Table 1. Solubility Tests.Functional Group Observations(specify type ifany)Samplein concentrated (+/-)H2SO4Color orangeHydroxyl groupHydroxyl groupHydroxyl group1-butanolColor orange2-butanolColor orangediisopropyletherLook at the structures of compounds tested for solubility in concentrated H2SO4.What generalization can be made for a substance to be soluble in concentrated H2SO4 ?

Introduction: We have to tell the observations for the following reactions taking place.

Table 1. Solubility Tests. Functional Group Observations (specify type if any) Sample in concentrated H2SO4 Color orange (+/-) Hydroxyl group Hydroxyl group Hydroxyl group 1-butanol 2-butanol Color orange + Color orange diisopropyl ether Look at the structures of compounds tested for solubility in concentrated H2SO4. What generalization can be made for a substance to be soluble in concentrated H2SO4

Table 1. Solubility Tests. Functional Group Observations (specify type if any) Sample in concentrated H2SO4 Color orange (+/-) Hydroxyl group Hydroxyl group Hydroxyl group 1-butanol 2-butanol Color orange + Color orange diisopropyl ether Look at the structures of compounds tested for solubility in concentrated H2SO4. What generalization can be made for a substance to be soluble in concentrated H2SO4

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 91AE: The solubility of benzoic acid (HC7H5O2), is 0.34 g/100 mL in water at 25C and is 10.0 g/100 mL in...

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The solubility of benzoic acid (HC7H5O2), is 0.34 g/100 mL in water at 25C and is 10.0 g/100 mL in benzene (C6H6) at 25C. Rationalize this solubility behavior. (Hint: Benzoic acid forms a dimer in benzene.) Would benzoic acid be more or less soluble in a 0.1-M NaOH solution than it is in water? Explain.
Solubility data of a sample is given below: Solvent Solubility in Cold Solvent Solubility in Hot Solvent Toluene Insoluble Soluble Dichloromethane Insoluble Insoluble Methanol Soluble Soluble From the above list, which solvent is bes ited for recrystallization this sample? Select one: Toluene Dichloromethane Methanol O Cannot be determined.
45. Fig. 9 presents a plot of change in KNO3 solubility in water with increasing temperature. This plot shows the concentration of the saturated solution expressed in g of KNO3 per 100 g of H2O. Calculate the molarity of this solution at 30ºC knowing that the density at this temperature equals 1.25 g/cm³. 100 90 Fig. 9, Change in KNO3 solubility in water with increasing temperature A. 12.4 mol/dm³ B. 5.0 mol/dm³ C. 4.0 mol/dm³ D. 3.6 mol//dm³ E. 1.8 mol/dm³ solubility g of KNO3 in 100g of H₂O 80 70 60 50 40 30 20 10 0 0 10 20 30 30 40 50 60 70 temperature/°C
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…
Match each definition or prompt with the correct term on the right. The term used for a [Choose ] solution where water is the solvent. Water is considered this, due for its [Choose ] ✪ ubiquity in solutions. Water can conduct [Choose] ✪ an electric current with these dissolved in solution On it's own, pure water has a virtually [Choose ] ◆ no ability to do this to an electric current. In a saltwater solution, the salt is [Choose ] considered this. Glucose and other [Choose ] covalent compounds (except acids) are consider this when acting as solutes, and unable to carry current. î î
You are given an 18% solution of sodium imidazole. What mass of imidazole (in g) would be in 20 mL of this solution? a. You need to use the sodium imidazole stock solution from Q11 to make a dilute imidazole solution (final volume 180 mL) at a final concentration of 0.2 M. The molecular weight of imidazole is 90 g/mole. What volume of imidazole stock would you use (mL)? b. You need to use the sodium imidazole stock solution from Q11 to make a dilute imidazole solution (final volume 180 mL) at a final concentration of 0.2 M. The molecular weight of imidazole is 90 g/mole. What volume of water would you add (mL)?
2. You have a solution that contains 4.0g of oxalic acid dissolved in 100 mL of water. This solution is placed in a separatory funnel, and then 100 mL of diethyl ether is added to the separatory funnel and an extraction is performed. (Diethyl ether and water are immiscible solvents.) Use the following constants to calculate how much oxalic acid is in each solvent after the extraction. Solubility of oxalic acid in water = 9.5 g / 100 mL Solubility of oxalic acid in ether = 16.9 g/100 mL
Prepare the following solution quantitatively using boiled distilled water 1. 250.0 mL 1.0 M stock HCl solutionNOTE: Use the 3.0 M HCl solution from the pic Prepare the following solution quantitatively using boiled distilled water 1. 250.0 mL 0.0500 M standard HCl solution from 1.0 M HClpls compute how to prepare them
why is cyclohexene soluble in H2SO4? please cite reference
Why is salt not soluble in isopropyl alcohol?