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VOLUMETRIC ANALYSIS THE TITRATION OF ACIDS AND BASES PART II 1. (a) A titration of 5.00 mL acetic acid required 24.84 mL of 0.2074 M sodium hydroxide for complete neutralization. Calculate the molarity (moles/L) of the acetic acid. Note: since the mole ratio between acetic acid and sodium hydroxide is 1:1, the following equation applies MaVa = M.Vb, where M = molarity (moles/L), V = volume, a = acid (acetic acid), b = base (sodium hydroxide). Show the calculation and use proper number of sig figs. (b) Convert the answer in 1a from moles/L to g/L. (Hint: use the molar mass for acetic acid; CH3COOH) (c) A titration of a sample of an unknown monoprotic acid required 31.72 mL of 0.2074 M NaOH to reach the endpoint. Calculate the number of moles of NaOH added. Show the full calculation and use proper number of sig figs. 2. Describe the procedure for PART Il (Second Week) (Steps 1 & 2) of the experiment. This could be in an outline format or a flow chart format or paragraph format. It should not be copied directly from the manual. (This should be between 1/2 and one page, you may use the back of the page) 3. Briefly discuss all safety precautions related to this experiment. (Chemical and equipment related.)

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