Organic Chemistry (9th Edition)
9th Edition
ISBN: 9780321971371
Author: Leroy G. Wade, Jan W. Simek
Publisher: PEARSON
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Chapter 15.14, Problem 15.23P
Phenolphthalein is an acid-base indicator that is colorless below pH 8 and red above pH 8. Explain briefly why the first structure is colorless and the second structure is colored.
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Phenolphthalein reacts to basic solutions (pH above 7) by changing to a pink color. If you had phenolphthalein in both an acidic (~6 pH) solution and an even more acidic solution (~5 pH), which solution would take more NaOH (a basic substance) to turn the solution pink?
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Chapter 15 Solutions
Organic Chemistry (9th Edition)
Ch. 15.2 - Prob. 15.1PCh. 15.2 - Prob. 15.2PCh. 15.2 - Prob. 15.3PCh. 15.4 - Prob. 15.4PCh. 15.4 - Prob. 15.5PCh. 15.5 - Treatment of an alkyl halide with AgNO3 in alcohol...Ch. 15.5 - Propose a mechanism for each reaction, showing...Ch. 15.6 - When Br2 is added to buta-1,3-diene at 15 C, the...Ch. 15.7 - Prob. 15.9PCh. 15.7 - When N-bromosuccinimide is added to hex-1-ene in...
Ch. 15.7 - Prob. 15.11PCh. 15.9 - Addition of 1-bromobut-2-ene to magnesium metal in...Ch. 15.10 - Show how you might synthesize the following...Ch. 15.11 - Predict the products of the following proposed...Ch. 15.11 - Prob. 15.15PCh. 15.11A - Prob. 15.16PCh. 15.11B - Prob. 15.17PCh. 15.11B - Predict the products of the following Diels-Alder...Ch. 15.12C - Prob. 15.19PCh. 15.12C - Prob. 15.20PCh. 15.13C - Prob. 15.21PCh. 15.13D - Using the examples in Table15-2 to guide you,...Ch. 15.14 - Phenolphthalein is an acid-base indicator that is...Ch. 15 - Prob. 15.24SPCh. 15 - Prob. 15.25SPCh. 15 - Show how the reaction of an allylic halide with a...Ch. 15 - Prob. 15.27SPCh. 15 - A solution was prepared using 0.0010 g of an...Ch. 15 - Prob. 15.29SPCh. 15 - Prob. 15.30SPCh. 15 - Prob. 15.31SPCh. 15 - Prob. 15.32SPCh. 15 - Prob. 15.33SPCh. 15 - Give the structures of the products represented by...Ch. 15 - Furan and malemide undergo a Diels-Alder reaction...Ch. 15 - Prob. 15.36SPCh. 15 - Prob. 15.37SPCh. 15 - Prob. 15.38SPCh. 15 - Prob. 15.39SPCh. 15 - Determine whether each structure is likely to be...Ch. 15 - An important variation of the Diels-Alder reaction...
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- Compare the percent dissociation of the acid in Exercise 21a with the percent dissociation of the acid in Exercise 21d. Explain the large difference in percent dissociation of the acid.arrow_forwardMethyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?arrow_forwardmy question is the fifth onearrow_forward
- An analytical chemist is titrating 211.2 mL of a 0.5700M solution of aniline (C6H5NH₂) with a 0.7200M solution of HNO3. The pK, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 140.1 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 P X Sarrow_forwardPhenolphthalein is an acid–base indicator. In solutions of pH 6 8.5, it is colorless; in solutions of pH 7 8.5, it is deep red-purple. Account for thechange in color.arrow_forwardPhenol red is a common acid-base indicator. It has a pKa equal to 8.000. It's undissociated form is yellow and its anionic form is violet. What color would a solution containing phenol red solution if the pH is 7.50? yellow yellow-orange red-orange red-violet violetarrow_forward
- 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. To prepare the buffer, a total volume of 550 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.98 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 1 decimal place)arrow_forwardPhenol red is a common acid-base indicator. It has a pKa equal to 8.000. Its undissociated form is yellow and its anionic form is violet. What is the concentration ratio between the acidic form vs. the basic form, [H- PRED]/[PRed], of the pH = 7.50 solution? Hint: Determine the concentration ratio of methyl red and its conjugate.arrow_forward. Which of the following is NOT a buffer? Explain your choice.● CH3CH3NH2 – CH3CH3NH3Cl● NaHSO4 – H2SO4● C6H5OH – C6H5O-● HNO2 – KNO2arrow_forward
- Please fill in the blanks of the question in the image below using the keywords provided: 3 times 1/3 100 times 1/100 acid basic higher lowerarrow_forwardWhat is the [CH3COO−]/[CH3COOH] ratio inan acetate buffer at pH 5.00?arrow_forwardA solution which is yellow in the presence of alizarin yellow indicator and red in the presence of phenolphthalein, must have a pH which is in what range? Refer to precision of indicators in the picture what is the lowest possible ph and the highest possible ph ?arrow_forward
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