Chem 106 Test 3

1. A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 50.0 mL of LiOH.

• 3.22

• 2.35

• 0.68

• 1.52

1. A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Ka of HF is 3.5 × 10-4.

• 9.62

• 7.00

• 8.14

• 3.46

1. A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HF is 3.5 × 10-4.

• 3.82

• 3.46

• 3.09

• 2.78

Tags

NGSS.HS-PS1-7

Strong acids do not make good buffered solutions because

• Strong acids dissociate completely and the equilibrium lies far to the right

• Strong acids dissociate completely and the equilibrium lies far to the left

• Strong acid react completely with any base and the equilibrium lies far to the right

• Strong acid react completely with any base and the equilibrium lies far to the left

1. Calculate the pH of a solution of 2.0 M HF when 1.5 M KF is added to it.  (Ka for HF = 7.2 x 10-4)

• 3.14

• 3.02

• 3.26

• 4.02

Bromthymol blue, an indicator with a Ka value of 1.0 x 10-7, is yellow in its HIn form and blue in its In- form.  Suppose we put a few drops of this indicator in a strongly acidic solution.  If the solution is then titrated with NaOH, at what pH will the indicator color change first be visible?

• 4

• 5

• 6

• 8

1. In the titration of 20.00 mL of 0.500 M CH3COOH with 0.500 M NaOH.  (Ka for acetic acid is 1.8 x 10-5).
   Calculate the pH at the point in the titration where 7.45 mL of 0.500 M NaOH has been added.

• 4.52

• 5.46

• 3.21

• 4.34

In the titration of 20.00 mL of 0.500 M CH3COOH with 0.500 M NaOH.  (Ka for acetic acid is 1.8 x 10-5).
Calculate the pH at the point in the titration where 20.00 mL of NaOH has been added.

• 10.72

• 8.95

• 9.07

• 11.05

What does it mean for a titration solution to be at equilibrium?

• The molarity of the acid and base are equal.

• The volumes of the acid and base are equal.

• The moles of the acid and base are equal.

• The Concentration of the acid and base are equal.

What is the pH of a Strong Acid Strong Base titration solution at equilibrium?