Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838. Both functional groups of salicylic acid ionize in water, with Ka = 1.0x10 for the CO2H group and 4.2x10 13 for the OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L). (Please use standard notation and don't enter units for your answer.)

Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838. Both functional groups of salicylic acid ionize in water, with Ka = 1.0x10 for the CO2H group and 4.2x10 13 for the OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L). (Please use standard notation and don't enter units for your answer.)

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter12: Chirality

Section: Chapter Questions

Problem 10CTQ

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Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the barkof the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838.(a) Both functional groups of salicylic acid ionize in water, with Ka = 1.0 × 10−3 for the—CO2H group and 4.2 × 10−13 for the −OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L).(b) Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H. The −CO2H functional group is stillpresent, but its acidity is reduced, Ka = 3.0 × 10−4. What is the pH of a solution of aspirin with the same concentration as a saturated solution of salicylic acid (See Part a).(c) Under some…
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Organic Chemistry : Acid and Bases