Bronsted Lowry Acids and Conjugate Pairs

What might happen if you mixed a strong acid with an equally strong base?

• You would see an explosive chemical reaction.
• The acid would destroy the base.
• The base would destroy the acid.
• You'd wind up with a pH-neutral substance.

What is the conjugate acid in the following equation?

• PO₄^3- 
• HNO₃ 
• NO₃^- 
• HPO₄^2-
  

What is the conjugate base in the following reaction?

• HCO₃^- 
• HCl
•  H₂CO₃ 
• ^Cl-

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

• HSO₄^-
• H₂O
• H₃O⁺
• SO₄^2-

CO₃^2-(aq)+H₂O(l)      →              HCO₃^-(aq)+OH^-(aq)
Using the above reaction, which compound is the conjugate base?

• CO₃^2-
• H₂O
• HCO₃^-
• OH^-

What are the products to a neutralization reaction?

• H₂ + Ionic Salt
• H₂O + Ionic Salt
• H₃O⁺ + Ionic Salt
• OH^- + Ionic Salt

A compound that donates H⁺ ions is 

• A Bronsted-Lowry Acid
• An Arrhenius Acid
• A Bronsted-Lowry Base
• An Arrhenius Base

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

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

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

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

If a solution is basic which ion will be more present?

• H+
• K+
• OH-
• H-