Chemistry Ch. 15 Section 1 Practice pH pOH

What occurs during the self-ionization of water?

• the pH of the solutions increases, and the pOH decreases

• a hydroxide is transferred from one water to another forming an acid and a base

• a neutralization reaction occurs forming a salt and water

• a proton is transferred from one water to another forming a hydronium ion and a hydroxide ion

The Kw at room temperature (25 degrees C) is equal to 1.0 E-14.  It can also be defined as:

• the pH and pOH of a solution

• the product of the hydronium ion and the hydroxide ion concentrations

• -log [hydronium ion]

• antilog -pH

For a solution, pH + pOH =

• 7

• 1.0 E-14

• 14

• -log (1.0 E-14)

What is the OH^- concentration for a 1.0 E-2 M solution of NaOH?

• 1.0 E-12 M OH^-

• This cannot be determined from the information given.

• 2

• 1.0 E-2 M OH^-

What is the H₃O⁺ concentration for a 1.0 E-2 M solution of NaOH?

• 1.0 E-2 M H₃O⁺

• 1.0 E-12 M H₃O⁺

• 2

• antilog (1.0 E-2 M H₃O⁺)

A 1.0 E-4 M solution of HNO₃ has a hydronium ion concentration of:

• 1.0 E-14/1.0 E-4

• 1.0 E-10 M

• log (1.0 E-4 M)

• 1.0 E-4 M

What is the concentration of hydroxide ions in a 2.0 M HCl solution?

• 5.0 E-15 M OH^-

• 2.0 M OH^-

• 2.0/1.0 E-14 M OH^-

• antilog (-2.0)

If the pH of a solution is 4.0, what is the pOH?

• 4.0

• 1.0 E-4

• 10

• Cannot be determined from the information

If the pH is less than the pOH the solution is a(n)

• base

• acid

• neutral solution

• salt

If the hydronium ion H₃O⁺ concentration is equal to the hydroxide ion OH^- concentration, the solution is a(n)

• acid

• base

• salt

• neutral solution