beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in water. Label conjugate base and weak acid in this reaction. Saliva has a pH of 6.8, Calculate the percentage of arecoline in the HA form in typical saliva. Betel nut is usually chewed with a small amount of slaked lime Ca(OH)2. Explain why slaked lime improves the bioavailability and thus the effects of arecoline.

beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in water. Label conjugate base and weak acid in this reaction. Saliva has a pH of 6.8, Calculate the percentage of arecoline in the HA form in typical saliva. Betel nut is usually chewed with a small amount of slaked lime Ca(OH)2. Explain why slaked lime improves the bioavailability and thus the effects of arecoline.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 38QRT

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Chemistry beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in water. Label conjugate base and weak acid in this reaction. Saliva has a pH of 6.8, Calculate the percentage of arecoline in the HA form in typical saliva. Betel nut is usually chewed with a small amount of slaked lime Ca(OH)2. Explain why slaked lime improves the bioavailability and thus the effects of arecoline.
Methylamine, CH3NH2, has a Kb of 4.4 x 10-4. What is the pH of a 0.54 M solution of methylamine? Your answer should be to two places past the decimal. Calculate the pH of a 0.21 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).
Trichloroacetic acid (CCl3COOH) is a corrosive acid that is used to precipitate proteins. The pH of a 0.050 M solution of trichloroacetic acid is the same as the pH of a 0.040 M HClO4 solution. Calculate Ka and pKa for trichloroacetic acid.
3) Calculate the pH of a 27 mg/L solution of hydrocyanic acid (HCN). The pKa of hydrocyanic acid is 9.3.
Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin ( 5.7×102mg ) is dissolved in 0.33 L of water. Express your answer to one decimal place.Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin ( 5.7×102mg ) is dissolved in 0.33 L of water. Express your answer to one decimal place.
Calculate the pH of a 0.24 M solution of sodium lactate. The pKa of lactic acid is 3.86.
Calculate the pH of a 0.12 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).
Consider the following data on some weak acids and weak bases: acid base Ba K, name formula name formula hydrocyanic acid HCN 10 4.9 x 10 methylamine| CH3NH2 |4.4 × 10 HCH,CO2 1.8 × 10 ethylamine C2H5NH2|6.4 × 10 acetic acid Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaCN choose one 0.1 M KBr choose one 0.1 М КСН3СО2 choose one 0.1 М CН3NHзBr choose one
A weak acid, HA, has a pka = 6.78. If one dissolved 0.898 moles of a salt containing one mole equivalent of the conjugate base of the weak acid (e.g. NaA where A is the conjugate base of the weak acid) into 1 Liter of water, then what would be the resulting pH?
Calculate the pH at 25°C of a 0.59M solution of potassium cyanide KCN . Note that hydrocyanic acid HCN is a weak acid with a pKa of 9.21. Round your answer to 1 decimal place.
Give the definitions of pH and pKa. What are the differences between these two terms? Calculate the pH of salicylic acid solution when the solution is titrated to contain only 1.0% of salicylates. Use the fact, pKa (salicylic acid) = 2.97, in your calculation.
Consider the acid HXOy where X is a halogen that is less electronegative than oxygen. Which of the following gives the relationship between Ka of the acid and the value of y and gives the correct reasoning? As y increases the value of Ka increases because the conjugate base of the acid becomes less stable. As y increases the value of Ka increases because the conjugate base of the acid becomes more stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes less stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes more stable.