Chemistry Report

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Solution Stoichiometry and Gas Law Problems Problem 1 In flask A, 1.500g of silver nitrate solid is dissolved in 50.0mL of water, while in flask B, 0.500g of potassium carbonate is dissolved in 25.0mL of water. The two solutions are then mixed together. a) Before mixing, what is the molarity of each solution? b) Write the balanced molecular equation, the complete ionic equation, and the net ionic equation for the reaction. c) If the percentage yield is 85.0%, what mass of precipitate is actually produced? d) How many moles of silver ions remain in solution? e) What is the concentration (M) of potassium ions that remain in solution? Problem 2 Ethanol (C2H5OH) reacts with permanganate ions in acidic solution to produce acetic acid and manganese (II) ions. Since this reaction involves a dramatic color change, it can be used in a titration experiment. Here is the net ionic equation: 12 H+ (aq) + 4 MnO4– (aq) + 5 C2H5OH (aq) ⎯→ 5 HC2H3O2 (aq) + 4 Mn2+ (aq) + 11 H2O (l) deep purple almost colorless 1.00 mL of a white wine was added to excess sulfuric acid solution, then titrated with a 0.100 M KMnO4 solution. It took 20.4 mL of the KMnO4 solution to reach the endpoint. a) Which substance is oxidized, and which reduced, in the reaction? b) What is the molar concentration (molarity) of ethanol in the wine? Chem 131 Solution Stoichiometry and Gas Law Problems Page 1 Problem 3 As part of some research for the product Alka-Seltzer, a researcher combines 0.840g sodium bicarbonate with 100.0 mL of 0.0500 M citric acid (H3C6H5O7). a) Write the molecular, complete ionic, and net ionic equations for this reaction (assume that each molecule of citric acid is completely neutralized). b) If the dry gas that the student actually collects occupies a volume of 0.196 L at 25°C and 1.00 atm pressure, what is the percentage yield of this reaction? c) The researcher

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