AP Chem Unit 08 Day 02 Practice

At 25°C, the [H₃O⁺] of a solution is found to be 1.0x10^-4M. What is the [OH-] of the solution and would the solution be considered acidic, basic, or neutral?

• [OH-]=1.0x10^-4 M

  Basic

• [OH-]=1.0x10^-10 M

  Acidic

• [OH-]=1.0x10^-4 M

  Acidic

• [OH-]=1.0x10^-10 M

  Basic

Consider the K_a values for the following acids:

 

Acid                                       K_a

chlorous acid, HClO           1.1x10^-2

acetic acid, HC₂H₃O₂          1.8x10^-5

oxalic acid, HC₂HO₄          2.0x10^-3

malonic acid, HC₃H₃O₄      2.4x10^-2

 

Which has the strongest conjugate base?

• chlorous acid

  HClO

• acetic acid

  HC₂H₃O₂

• oxalic acid

  HC₂HO₄

• malonic acid HC₃H₃O₄

HF(aq) + H₂O(l) ⇄ H₃O⁺(aq) + F⁻(aq)

The equilibrium constant, K_a, for the reaction above is 7.2x10^-4.  Which answer shows the bases and their relative strengths?

• F⁻ > H₂O

• HF > H₃O⁺

• H₂O > F⁻

• H₃O⁺ > HF

Tags

NGSS.HS-PS1-2