result would you call closer to the literature value? Why?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…To accurately prepare a standard solution, the correct glassware must be used to perform the dilution. What glassware is required to prepare a standard solution from a solid? Choose the most correct answer. beaker, conical flask, Pasteur pipette (dropper) beaker, volumetric flask, conical flask beaker, volumetric flask, Pasteur pipette (dropper) Pipette, volumetric flask, Pasteur pipette (dropper) beaker, measuring cyclinder, Pasteur pipette (dropper)
- The image shows a small volume within a 1.0 L solution with a solute concentration of 1 M. The blue spheres represent the solute particles in the solution. Identify whether you would need to add more solute or more solvent to the solution to achieve each of the following solutions. Each image represents the same small volume within the solution. Add solute Add solvent A stv Aa MacBook Air1 What mass of solid radium sulfate (the most insoluble compound known) will remain when 10 L of a saturated solution is transferred to a new container and the water evaporated to complete dryness? Ksp for RaSO4 = 4.30 x 10–11. a. 0.0021 g b. 0.021 g c. 0.071 g d. 0.710 g e. 0.0070 g3. A student peeled the skins from grapes, exposing cells with membranes that are only permeable to water. 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 Solution Seawater Grape soda CaCl₂ Grape juice Concentration of Solution (weight/ volume) 3.5% 11% 18% 1.8% Percent Change in Mass 1.3% -11.4% -21.5% -0.5% Identify one solution that is hypertonic to the grape. Justify your choice.
- 7a) Calculate the number of grams of hydrogen peroxide contained in 25.0 mL of a 3.60 M solution. 7b) What mass of a 30% (w/w) hydrogen peroxide solution is required to provide the mass calculated in question 7a? A w/w solution means g solute/100 g solution. Hint: You need to use your previous answer to 3 sig figs to get this answer to 3 sig figs. Your answer should have 3 sig figs.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 MilliQData Table –– Heat of Dissolution Salt NH4Cl CaCl2 NaCl NaOH Volume of water 45.0 mL 45.0 mL 45.0 mL 45.0 mL Density of H2O 0.9989 g/mL 0.9989 g/mL 0.9989 g/mL 0.9989 g/mL Mass of H2O Mass of salt 5.005 g 5.037 g 5.024 g 5.078 g Molar mass of salt 53.49 g/mol 110.98 g/mol 58.44 g/mol 40.00 g/mol Moles of salt 0.009357 mol 0.04539 mol 0.08597 mol 0.1269 mol Mass of solution (m) 50.0 g 50.1 g 50.1 g 50.1 g Initial temperature (Tinitial) 23.9°C 22.2°C 23.7°C 22.8°C Final temperature (Tfinal) 16.5°C 36.5°C 21.5°C 40.5°C Temperature change (Tfinal−Tinitial) Heat of dissolution (Q) Heat of dissolution per mole (Qsoln) Fill out the missing rows of your data table. (for numbers 1-3, you can pick one column of solid and just show the calculation for that column) Determine the change in temperature of the…
- 1. Sodium citrate: 0.015 M. Calculate the mass of sodium citrate dihydrate, Na3C6H5O7(H2O)2, needed to prepare 50 mL of a 0.015 M sodium citrate solution. 2. Silver nitrate: 5.0 x 10-4 M. Calculate the volume of 0.20 M AgNO3 solution needed to prepare 50 mL of 5.0 x 10-4 M AgNO3 solution. 3. Hydrogen peroxide: 0.050 M. Calculate the volume of 1.4 M H2O2 solution needed to prepare 50 mL of 0.050 M H2O2 solution. 4. Sodium borohydride: 0.015 M. Calculate the volume of 0.15 M NaBH4 solution needed to prepare 25 mL of 0.015 M NaBH4 solution.Consider the solubilities of a particular solute at two different temperatures. Temperature (∘?) Solubility (?/100 ? ?2?) 20.0 48.3 30.0 87.6 Suppose a saturated solution of this solute was made using 84.0 g H2O84.0 g H2O at 20.0 °C. How much more solute can be added if the temperature is increased to 30.0 ∘C?Calculating the freezing point of an aqueous solution 3. What is the freezing point of an aqueous solution that contains 3 moles of the ionic solute Cack per once kilogram of water? €a* + 2CI Cacl2 4. What is the freezing point of an aqueous solution that contains 2.30 moles of rock salt (NaCI) per one kilogram of water? 5. What is the freezing point of an aqueous solution that contains 1.3 moles of MgC12 per 1 kg water?
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