2. Which of the following mixtures (check the box) would result in a buffered solution when 1.0 L of each of the two solutions are mixed? If the resulting solution is a buffer, determine the pH. O 0.20 M HNO3 and 0.40 M NaNO2 O 0.30 M HNO3 and 0.30M NaNO2 O 0.20 M HNO2 and 0.40 M HNO3 0.20 M HNO2 and 0.10 M NaOH

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Chapter1: Chemical Foundations
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2. Which of the following mixtures (check the box) would result in a buffered solution when 1.0
L of each of the two solutions are mixed? If the resulting solution is a buffer, determine the
pH.
O 0.20 M HNO3 and 0.40 M NANO2
O 0.30 M HNO3 and 0.30 M NaNO2
O 0.20 M HNO2 and 0.40 M HNO3
O 0.20 M HNO2 and 0.10 M NaOH
Transcribed Image Text:2. Which of the following mixtures (check the box) would result in a buffered solution when 1.0 L of each of the two solutions are mixed? If the resulting solution is a buffer, determine the pH. O 0.20 M HNO3 and 0.40 M NANO2 O 0.30 M HNO3 and 0.30 M NaNO2 O 0.20 M HNO2 and 0.40 M HNO3 O 0.20 M HNO2 and 0.10 M NaOH
1. 0.20 mol of KOH is added to 1.00 L of a solution that contains 0.50 M HC3H5O2 (Ka = 1.3 x
10-5) and 1.00 M NAC3H5O2.
|3|
a. Write the balanced net ionic equation for the reaction that occurs.
b. Determine the pH of the solution after the reaction. Assume the addition of KOH did
not change the volume.
Transcribed Image Text:1. 0.20 mol of KOH is added to 1.00 L of a solution that contains 0.50 M HC3H5O2 (Ka = 1.3 x 10-5) and 1.00 M NAC3H5O2. |3| a. Write the balanced net ionic equation for the reaction that occurs. b. Determine the pH of the solution after the reaction. Assume the addition of KOH did not change the volume.
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