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Applications of Aqueous Equilibria Common Ions When we dissolve acetic acid in water, the following equilibrium is established: –CH 3 COOH CH 3 COO -
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ACID/BASE SOLUTIONS. What is an acid? Bronsted-Lowry definition: An acid is a proton donor. So, what’s a base? Bronsted-Lowry definition: A base is a
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Aqueous Equilibria Chapter 15 Applications of Aqueous Equilibria
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The End of Equilibrium! (well, for us!) 1. K sp What is the solubility of FeCO 3 ? Solubility = MAXIMUM amount of a compound that can dissolve in water
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Basic concepts: Acid-Base chemistry & pH 1.Recognizing acid/base and conjugate base/acid 2.Calculation of pH, pOH, [H 3 O + ], [OH - ] 3.Calculating pH
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Titration Curves What’s in the beaker. Always ask… What’s in the beaker? When I start the titration, there is only water and whatever it is I’m titrating
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Titration Example Problem Suppose that 10.0g of an unknown monoprotic weak acid, HA, is dissolved in 100 mL of water. To reach the equivalence point, 100.0mL
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IICWG-8, 22-26 Oct. 2007
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Goes with chapter 19: Silberberg’s Principles of General Chemistry AP Chemistry Mrs. Laura Peck, 2013 1
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Indicators. Acid Base indicators Acid-base indicators can mark the end point of a titration by changing color. The equivalence point is defined
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Buffers
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Chapter 15 Applications of Aqueous Equilibria
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