Calculating pH of Solution with Acetic Acid and Sodium Acetate
Learn how to determine the pH of a solution containing 0.30 moles of acetic acid and 0.30 moles of sodium acetate in a 1.00-liter solution using the given Ka value. Understand the concept of weak and strong electrolytes in the ionization process.
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Presentation Transcript
Take out your 17.1 notes and work on the following: 1. What is the pH of a solution made by adding 0.30 moles of acetic acid and 0.30 moles of sodium acetate to enough water to make 1.00 liter of solution? Ka = 1.8 x 10-5
Whenever a weak electrolyte and a strong electrolyte with an ion in common are together, the weak electrolyte ionizes less than it would if it were alone. less
NaNO2to a solution of HNO2 (CH3NH3)Cl to a solution of CH3NH2 Sodium formate to a solution of formic acid Potassium bromide to a solution of hydrobromic acid NaCl to a solution of HC2H3O2
NaNO2to a solution of HNO2 Increase (CH3NH3)Cl to a solution of CH3NH2 Decrease Sodium formate to a solution of formic acid Increase Potassium bromide to a solution of hydrobromic acid Stay the same NaCl to a solution of HC2H3O2 Stay the same
pH = 4.73 0.060 M
Finish problems in slides (on my website calendar with answers) Take notes on 17.2
