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.

Constants | Periodic Table 2,2-Dimethylpropanoic (or pivalic) is a weak organic acid that has a pungent odour. It's ester with vinyl alcohol are used to ake polymers that are used as highly reflective lacquers. Part C In Part A, a 20.00 mL aliquot of a 0.185 mol L-1 2,2-dimethylpropanoic acid solution was titrated to its equivalence point with 18.7 mL of 0.198 mol L-1 NaOH solution. At the equivalence point, all of the weak acid, 2,2-dimethylpropanoic acid, is converted to its weak conjugate base, 2,2-dimethylpropanoate. What is the pH at this equivalence point? O 5.030 9.005 O 6.987 2-2-dimethylpropanoic acid O 4.995 O 8.970 The Ka of 2,2-dimethylpropanoic acid is 9.33x10-6.

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…

Please Provide detailed Correct solution.

13) Bromthymol blue (BTB) is a chemical indicator that is blue all alone. When combined with a basic solution, it turns green as a solution becomes more acidic it turns yellow in an acidic solution. Fill in what color you think bromthymol blue would be in each of the situations in the chart. If solution color is given, simply provide a logical, possible pH value based on the outcomes. Fill in the missing ions as well! Situation pH BTB color Ion present Water directly out of tap 7.2 pH after exhaled air is blown through a straw into water for 5 5.1 H+ min. 14 pH after a snail has lived in water for three days Very Yellow pH with 2mL of bleach added to the water Very Blue 5.0 pH with instant coffee added to the water pH after an aquatic plant is grown in water for three days in bright sunlight Light Blue OH- 14)Is BTB a chemical indicator? 15) What then does it "indicate"? 16) Based on the data above, why does drinking coffee cause stomach pain for some indivudals? 17) What effect does…

Please can you help me with these three. Thank you and have a nice weekend.

Hi,  When vinegar is added to a solution of sodium bicarboneate, the mixture immediately begis to bubble furiously.  As time passes, however, there is less and less bubbling. Explain why this happens. Thank you,

10:13 A) HNO₂ Which one of the following is a strong acid? B) HF C) HCIO4 Question 1 of 12 D) HC₂H3O2 Submit Tap here or pull up for additional resources

Assume that: • Acid 1 is a stronger acid that Acid 2. You prepare two separate solutions, using 1.0 mol of each acid and mixing it with 1.0 L of pure water. Determine which of the following statements is correct. Select all that apply. O Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE V a Acid 1 has a larger K value that Acid 2. b Acid 1 will generate a higher concentration of H,0* ions. The solution prepared using Acid 1 will have a lower pH. d. Acid 1 will generate a higher concentration of A- ions. e The concentration of unreacted "HA" at equilibrium for the Acid 1 solution will be lower. f The pK value for Acid 1 is lower than the pK value for Acid 2.

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

Table 12.3 (data)           Substance pH Substance pH Substance pH Lemon Juice   Household ammonia   Baking soda   Orange Juice   Detergent (Laundry)   Aspirin   Milk   Detergent (dishwashing)   Buffered aspirin   Salivia             Table 12.4 (report)       Substance pH Substances pH

11:16 PM Tue Oct 12 AA www-awn.aleks.com G periodic table - Goo... Favorites- YouTube... XA ALEKS- Caliyah Hel... G kno3 acid or base -... G linear programming... G write formulas for t... C Solve Objective Knowledge Check Question 8 Caliyah Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? ammonium nitrate potassium acetate O yes no potassium sulfide silver nitrate O yes no iron(II) chloride zinc acetate O yes O no I Don't Know Submit Ow Hill LLC All Rights Reserved. Terms of Use I Privacy Cente II

2) 1. Februurg 2, 2022 Lyonel Tanis CHM-0IL Section: C16130) Name: Date: Report Sheet: Characterization of a Weak Acid. UNKNOWN NUMBER A. Standardization of NaOH Solution TRIAL [HCI] Volume Moles Moles Volume [NAOH] HCI NaOH NaOH 24.65 25.75 0.1002 25.89 25.73 Average [NaOH]. B. Identification of the Unknown Acid 8. Determination of Molecular Weight TRIAL [NaOH] Volume Moles Moles Grams Molecula Unknown HOBN Unknown r Weight (g/mol) NaOH 0.2947 Lohe 24.07 1. 0.2943 2. 3 Average Molecular Weight (g/mol)

Keff is defined as: 1- Static acid solubility 2- Weak base ionization constant 3- Constant effective solvation product 4- All of the above

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?

STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION PRE-LABORATORY EXPERIMENT 10 QUESTIONS NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0,50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 18 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155

How do I solve this? I do know that it is linear.

In the titration of NaOH with vinegar, a student overshot the endpoint (i.e. added too much NaOH solution). How will this affect the calculate percent acetic acid in the vinegar? percent will be too high percent will be too low no effect on the percent

= O ACIDS AND BASES Identifying the major species in weak acid or weak base... esc The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. 0.7 mol of KOH is added to 1.0 L of a 0.7 M HCN solution. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCN is a weak acid. 0.13 mol of NaOH is added to 1.0 L of a solution that is 1.5M in both HCN and NaCN. Explanation @ Check 0 acids: 0 other: # bases: acids: 0 bases: 0 other: с $ % 5 09 SCO X G Search or type URL 00 6 0,0,... Ś & 7 ☆ * Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 8 Valentina... Health and sport... OG…

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.