AP/IB Chapter 14 & 15

Calculate the pH of a 5.0M solution of KOH

• 14.00

• 2.0 x 10^-15

• 14.70

• -0.70

Nitrous Acid HNO_2, has a Ka=4.0x10^-4. The pH of a 0.25M HNO₂ solution is?

• 2.00

• 2.30

• 2.70

• 3.70

What is the pH of a 2.0M solution of HClO₄?

• 13.70

• 0.30

• -0.30

• 14.30

What is the pH of a 10.0M HNO₃ solution?

• 10.000

• 1.000

• 0.000

• -1.000

The pH of a solution is raised from 3.0 to 5.0. Which of the following statements describing this process is FALSE?

• the pOH will be lowered from 11.0 to 9.0

• The [H⁺] will be decreased by a factor of 20

• The final [OH^-] at pH=5 is 1.x10^-9

• The initial [H⁺] at pH=3 is 1.x10-3

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

• 2.3M

• 11.70M

• 5.0x10^-3M

• 2.0x10^-12M

At 0^oC, the K_w for water is 1.2x10^-15. The pH of water at this temperature is:

• 7.00

• 6.88

• 7.56

• 7.46

The pH of a 0.6M solution of a weak acid is 4.0. What percent of the acid is dissociated?

• .02%

• 2%

• 7%

• 4%

The [OH^-] in a 0.50M pyridine, C₅H₅N (K_b=1.7x10^-9) solution is?

• 0.50M

• 2.9x10^-5M

• 1.8x10^-9M

• 3.3x10^-10M

Calculate the pH of the following aqueous solution: 0.50M NaF (pKa of HF=3.14). Choose from the following pH ranges

• 0.00-2.99

• 3.00-5.99

• 6.00-8.99

• 9.00-10.99

• 11.00-14.00