CHEM1101 Study Guide - Midterm Guide: Equilibrium Constant, Without Loss Of Generality, Ph

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Brønsted–Lowry Acid and Base

A Brønsted–Lowry acidmust have at least one removable (acidic) proton (H+) to donate.

A Brønsted–Lowry base must have at least one nonbonding pair of electrons to accept a

proton (H+).

What Is Different about Water?

• Water a at as a Brøsted–Lowry base and accept a proton (H+) from an acid

• It a also doate a proto ad at as a aid

• This akes ater amphiprotic.

Conjugate Acids and Bases

• The ter ojugateeas joied together as a

pair.

• Reatios between acids and bases always yield

their conjugate bases and acids.

Relative Strengths of Acids and Bases

• Aids aoe the lie ith HO as a ase are strog aids; their ojugate ases do ot at

as bases in water.

• Bases elo the lie ith HO

as an acid are strong bases; their

conjugate acids do not act as

acids in water.

• The sustaes etee the

lines with H2O are conjugate

acid–base pairs in water.

The stronger the acid, the

weaker is its conjugate base.

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Document Summary

A br nsted lowry acidmust have at least one removable (acidic) proton (h+) to donate. A br nsted lowry base must have at least one nonbonding pair of electrons to accept a proton (h+). What is different about water: water (cid:272)a(cid:374) a(cid:272)t as a br (cid:374)sted lowry base and accept a proton (h+) from an acid, it (cid:272)a(cid:374) also do(cid:374)ate a proto(cid:374) a(cid:374)d a(cid:272)t as a(cid:374) a(cid:272)id, this (cid:373)akes (cid:449)ater amphiprotic. Conjugate acids and bases: the ter(cid:373) (cid:272)o(cid:374)jugate(cid:373)ea(cid:374)s (cid:862)joi(cid:374)ed together as a pair. (cid:863, rea(cid:272)tio(cid:374)s between acids and bases always yield their conjugate bases and acids. The stronger the acid, the weaker is its conjugate base. The (cid:449)ord a(cid:373)phiproti(cid:272) is used: i(cid:374) pure (cid:449)ater, a fe(cid:449) (cid:373)ole(cid:272)ules a(cid:272)t as (cid:271)ases and a few act as acids, this is referred to as autoio(cid:374)isatio(cid:374). The equilibrium expression for this process is: kw = [h3o+][oh ]

Related Questions

In the Brønsted–Lowry concept of acids and bases, acid–base reactions are viewed as proton transfer reactions. The stronger the acid, the weaker is its conjugate base. If we were to think of redox reactions in a similar way, what particle would be analogous to the proton? Would strong oxidizing agents be analogous to strong acids or strong bases?

ceriseyellowjacket694

For conjugate acid-base pairs, how are K_a and K_b related?

Consider the reaction of acetic acid in water.

where

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 K_a for a monoprotic strong acid is 1x10⁶, calculate K_b 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 acid 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.)

limeswan13

For conjugate acid-base 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 × 10⁻⁵

Which two bases are competing for the proton?
Which is the stronger base?
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 the 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.)

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CHEM1101 Study Guide - Midterm Guide: Equilibrium Constant, Without Loss Of Generality, Ph

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