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- - What is the ideal solvent behavior for crystallization? - You will probably hear me say frequently: “minimum amount of hot solvent” during this lab. Why isthat?according to wikipedia what is the solubility of benzoic acid in water at 25 degrees and 100 degrees? if you were given 1.55 grams of benzoic acid how much boiling water would you need to dissolve it all (show all work)? If you were to cool the solution to 25 degrees afterwards, would the solution be saturated? justifyYou've just synthesized a new molecule and need to purify it by recrystallization. You find that it is poorly soluble in water and highly soluble in ethanol, even when cooled in ice. What solvent should work in this situation? a. water b. Recrystallization from any solvent is impossible. c. methanol d. a solvent mixture - water and ethanol
- After a recrystallization, a pure substance will ideally appear as a network of Choose...smalllargeround Choose...clumpspowderscrystals . If this is not the case, it may be worthwhile to reheat the flask and allow the contents to cool more Choose...completelyquicklyslowly .In which option is the order showing whether the questions given below are true or false? ( ) Airborne humectants are generally called hygroscopic substances. ( ) Removing water from solids can be done by heating your sample in the oven just below its melting point. ( ) Drying capacity is a measure of the drying efficiency of the dryer. ( ) Drying intensity is the amount of water held by 100 grams of dryer. ( ) For the phenomenon called "blooming" to occur, the vapor pressure of the hydrate system must be higher than the partial pressure of water in the air. A. Right, Wrong, Right, Wrong, RightB.Right, Right, Wrong, Wrong, RightC.Right, Wrong, Wrong, Wrong, RightD. Right, Wrong, Wrong, Right, RightE.Right, Right, Wrong, Wrong, RightThe solvent for an organic reaction is prepared by mixing 70.0 mL of acetone (C3H6OC3H6O) with 56.0 mL of ethyl acetate (C4H8O2C4H8O2). This mixture is stored at 25.0 ∘C∘C. The vapor pressure and the densities for the two pure components at 25.0 ∘C∘C are given in the following table. What is the vapor pressure of the stored mixture? Compound Vapor pressure(mmHg) Density(g/mLg/mL) acetone 230.0 0.791 ethyl acetate 95.38 0.900
- 1. What is the mole percent of methanol in your starting solution (composed of 1.5 mL and 6 mL isopropanol)? 2. Using the vapor-liquid equilibrium data graph (NOTE: You have to make this graph using the data provided) and your answer from question 1, answer the following: If your first distillate was 49 mole percent methanol, how many theoretical plates were in your distillation setup? Data Mole % of Methanol Temperature (°C) Vapor Liquid 66.22 95.35 90.10 67.94 89.10 79.00 70.22 80.00 66.05 72.67 68.50 52.20 74.78 57.00 40.80 77.06 42.85 29.30 78.94 29.00 19.50 81.00 13.20 8.10What is the final equilibrium temperature after you mix 10 grams of ice at 0 degrees C with 50 grams of water at 90 degrees C? I have posted my proffesor's solution I understand it for the most part but I'm confused on why in her solution she does the mass of ice times the specific heat of WATER times change in temp. Why does she use the specific heat of water and not ice?? I understand the rest of the problem but that is tripping me upa. Colloidal particles typically have a negative surface charge that attracts oppositely charged positive ions in the surrounding bulk solution. These so-called _______-ions are held at the particle surface through electrostatic and van der Waals forces of attraction strongly enough to overcome thermal agitation. b. Turbine and propeller type mechanical mixers used for rapid mixing of reagent chemicals have either ------------- flow impellers with flat or curved blades located parallel to the axis of the drive shaft, or --------------------- flow impellers with blades making an angle of less than 90o with the drive shaf
- For the liquid acetone, list all IMFs that have to be broken in order for it to mix with waterA batch of 500 ?? of ??? dissolves in water to form a saturated solution at 350 ? (77 °?) where the solubility is 30% by weight of ??? in water. The solution cools at 293 ? (20 °?) at which the solubility is 25.4% by weight. Determine the number of crystals obtained if 3.5% of the original water evaporates on cooling. Also, determine the capacity of the container in which this solution is cooled if it is 1.20 times the volume of the solution. The density of the solution is ???? ??/??Define the relative amounts of liquid and vapor phases in a saturated mixtureare specified by the quality x.