<p>1CHEM 2115 Lab Report Experiment #11 Acids, Bases, Salts & Buffers Chem I Lab</p><p>Section # Station # Date </p><p>A. Acid-Base Neutralization I. Describe your observations in the table below.</p><p>Observations</p><p>Solid residue</p><p>AgNO3 addition</p><p>Flame test</p><p>II. Write a balanced chemical equation for the neutralization reaction you observed.</p><p>B. pH Measurement I. Record the measured pH for the substances listed below.</p><p>Substance pH Substance pH Substance pH Lemon Juice Ammonia Baking soda Laundry Orange juice Aspirin detergent Dishwashing Buffered Milk detergent aspirin C. Acid-Base Indicators</p><p>Indicator Color in 0.05 M HCl Color in 0.05 M NaOH Methyl red Bromcresol green Phenolphthalein Methyl orange Methyl violet</p><p>I. Which indicator would be best in distinguishing between 0.05 M HCl and 0.05 M NaOH? Which would be the worst? Justify your answer.</p><p>D. Behavior of Salt Solutions</p><p>Salt Solution pH Sodium acetate Sodium carbonate Ammonium chloride Sodium chloride Boiled distilled water</p><p>I. Which ions exhibit significant Brønsted acid character? Brønsted base character? Are your results consistent the expected results based on the theory of hydrolysis? E. Buffers</p><p>Buffer Initial pH pH after adding HCl pH after adding NaOH Solution A Solution B Solution C Solution D Boiled water</p><p>I. Which solutions are able to buffer well against acid? Against base? Explain.</p><p>II. Are any solutions able to buffer well against both acid and base? Explain.</p><p>III. Do any solutions show little or no buffering ability? Explain.</p><p>IV. Write equations to show how a buffer made up of equimolar amounts of acetic acid, - CH3COOH, and acetate, CH3COO , would behave when (a) HCl is added and (b) NaOH is added.</p><p>V. At what point is a buffer solution no longer effective in resisting a pH change when a strong acid is added?</p>