A 0.11 M solution of weak acid, HA, has a pH of 5.08. a. Write the dissociation reaction of the acid in water. b. Write the acid dissociation constant expression. c. Given the table below, what is the most probable identity of the acid? Acid Ka Hypochlorous acid 3.0 x 10-8 Nitrous acid 7.1 x 10-4 Hydrogen cyanide 6.2 x 10-10 Propionic acid 1.3х 10-5

A 0.11 M solution of weak acid, HA, has a pH of 5.08. a. Write the dissociation reaction of the acid in water. b. Write the acid dissociation constant expression. c. Given the table below, what is the most probable identity of the acid? Acid Ka Hypochlorous acid 3.0 x 10-8 Nitrous acid 7.1 x 10-4 Hydrogen cyanide 6.2 x 10-10 Propionic acid 1.3х 10-5

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 29Q

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A 0.11 M solution of weak acid, HA, has a pH of 4.24. Write the dissociation reaction of the acid in water. Write the acid dissociation constant expression. Given the table below, what is the most probable identity of the acid? Acid Ka Hypochlorous acid 3.0 x 10⁻⁸ Nitrous acid 7.1 x 10⁻⁴ Hydrogen cyanide 6.2 x 10⁻10 Propionic acid 1.3 x 10⁻⁵
This compound is a weak organic base: C18H21O3N + H2O <-------> C18H21O3NH+ + OH- A 5.00 x 10-3 M solution has a pH of 9.57. a. Whats the Kb expression b. What are the equilibrium concentrations of the reactants and products? c. What is the value of Kb? d. What is the % ionization?
Lactase is an enzyme that breaks down the sugar lactose which is commonly found in dairy products. Some people develop lactose intolerance as they grow older and the amount of lactase enzyme in their gut diminishes. Since the enzyme is commonly found in the gut of humans it can withstand a pH that is very acidic, ranging from a pH of 2-7. A student decided to do an experiment to determine how the pH of a solution affects lactase enzyme activity. Lactase works by breaking lactose into its two component sugars of glucose and galactose. To conduct the experiment the student prepared a solution of lactose and placed it into 5 different test tubes. A pH buffer solution was then added to each test tube with a pH of 2.0 in the first tube, 4.0 in the second, 6.0 in the third, 8.0 in the fourth, and a 10 pH in the fifth. Next, the enzyme lactase was added in equal amounts to each test tube and allowed to sit for ten minutes white the enzyme reacted with the lactose. At the end of the ten…
Palmitic Acid, CH3(CH2)14COOH, found in both bacon fat and many soaps. Palmitic acid partially ionizes in water. Write a balanced chemical reaction for the dissociation of palmitic acid into its conjugate base and hydrogen ion. Write an expression for the equilibrium constant for palmitic acid. The equilibrium concentrations are [CH3(CH2)14COOH] = 0.1 M and [H+] = [CH3COO-] = 0.0133352 M. Calculate the equilibrium constant of ionization KA. Calculate the pKA of palmitic acid. Draw (by hand) the titration curve for palmitic acid. Please label your axes appropriately.
Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.
A 0.11 M solution of weak acid, HA, has a pH of 5.08.a. Write the dissociation reaction of the acid in water.b. Write the acid dissociation constant expression.c. Given the table below, what is the most probable identity of the acid?
A 10.0 mL sample of 0.20 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0700 mol/L NaOH(aq) and then diluted to a final volume of 100. mL. Calculate the concentration of OH- ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.
The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. B. The total acid concentration (nitric + nitrous acid) of the 10.0 mL solution of “acid rain” is determined by an acid-base titration method. You add 5.00 mL of the titrant sodium hydroxide with a concentration of 0.0114 M to reach the endpoint. i. What is the number of moles of hydroxide ions added? ii.Write one net ionic equation for the…
For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. A. One simple way to measure the [H+] is to measure pH. If a 10.0mL solution of “acid rain” is measured to have a pH=2.77, what is the concentration of strong acid, HNO3, formed? Hint: pH=-log[H+] and 10–pH= [H+], where [H+] is in molarity units.
The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
The labels on most pharmaceuticals state that the medicine should be stored in a cool, dark place. In the context of this chapter, explain why this is sound advice.