### Hypothetical Solubility Data for Compound A#### Solubility Data Table| Solvent | Solubility in Boiling Solvent | Solubility in Cold Solvent ||-----------|-------------------------------|----------------------------|| Hexanes | 0.3 g/100 mL | 0.02 g/100 mL || Ethanol | 10 g/100 mL | 9 g/100 mL || Water | 4 g/100 mL | 0.2 g/100 mL || Methanol | 3 g/100 mL | 0.3 g/100 mL |#### Multiple Choice QuestionChoose the best solvent to purify 2 g of compound A by crystallization.- [ ] Methanol- [ ] Ethanol- [ ] Hexanes- [ ] Water#### Detailed Explanation of the Solubility Data TableThe table provided lists the solubility of compound A in various solvents at two different conditions: when the solvent is boiling and when it is cold.- **Hexanes**: Solubility is 0.3 grams per 100 mL in boiling hexanes and 0.02 grams per 100 mL in cold hexanes.- **Ethanol**: Solubility is 10 grams per 100 mL in boiling ethanol and 9 grams per 100 mL in cold ethanol.- **Water**: Solubility is 4 grams per 100 mL in boiling water and 0.2 grams per 100 mL in cold water.- **Methanol**: Solubility is 3 grams per 100 mL in boiling methanol and 0.3 grams per 100 mL in cold methanol.By comparing the solubility of compound A in different solvents under boiling and cold conditions, you can determine which solvent is most effective for purification by crystallization. Effective purification often relies on a significant difference in solubility between hot and cold solvents to allow for maximum recovery of the compound when cooled.Note: The best solvent for crystallization usually has a high solubility for the compound when hot and a significantly lower solubility when cold.

As solution has two main components, one is solute and other is solvent. That component which is…

Hypothetical solubility data for compound A. Solubility in Boiling Solvent 0.3 g/100 mL 10 g/100 mL 4 g/100 mL 3 g/100 mL Solubility in cold Solvent 0.02 g/100 mL 9 g/100 mL 0.2 g/100 mL 0.3 g/100 mL Solvent Hexanes Ethanol Water Methanol Chose the best solvent to purify 2 g of compound A by crystallization. Methanol Ethanol Hexanes Water

Hypothetical solubility data for compound A. Solubility in Boiling Solvent 0.3 g/100 mL 10 g/100 mL 4 g/100 mL 3 g/100 mL Solubility in cold Solvent 0.02 g/100 mL 9 g/100 mL 0.2 g/100 mL 0.3 g/100 mL Solvent Hexanes Ethanol Water Methanol Chose the best solvent to purify 2 g of compound A by crystallization. Methanol Ethanol Hexanes Water

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the Ke of cyclohexane using the freezing point of cyclohexane (6.50°C) and benzophenone (4°C). Given: Mass of benzophenone = 0.438g Molar mass of benzophenone = 182.217 g/mol Volume of cyclohexane = 25mL Density of cyclohexane = 0.779 g/mL %3D
Rank these substances in order of increasing solubility in water. Solubility Substances (4 items) (Drag and drop into the appropriate area) Most soluble CH3CH2CH2OH 1 CH3(CH2)5OH CH3(CH2)3OH 2 CH3CH2OH 3. 4 Least soluble
Need help ASAP!! thanks! The minimum volume of boiling water is used to dissolve 1.50 g acetanilide. The hot solution is cooled to room temperature and the acetanilide recrystallizes. What mass of acetanilide remains dissolved in water? (solubility of acetanile at 100o C is 5 g/100 mL and at room temperature is 0.54 g/100 mL). (Enter a number only with no g unit.)
Which of the following will have the greatest solubility in water? Which will have greatest solubility in ethyl acetate (an organic solvent)? HO зас Select one: NH₂ منشود III CH₂ a. I in water and IV in ethyl acetate H₂C H₂C HO HO HO OH HO II IV NH
Calculate the solubility of CdCO3 (Ksp = 5.1 x 10-12) in moles per liter. Ignore any acid–base properties. Calculate the solubility of Sr3(PO4)2 (Ksp = 1.5 x 10-31) in moles per liter. Ignore any acid–base properties.
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?
10. A volumetric flask contains 25.0 mL of a 14% m/V sugar solution. If 2.5 mL of this solution is added to 22.5 mL of distilled water, what is the % m/V of the new solution. O 1.4 % m/V 14 % m/V O 7.1 % m/V O 71 % m/V
15) Which one of the compounds below has the highest solubility in water, expressed in moles per liter? A) BaF2, Ksp = 1.7 x 10-6 B) Sr(103)2, Ksp = 3.3 × 10-7 C) SrF2, Ksp = 2.8 × 10-9 D) MgF2, Ksp = 6.5 × 10-9 E) PbCl2, Kp = 1.6 × 10-5 sp
escriptionSolubility (soluble, insoluble, miscible & immiscible)25 mL of water and 1 g of salt—the resulting mixture is clear and colorless 25 mL of water and 1 g of solid silver chloride—the resulting mixture is cloudy and solid settles out. 25 mL of water and 5 mL of mineral oil—the resulting mixture is cloudy and gradually separates into two layers.
1. A 1.2000 g sample of (NH4)2Ce(NO3)6 (548.23 g/mol) is dissolved in water and diluted to 100.0 mL. Calculate the molar analytical concentration of the (NH4)2Ce(NO3), solution Calculate the molarity of NO3 Calculate the pCe Calculate the ppm NH4+ (18.0385 g/mol) in the solution
The amino acids alanine (MW = 89.1 g/mol) and leucine (MW = 131.2 g/mol) have solubilities of water at room temperature that are reported to be 166 g/L and 24 g/L respectively. Calculate the molar solubilities of each of these compounds. Write the structure for each amino acid and explain the trend in molar solubility in terms of the structure of the two amino acids. Do you think that leucine would have the same or a different structure depending upon if it was dissolved in water or an organic solvent such as dichloromethane? Provide the structure(s) that you might expect along with a brief explanation.
Why do two layers form when solutions containing water are added to the extracted dichloromethane (CH2CI-2) solution?