1. Because carbon tetrachloride (CC14) is not soluble in water, a test tube containing the two liquids willform two layers. Predict which layer is on top and justify your answer with a detailed explanation. Ifmolecular iodine (I2) is added to the test tube, predict which liquid layer will dissolve most of the iodineand justify your answer – by looking up and recording the densities of both liquids on the Internet orCRC Handbook (in the Lab)Label these two "layers"In the pictogram on the left.

The density of carbon tetrachloride (CCl4) and water (H2O) are 1.59 gm/ml and 0.997 gm/ml means…

Answered: 1. Because carbon tetrachloride (CC14)…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section13.1: Solubility And Intermolecular Forces

Problem 13.1PSP

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Sodium chloride (NaCl) was isolated from SiO2 and CaCO3 by dissolving it in distilled water. Unmentioned is that CaCO3 is slightly soluble in water (0.001 g/100 mL). Describe the effect this fact will have on each component of the mixture: will the “isolated“ mass of each be greater than, equal to, or less than that in the sample?
Saturated aqueous sodium chloride (d = 1.2 g/mL) is added to the followingmixtures in order to dry the organic layer. Which layer is likely to be on thebottom in each case?a. Sodium chloride layer or a layer containing a high-density organic compound dissolved in methylene chloride (d = 1.4 g/mL)b. Sodium chloride layer or a layer containing a low-density organic compound dissolved in methylene chloride (d = 1.1 g/mL)
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In class we are learning about solubility, electrolytes both strong and weak. I totally get it. I just want to review how the notation of polar covalent soluble nonelectrolytes work. For example, Glucose as a solid being dropped in a water solution. Even though it is not ionic, it is very soluble and does not break up, so is not a electrolyte. Like an Ionic soluble, it does get hydrated. Thus , by thjs logic should it be notated like this? Glucose (s) >>>>>>>> Glucose (aq) ??? Or is there some other notation for sugar solution?
You are given the suggestion that a 0.15 ppm quinine aqueous solution is a good concentration to shoot for in the experiments, but quinine fluoresces best when it is acidified to 0.10 M H2SO4. Describe how to make 100 mL of the recommended solution starting with quinine sulfate (actually, quinine hemisulfate salt monohydrate). Assume you also have 1.0 M sulfuric acid and de-ionized water. Describe the process of a substance undergoing fluorescence and compare to the process of phosphorescence.
50.0 mL of a 0.60 M solution of pyridine in ethanol is to be prepared by measuring out a known volume of pure liquid pyridine and diluting to 500 mL with ethanol. The molar mass of pyridine is 79.1 g/mol, and its density at room temperature is 0.982 g/mL. What volume of pyridine is required for this solution?
A solution of 655 mL of 0.852 M CO(NH2)2 is mixed with a solution of 432 mL of 0.487 M CO(NH2)2. It is then evaporated on a hotplate to a volume of 825 mL. What is the molarity of CO(NH2)2 in this final solution? [Be aware that evaporation only changes the amount of water, not the amount of CO(NH2)2, because the boiling point of CO(NH2)2 is nearly 200 °C, too high to evaporate out of the solution to a significant extent].
Four students are investigating how temperature affects solubility rates of different solutes in water. After preparing their own saturated solutions at 50 ⁰C, they allowed them to cool down to 25 ⁰C. Saturated Solutions in Water Student Solute Temperature ⁰C Quantity Dissolved (g/100 g H2O) Amber LiCl 25 82 50 97 James KCl 25 36 50 44 Rachel NaCl 25 35 50 37 Timothy C12H22O11 25 103 50 130 Analyzing the results of their investigation, how would you rank the students with the quantity of grams that came out of their solutions from GREATEST to LEAST? A James > Rachel > Timothy > Amber B Amber > James > Timothy > Rachel C Timothy > Amber > James > Rachel D Rachel > James > Amber > Timothy
It is important to always minimize the amount of solvent used, allowing for evaporation. If we add a relatively large excess, we expect our recrystallization to produce lower percent recoveries. A common mistake is to misplace the decimal, resulting in addition of 11x the solvent instead of the recommended 1.1x. If a substance dissolves in a solvent at 1g/468 mL at room temperature and at 1g/13 mL at the solvent's boiling point, what would be the maximum expected amount recovered if using 11x the minimum amount of solvent in recrystallizing 10 g of the substance? Report your answer in grams to one decimal place.It is important to always minimize the amount of solvent used, allowing for evaporation. If we add a relatively large excess, we expect our recrystallization to produce lower percent recoveries. A common mistake is to misplace the decimal, resulting in addition of 11x the solvent instead of the recommended 1.1x. If a substance dissolves in a solvent at 1g/468 mL at room…
At 0 oC, the solubility of sodium acetate in water is 36.1 g per 100 g of water and at 40 oC, the solubility is 66.4 g per 100 g of water. A 100 g sample of sodium acetate is dissolved in 250 g of water at 40 °C. The solution is cooled to 0 °C and a small amount of solid is observed. This solution is ________. - supersaturated - saturated - unsaturated - hydrated
This question is related to chemical potential in a solution and how it relates to physical properties. What is the relationship between the freezing point of a dilute solution vs. that of the pure liquid? Provide an explanation for this relationship based on thermodynamics. If the temperature is increased in a saturated solution of A in equilibrium with solid A, what will you observe? Give a thermodynamic explanation for this (based on chemical potential and mole fraction)

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