Interpretation: The name and chemical structures of three
Concept Introduction: Functional groups are the groups of atoms or atoms which are bonded with parent carbon chain in the organic molecule and are responsible for the physical and chemical properties of the compound. In
Some of the functional groups can easily ionized in acidic medium and exist in both neutral and ionized form that depends on the pH of solution.
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Experimental Organic Chemistry: A Miniscale & Microscale Approach (Cengage Learning Laboratory Series for Organic Chemistry)
- Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C;H;N NH,+ CH;NH;* CH$NH;* CH;NH;* C;H;NH* 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 3. Compute the concentration of the weak base in Molarity. (Write your answer in 3 decimal places without the unit).arrow_forwardAfter separating the acidic and neutral compounds in a mixture, how does one recover the neutral compound from the organic solution that it is in? O 1) Treat with HCl until acidic to precipitate the neutral compound as a solid. Heat the solution on a hot plate to evaporate the organic solvent and recover O 2) the neutral compound as a solid. Wave a magic wand and speak the spell of recovery to get the neutral O 3) compound as a solid. You don't need to recover the neutral compound as a soild, toss out the O4) organic solution and clean up the lab.arrow_forward40)arrow_forward
- Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH3 CH;NH2 C2H§NH2 CgH;NH2 C3H;N NH,+ CH;NH3* CH;NH3* CH;NH;* C3H;NH+ 1.8 × 10-5 4.38 × 10–4 5.6 × 10-4 3.8 × 10-10 Ammonia Methylamine Ethylamine Aniline Pyridine 1.7 x 10-9 3. Compute the concentration of the weak base in Molarity. (Write your answer in 4 decimal places without the unit).arrow_forwardAn analytical chemist is titrating 59.0 mL of a 0.8100M solution of ethylamine (C₂H₂NH₂) with a 0.4700M solution of HNO3. The pK, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 74.6 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.arrow_forwardAn analytical chemist is titrating 179.5 mL of a 0.8700M solution of ethylamine (C,H,NH,) with a 0.07400M solution of HNO,. The p K, of ethylamine is 3" 9. 3.19. Calculate the pH of the base solution after the chemist has added 638.4 mL of the HNO, solution to it. 3 Note for advanced students: you may assume the final volume equals the initlal volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = ||| Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessit hp Ce escarrow_forward
- An analytical chemist is titrating 147.6 mL of a 0.4800M solution of ethylamine (C₂H5NH₂) with a 0.2200M solution of HNO3. The pK, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 202.2 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 Xarrow_forwardUsing the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula K Ammonia NH3 CH;NH2 C2H;NH2 CH;NH, CSH;N NH,+ CH;NH;* CH NH;+ CH;NH;+ C;H;NH 1.8 x 10-5 Methylamine Ethylamine Aniline 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 2. Compute for pKb. (round off final answer to 2 decimal places)arrow_forwardSelect the correct answers: “Ocean acidification is a process that occurs when atmospheric carbon dioxide dissolves in the ocean and is subsequently converted into (methane; carbonic acid; carbonate ions; sodium carbonite) . This then causes the pH of the ocean to (increase; decrease; fractionate; multiply) and become more acidic.”arrow_forward
- Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. 1. Compute the pOH of the buffer solution. (Write your answer in 2 decimal places).arrow_forwardt" under the one which would be soluble in water. Writeeast" under the one which would be least soluble in water. butanoic acid heptanoic acid formic acid Write "lowest" under the compound with the lowest boiling point. Write "highest" under the compound with the highest boiling point. butanoic acid cyclohexane pentanol Write "most" under the one which would be most acidic. Write "least" under the one which would be least acidic. phenol benzoic acid cyclohexanol Write "best" under the one which would be likely to smell best. Write "worst' under the one which would be likely to smell worst. butanoic acid 2-pentanone methyl butanoate Write in the products. a) (C,H),CULI CH b) HOCH,CH,OHarrow_forwardUsing the table of the weak base below, you have chosen Aniline as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.71 M in this salt. The desired pH of the buffer should be equal to 3.8. Compute the pOH of the buffer solution. (Write your answer in 1 decimal place).arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningEBK A SMALL SCALE APPROACH TO ORGANIC LChemistryISBN:9781305446021Author:LampmanPublisher:CENGAGE LEARNING - CONSIGNMENT