Question

I know some of the measured pH values are a little off due to error in the lab, but I need help filling out the “Ion Hydrolyzed” table and then the “Net Ionic Equation” part. I remember doing net ionic equations in General Chemistry I, bit don’t see how it applies here.

Thanks, in advance! (i will rate!)

Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its pH. 3. To determine the acid dissociation constant of acetic acid using the Henderson-Hasselbach equation. 4. To test a buffer's capacity by reacting it with a strong acids and a strong base. Discussion: Buffers are solutions that resist changes in pH when small quantities of an acid or base are added to them. These solutions contain a weak acid and its conjugate base or a weak base and its conjugate acid. Because these mixtures contain both the acidic and basic species, they can easily neutralize small quantities of either Hi or OH. Buffers are also resistant to dilution effects, maintaining the same pH even when water is added to them. Part A: Acidic and Basic Properties of lonic Compouds The first part of the experiment involves using a pH meter to determine the pH of several salt solutions. A pH meter consists of a meter and two electrodes. The measurement of pH requires two electrodes, a sensing electrode that is sensitive to H3O+ concentration and a reference electrode. This is because the pH meter is really a voltmeter that measures the electrical potential of a solution. The reference electrode is an electrode that develops a known potential that is essentially independent of the contents of the solution into which it is placed. The glass electrode is sensitive to the H2O concentration of the solution into which it is placed. Part B: Buffers A buffer system will be prepared from solutions of conjugate acid-base pairs. The pH of the buffer system will be determined using the pH meter. The K of the weak acid used in the buffer will be calculated using the pH data. The effect of adding an acid and a base to the system will be monitored. For a weak acid, Reaction: HA (aul + H20 - H,O*raq + Alaal And K = [H3OA1 [HA] Knowing the experimentally determined pH of the solution the [H3O') can be calculated from pH = -log[H3O'] The K of the buffer system can be calculated from the Henderson-Hasselbalch equation pH = pk + log [A] [HA]

Answer 1

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