What will be the pH of a buffer solution containing an acid with a pKa of 2.2 with an acid concentration equivalent to that of its conjugate base? Round your answer to the nearest tenth. Provide your answer below: pH =

What will be the pH of a buffer solution containing an acid with a pKa of 2.2 with an acid concentration equivalent to that of its conjugate base? Round your answer to the nearest tenth. Provide your answer below: pH =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 37QAP

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Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Find the value of Kb for the conjugate base of the following organic acids. (a) picric acid used in the manufacture of explosives; Ka = 0.16 (b) trichloroacetic acid used in the treatment of warts; Ka = 0.20
Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Find the value of Kb for the conjugate base of the following organic acids. (a) picric acid used in the manufacture of explosives; K a =0.16 (b) trichloroacetic acid used in the treatment of warts; K a =0.20
Several acids and their respective equilibrium constants are: Which is the strongest acid? Which is the weakest acid? Which acid has the weakest conjugate base? Which acid has the strongest conjugate base?
The pKa of NH3 is estimated to be 35. Its conjugate base, the amide ion (NH2−), can be isolated as an alkali metal salt, such as sodium amide (NaNH2). Calculate the pH of a solution prepared by adding 0.100 mol of sodium amide to 1.00 L of water. Does the pH differ appreciably from the pH of a NaOH solution of the same concentration? Why or why not?
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?
Acetic acid (pK, = 4.76) was dissolved in an aqueous solution buffered to a pH of 5.76. Determine the ratio of the concentrations of acetate ion and acetic acid in this solution. Which species predominates under these conditions? O The acid predominates, because the ratio of [acetate ion]/[acetic acid] = 0.01. O Neither species predominates, because the ratio of [acetate ion]/[acetic acid] = 1. O The conjugate base predominates, because the ratio of [acetate ion]/[acetic acid] = 10. The conjugate base predominates, because the ratio of [acetate ion]/[acetic acid] = 100. %3D O The acid predominates, because the ratio of [acetate ion]/[acetic acid] = 0.1.
According to the table in the text, hydrogen fluoride (HF) has a pK, of 3.2. If a solution of HF is brought to a pH of 5.0, what will be true of the relative concentrations of HF and fluoride ion (F) in that solution? The fluoride ion concentration will be zero O Both fluoride ion and HF will be present, but the concentration of HF will be greater than that of fluoride ion The concentration of the fluoride ion will be greater than that of HF O The concentration of the fluoride ion will be the same as that of HF
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If enough of a monoprotic acid is dissolved in water to produce a 0.0124 M solution with a pH of 6.72, what is the equilibrium constant, p?a, for the acid? kindly consider the following when answering the question For weak acids that are so dilute or so weak that the pH of the solution lies between 6 and 7, the autoprotolysis of water must be taken into account when determining the p?a value. At equilibrium, there are four species in solution, the weak acid, HA, its conjugate, A−, H3O+, and OH−. Start by developing four equations that describe what is occurring in the solution at equilibrium.