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Part 1: Establishing equilibrium.
You dissolve solid AgCl into water. (Ksp =1.8 x 10-10) Calculate the concentration of chloride ions present after the reaction reaches equilibrium.
Part 2: Le Chatelier
You add 1mL of 0.004 M HCl to 1L of the solution. Will the solid AgCl precipitate, dissolve further, or not change? Support your answer with the relevant chemical reaction and a calculation.
Part 3: Predicting Direction of Equilibrium
In a different beaker you add 10 mL of .002 M NaCl to 5 mL of .003 M AgNO3. Will AgCl precipitate? Support your answer with a calculation.
In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Ch telier's principle
A student placed 12.5 g of glucose in a volumetric flask, added enough water to dissolve the glucose by swirling
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When 4.220 g of calcium hydroxide is reacted with a 30.0 mL of a 0.200 M sulfuric acid solution how many grams of calcium sulfate and water are formed?
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