B-L Acids and Base Concept Check

A compound that donates H⁺ ions is

• A Bronsted-Lowry Acid

• An Lewis Acid

• A Bronsted-Lowry Base

• An Lewis Base

A Bronsted Lowry base:

• donates H+ to another substance

• accepts H+ from another substance

• produces H+

• produces OH-

In this reaction...
CH₃NH₂ + H₂O --> CH₃NH₃⁺ + OH^-
CH₃NH₂ can be classified as which of the following? (HINT...follow the H⁺!!!)

• A Brønsted-Lowry base
• A Brønsted-Lowry acid
• A Lewis acid
• An Arrhenius acid

HSO₄^-(aq)+H₂O(l)      →       H₃O⁺(aq)+SO₄^2-(aq)
Identify the Acid in the above reaction.

• HSO₄^-
• H₂O
• H₃O⁺
• SO₄^2-

Which of the following is transferred between a conjugate acid-base pair?

• An Electron
• A OH^- ion
• A Proton
• A Neutron

A substance that remains when a base has accepted an H⁺ ion is

• An acid
• A Base
• A Conjugate Acid
• A Conjugate Base

The following statement is true for Bronsted Lowry Conjugate Acid Base pair EXCEPT

• Bronsted Lowry Acid is a proton donor
• Bronsted Lowry Acid is a electron pair acceptor
• Conjugate acid has 1 hydrogen atom more than base
• Conjugate base has 1 hydroxide more than base

Which of the following shows the correct conjugate acid base pair?

• HCI (acid) / H₃O⁺ (conjugate base)
• HCI (acid) / CI^- (conjugate base)
• HCI (base) / CI^- (conjugate acid)
• HCI (base) / H₃O⁺ (conjugate acid)

Which of the following shows the correct conjugate acid base pair?

• H₂O (base) / H₃O⁺ (conjugate acid)
• H₂O (acid) / CH₃COO^- (conjugate base)
• CH₃COOH (acid) / H₃O⁺ (conjugate base)
• CH₃COOH (base) / CH₃COO^- (conjugate acid)

H₂O is amphiprotic, can act as acid or base. Which of the following is TRUE ?

• H₂O is an acid because it is a proton donor
• H₂O is an base because it is a proton acceptor
• H₂O can gain or lose a proton, H⁺
• H₂O can easily form hydronium ion, H₃O⁺