Place 2.4 grams of sulfanilic monohydrate in a 125 ml Erlenmayer flask and dissolve it in 25 ml of 25% aqueous sodium carbonate by boiling. Cool the solution in the flask with running water before adding 0.95 gram of sodium nirite with stirring to dissolve the solid. Pour the solution into a 50 ml Erlenmayer flask containing 12.5 grams of ice and 2.5 ml of concentrated hydrochloric acid. Within a few minutes the white diazonium sulfonate inner salt should form a suspension. Transfer half of it to a 100 ml beaker, and keep both containers cold until each is used in later steps.  Identity test used is ________ Reagents used are ___________ MOA _____________ Product ____________ Visible result _________

A 2.00-g sample of a large biomolecule was dissolved in 15.0 g carbon tetrachloride.The boiling point of this solution was determined to be 77 .85°C. Calculate the molarmass of the biomolecule. For carbon tetrachloride, the boiling-point constant is 5.03°C∙ kg/mol, and the boiling point of pure carbon tetrachloride is 76.50°C.

Please show steps and answer accordingly. Thanks!

Which of the following is false about exothermic dissolutions? Select one: PLEASE EXPLAIN WHY IT IS TRUE AND WHY IT IS FALSE. Exothermic dissolutions will always result in an increase in the solution temperature Decreasing the temperature will increase solubility Exothermic dissolutions occur when solute-solvent interactions are weaker than solute-solute and solvent-solvent interactions Cooling a solution of Ca(OH)2will result in better dissolution

A solution is prepared by adding 425g of AgNO3 to 0.150L of water at 40.0∘C. The solubility of AgNO3 at 40.0∘C is 311g100.mL. How many grams of AgNO3 are expected to precipitate if the temperature is dropped to 0.00∘C where the solubility of AgNO3 is only 122g100.mL? Give the answer with three significant figures.

Suppose that you have a 1:1 mixture of compounds that is comprised of compound X and compound Y. You desire pure compound X and are planning a recrystallization to enhance the purity. Which solvent below is optimal for your recrystallization?      Ethanol (boiling point = 78 °C)   Solubility At   0  °C 100  °C Compound X 0.05 g/mL 0.20 g/mL Compound Y 0.02 g/mL 0.40 g/mL           Water (boiling point = 100 °C)   Solubility At   0  °C 100  °C Compound X 0.02 g/mL 0.05 g/mL Compound Y 0.01 g/mL 0.10 g/mL           Methanol (boiling point = 65 °C)   Solubility At   0  °C 65  °C Compound X 0.04 g/mL 0.10 g/mL Compound Y 0.02 g/mL 0.30 g/mL         Acetone (boiling point = 56 °C)   Solubility At   0  °C 56  °C Compound X 0.10 g/mL 0.50 g/mL Compound Y 0.20 g/mL 0.50 g/mL         Ethyl Acetate (boiling point = 77 °C)   Solubility At   0  °C 77  °C Compound X 0.10 g/mL 0.60 g/mL Compound Y 0.30 g/mL 0.60…

Describe how to prepare 100.0 mL of 0.0600 mol/L copper(II) sulfate solution from a 0.304 mol/L stock solution of copper(1I) sulfate. Include the necessary calculations and references to the appropriate equipment.

Caffeine can be extracted from tea bags using liquid-liquid extraction. After extracting the tea in hot water, sodium carbonate can be added to form the starting aqueous solution. In a separatory funnel containing 20 mL of diethyl ether, the same volume of aqueous solution will be added. The same procedure will be done in another separatory funnel but this time the organic solvent is hexane. Both separatory funnels will be shaken to release the pressure, and let stand to promote layer separation. The organic layers now containing caffeine will be separated into separate beakers. The beakers were then dried using calcium chloride (CaCl2). The beakers containing both solvents will be dried to obtain the isolated caffeine. Why is it important to release the pressure by venting out the separatory funnel? How will this affect the extraction when bypassed?

An organic chemistry student isolates 738 mg of salicylic acid (SA) and decides to use methanol in an attempt to purify it by recrystallization. Use the following information to calculate the maximum amount (in mg) that can purified from the crude product. SA solubility in methanol: o°C = 41.3 g/100 mL 56 °C = 64.5 g/100 mL

3. You are asked to calculate the Kf for t-butyl alcohol (MW = 74.122 g/mol). You gather the following information in your experiment. You weigh out 2.124 g t-butyl alcohol and you determine the freezing point of the solvent t-butyl alcohol is 21.6 °C (freezing point pure t-butyl alcohol). You then add water to the test tube with the t-butyl alcohol and measure the freezing point to be 15.3 °C. What key piece of information are you missing to calculate the Kf?