Ch. 14 Pre-Quiz

Acids by definition: 

• donate H⁺ 
• accept H⁺
• donate OH^- 
• accept OH^- 

Bases by definition have a pH of: 

• 7
• 0-6
• 8-14
• 0-14

What is the difference between an acid and it's conjugate base? 

• It has lost an H+ ion 
• It has lost an OH^- ion 
• It has gained an H⁺ ion 
• It has gained an OH^- ion 

Reaction of water with H⁺ produces: 

• hydronium ion (H₃O⁺) 
• hydroxide ion (OH^-) 
• H⁺ ion 
• Cl^- ion

HBr + NH₃ → NH₄⁺ + Br⁻
What is the base in the above reaction? 

• NH₃
• NH₄⁺
• Br^-
• HBr

HBr + NH₃ → NH₄⁺ + Br⁻
What is the conjugate base in the above reaction? 

• HBr 
• NH₃
• NH₄⁺
• Br⁻

HBr + NH₃ → NH₄⁺ + Br⁻
What is the conjugate acidin the above reaction? 

• HBr
• NH₃
• NH₄⁺
• Br⁻

Strong acids by definition: 

• have large K values
• have small K values 
• do not dissociate completely in water 
• dissociate slightly in water

At 60°C, the value of K_w is 1 × 10⁻¹³.
Calculate [H+] in a neutral solution at 60°C.

• 5.0x10^-14
• 1 × 10⁻¹³
• 3.2x10^-7
• 1.5x10^-3

At 60°C, the value of Kw is                    1 × 10⁻¹³.
 Using Le Chatelier’s principle, predict whether the reaction below is exothermic or endothermic.
2H₂O(l) → H₃O⁺(aq) + OH⁻(aq)

• endothermic
• exothermic
• endergonic
• none of these