pH, pOH, [H3O+], [OH-], Kw

A sample of pure water is neutral because it contains

• some hydronium ions. 
• equal amounts of hydroxide and hydronium ions.
• some hydroxide ions.
• only H₂O molecules. 

If you add 0.001 moles of HCl to 1 liter of water, the pH of the solution will be

• 2.0 
• 5.0
• 3.0
• 1.0

How does the concentration of Sr(OH)_2 compare to the concentration of OH^-^ in the same solution?

• [Sr(OH)_2] = [OH^-]
• [Sr(OH)_2] < [OH^-]
• [Sr(OH)_2] > [OH^-]
• [Sr(OH)_2] ? [OH^-]

A solution has a
[OH-]=2.4x10^-4M.  
Does this correspond to a pOH greater than or less than 4?  Is the solution acidic or basic?

• pOH < 4; acidic
• pOH > 4; acidic
• pOH < 4; basic
• pOH > 4; acidic

The [H₃O⁺] of a solution is 5.0x10^-8. How would you determine the [OH^-]?

• Divide 1.0x10^-14 by 
  5.0x10^-8
• Multiply 1.0x10^-14 by 
  5.0x10^-8
• Add 5.0x10^-8 to
  1.0x10^-14
• Subtract 5.0x10^-8 from 
  1.0x10^-14

A solution in which the pH is 12.5 would be described as _______ and would have a pOH of ____.

• Basic; 1.5
• Basic; 12.5
• Acidic; 1.5
• Acidic; 12.5

A solution contains 0.00100M HCl. Determine the [OH⁻]. 

• 1.00x10^-3M [OH⁻]
• 1.00x10^-14M [OH⁻]
• 1.00x10^-7M [OH⁻]
• 1.00x10^-11M [OH⁻]

The pH of a solution is 4.0. What is the H₃O⁺ concentration in this solution?  Is this an acidic or a basic solution?

• 1.0x10^-4M; Acidic
• 1.0x10^-4M; Basic
• 1.0x10^-10M; Acidic
• 1.0x10^-10M; Basic

Calculate the [H⁺] in a solution which shows a pH of 11.70. 

• 11.7 M
• 2.0 × 10⁻¹² M
• 5.0 × 10⁻³ M
• 2.3 M

Identify [OH⁻] = 1.0 × 10⁻⁶M as being true of acidic or basic solutions at 25◦C and then determine the pH. 

• basic; pH = 6
• acidic; pH = 6
• basic; pH = 8
• acidic; pH = 8