Can you please answer Question 2 a,b please thanks (9)Potons transfer immediately between acids and bases to reach an equilibrium. In the followingacid base reactions, draw Lewis structures for the coniugate acid and conjugate base formed when thereactants (on the left) are mixed.(a) CH;C(=0)OH + NH3acetic acid(conj, acid(conj, base)Acid(b) HCt=0]OHformic acıd+ CH3CH NH2(conj, acid(conj. base)(c) CH:CH,CH2C(%30H + Na/OHbutano ic acid[Na"/CrT + Hż0 +3. By definition the pH of a dilute solution of a weak acid equals its pka only when the concentrations ofunionized acid (HA) equals the concentration of its ionized conjugate base (A]. At any given pH an acid will bemostly ionized or unionized depending on its pka. Given the following weak acids and their pKa's decidewhether the acid is mostly ionized or mostly unionized at the pH shown.la] CH.C=0]OH [pKa = 4.76] at pH = 5.76[b] HC(=0)OH[pKa 3.75]at pH 2.75[c] CH.CH,CH,NH, [pKa = 10.7] at pH =8.7fdj H,S[pKa 7.0]at pH = 2[e] CH,OH[pka = 15.5] at pH = 9.5

Answered: Image /qna-images/answer/0d907e02-742e-4625-a046-de31f4a55374.jpg

2. Protons transfer immediately between acids and bases to reach an equilibrium. In the following acid base reactions, draw Lewis structures for the conjugate acid and conjugate base formed when the reactants (on the left) are mixed. (a) CH;C(=0)OH + NH3 acetic acid (conj, acid (conj, base) Ac id (b) HC(=0)OH formic acud + CH3CH NH2 (conj, acid (conj. base)

2. Protons transfer immediately between acids and bases to reach an equilibrium. In the following acid base reactions, draw Lewis structures for the conjugate acid and conjugate base formed when the reactants (on the left) are mixed. (a) CH;C(=0)OH + NH3 acetic acid (conj, acid (conj, base) Ac id (b) HC(=0)OH formic acud + CH3CH NH2 (conj, acid (conj. base)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 8RQ: For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in...

See similar textbooks

Similar questions

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?
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
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.)
You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
Write two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.
The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()