M2L2 ; D,Ingram ; Lab Report Qualitative Synthesis of Aspirin

Natural goldenrod pigment is a yellow dye that changes to a bright red color in the presence of a basic solution and remains yellow in contact with an acidic or neutral solution. Peter is using goldenrod paper to test three solutions he prepared      Because Peter wants his message to be clearly visible in a red background at the end of his investigation, in what sequence should he use the solutions to paint the paper? A Paint first with lemon juice and then with tap water.   B Paint first with laundry detergent and then with tap water.   C Paint first with laundry detergent and then with lemon juice.   D Paint first with lemon juice and then with laundry detergent.

Question: Comment on the solubility of the two dyes in water. In your answer consider intermolecular bonds and their relative strengths. Solubility of dye C: Solubility of dye D:

What is the precipitant resulting from the following lab procedure? Lab: Extraction of a Three Component MixtureIntroduction:Understanding how a molecule will react based on its properties is the core of organic chemistry.One of the easiest to understand “structure-activity” relations is acid/base chemistry. In addition, thechemistry and thinking process in acid/base chemistry can be extended to be the basis for many of thereactions that you will learn about in this class. This lab will take advantage of acid/base propertiesin order to separate compounds using liquid/liquid extraction techniques. The following compoundsare present in the sample that you will be given and need to be separated into their pure components.Benzoic Acid Ethyl-4-aminobenzoate 9-FluorenoneProcedure:In the main hood you will find the powdered mixture of the three compounds, BenzoicAcid, Ethyl-4-Amino Benzoate, and 9-Fluorenone. Add this mixture to a clean separatory(sep) funnel (be sure the stopcock and closed…

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Nitric acid readily dissolves UO₂. Why doesn't hydrochloric acid dissolve UO2?    Please provide only typed answer solution no handwritten solution needed allowed

Part C – Acid–base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO3 to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system.

Question 9: 30.0 mL of a 0.20 M solution of the weak base methylamine is titrated with 0.10 M nitric acid (HNO3). The Kb of methylamine can be found in Appendix I. Calculate the pH at each volume of base addition as listed below and report your answer to two decimal places The initial pH (after 0.0 mL of nitric acid addition) is The pH after 10.0 mL of nitric acid addition is The pH after 30.0 mL of nitric acid addition is The pH after 60.0 mL of nitric acid addition is The pH after 65.0 mL of nitric acid addition is 100

Complete the lCF table. OH- +HA forms A-+ H20 MOL OH- MOL OF MOL OF FROM NAOH ACETATE ACETIC ACID INITIAL 0.005 0.5 0.5 CHANGE FINAL

When we dissolve aspirin in vinegar to extract pure aspirin, what is vinegars role on the chemical reactions taking place? What chemical reactions take place and what reaction equations explain the role of the vinegar on the component of the formulation of the aspirin or aspirin salt?

If salicylic acid dissociated into two particles when dissolved into myristic acid (it does not), would this change your calculated Kf value? Explain why. (Hint: look over your notes on the van’t Hoff factor, from lecture, for help.)

Watch the ChemTour animation below on buffers before answering the following question. BUFFERS Introduction A pH buffer is a solution that can minimize changes in pH when small amounts of acid or base are added to it. Control of pH is very important for chemical reactions in living systems. Our blood pH is about 7.4, and changes of a few tenths of a pH unit either way can cause serious health consequences. The blood has a buffer system to help regulate pH. Death Acidosis Alkalosis Death 6.6 6.8 7.0 7.2 7.4 7.6 7.8 8.0 Section 1 of 14 1st attempt See Periodic Table A 1.00 L solution contains 21.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.76? K, (HNO2) = 4.0 × 10-4. X 143.5 Normal 国

Watch the ChemTour animation below on buffers before answering the following question. BUFFERS Introduction A pH buffer is a solution that can minimize changes in pH when small amounts of acid or base are added to it. Control of pH is very important for chemical reactions in living systems. Our blood pH is about 7.4, and changes of a few tenths of a pH unit either way can cause serious health consequences. The blood has a buffer system to help regulate pH. Death Acidosis Alkalosis Death 6.6 6.8 7.0 7.2 7.4 7.6 7.8 8.0 Section 1 of 14 2nd attempt Feedback See Periodic Table See Hint A 1.00 L solution contains 14.52 g of nitrous acid, HNO,. What mass of sodium nitrite, NaNO,, should be added to it to make a buffer with a pH of 3.26? K, (HNO2) = 4.0 × 10-4. * 8.79 Normal

1. Calculate the theoretical molarity of 100ml of a 0.10 M NaOH solution. 2. Calculate the actual molarity of the NaOH solution that you prepared. 3. Calculate the percent error between the two NaOH values above.

If you react benzoic acid with a base, the resulting ion will be soluble in water. If you add HCl to this solution, the solution immediately turns cloudy. What is the reason for this observation? The HCl returns the proton to the ion. The resulting benzoic acid compound is not soluble in water. HCl is a cloudy solution The ion of benzoic acid is not soluble due to the nonpolar portion of the molecule. Because HCl is an acid and donates protons, reaction with HCl can make the solution cloudy.

Choose the letter that ranks the numbers from Least Soluble to Most Soluble when mixed with H,0 1) a. Least→2), 4), 3), 1) → Most b. Least→2), 3), 1) , 4) → Most c. Least→1), 4), 2), 3) → Most d. Least→1), 3), 4), 2) → Most e. Least>1), 2), 4), 3) → Most Br k + 4) HO, 2) 3)