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?
Addition of phenolphthalein to an unknown colorlesssolution does not cause a color change. The addition ofbromthymol blue to the same solution leads to a yellowcolor. (a) Is the solution acidic, neutral, or basic? (b) Whichof the following can you establish about the solution: (i) Aminimum pH, (ii) A maximum pH, or (iii) A specific rangeof pH values? (c) What other indicator or indicators wouldyou want to use to determine the pH of the solution moreprecisely?
For the chemical reaction below the Bronsted-Lowry acid
is:
NH3 + CH3COOH = NH4* + CH3 C00-
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_forward"Calcium ions/oxalic acid equilibrium in the kidney" Base on the above statement, give an equilibrium related to that and answer the following questions: What is the K value of the equilibrium if it is available. Base on Le Chatelier's principle, when will that equilibrium will not meet and what negative effects will happen when the equilibrium is not met. Suggest the preventive measures that can be taken to avoid negative effects whem the equilbrium is not met.arrow_forward
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- What makes an ideal buffer?arrow_forwardList 4 factors that can influence the acidity of a Bronsted-Lowry acid (and thus, the stability of its conjugate basearrow_forwardWhich three statements accurately describe the blood buffering system in humans? The blood buffering system utilizes the H, CO,/HCO, conjugate acid/base pair. The blood buffering system maintains the pH of blood near 7.4. The blood buffering system depends on the ionization of H, PO, The blood buffering system is facilitated by the enzyme carbonic anhydrase, which interconverts carbon dioxide and water to carbonic acid, ionizing into bicarbonate and H. The blood buffering system utilizes the acetic acid/acetate conjugate acid/base pair. O # e M へ吧急 11:28 AM 号 3/4/2021 DELLarrow_forward
- Acid Base Equilibria and Salt Equilibria 0.1 mole of ethanoic acid is dissolved in 1 liter of water at 25°C. Which of the following actions increases the dissociation constant, K, of ethanoic acid? O Increasing the temperature of ethanoic acid O Decreasing the temperature of ethanoic acid O Increasing the concentration of ethanoic acid O Diluting the acid with water 14 15 16 17 18 19 20 21 22 23arrow_forwardThe Ka of formic acid (HCO2H) is 1.8x10-4. What would the pH of a solution containing equal concentrations of formic acid and sodium formate be? Use the H-H equation for buffers to solve this. This is true in general for solutions where the acid and conjugate base are present in equal concentrations.arrow_forwardWhat is the [CH3COO−]/[CH3COOH] ratio inan acetate buffer at pH 5.00?arrow_forward
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