Arrhenius, Bronsted-Lowry & Lewis Acid-Base Definitions

The Acid-Base classification system that defined acids as those that release H⁺ and bases as release OH^- is known as ________.

• Bronsted-Lowry
• Arrhenius acid-base
• Lewis acid-base
• Monoprotic and Polyprotic Acids

The Acid-Base classification system that defined a __________ is any compound that can donate a proton (an H⁺ ion) to an appropriate acceptor. A _________ is a compound that can remove (or accept) a proton.

• Bronsted-Lowry
• Arrhenius acid-base
• Lewis acid-base
• Monoprotic and Polyprotic Acids

The Acid-Base classification system that defined _________ acid has only one acidic hydrogen that would be transferred to a strong base, whereas a _________ has two or more acidic hydrogens.

• Bronsted-Lowry
• Arrhenius acid-base
• Lewis acid-base
• Monoprotic and Polyprotic Acids

Many cleaning solutions are bases. Which of the following is a property of most bases?

• feels slippery
• white color
• can only be liquid
• tastes sour

Water is polar because...

• Hydrogen has a slight positive charge and oxygen has a slightly negative charge.
• The entire molecule has a positive charge.
• The entire molecule has a negative charge.
• Hydrogen has a slight negative charge and oxygen has a slightly positive charge.

What is the conjugate acid in the following equation?

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

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.

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

What are the products to a neutralization reaction?

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