First set of notes after exam 3
First set of notes after exam 3 chem 10061-001
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This 2 page Class Notes was uploaded by Matthew Goetz on Wednesday April 27, 2016. The Class Notes belongs to chem 10061-001 at Kent State University taught by David bowers in Summer 2015. Since its upload, it has received 16 views. For similar materials see general chemistry 2 in Chemistry at Kent State University.
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Date Created: 04/27/16
First Chem study guide after exam 3: Buffer capacity: A buffer’s ability to resist pH change. Higher concentrations of buffer components have higher capacities. pH of a buffer is independent of its capacity, concentration is more important. Buffer range: Range over which a buffer works effectively. Most buffers have range of +/ 1 pH. How to prepare a buffer: Choose your conjugate acidbase pair. Use the Henderson Hasselbach equation to calculate the ideal ratio between them. Use this ratio to calculate the amounts of each to mix together. Mix the solutions…. AcidBase titrations: A way to quantify a reaction. Base is dropped into acid until color change to decide pH based on how much base was needed. Uses indicators, which are weak organic acids that respond to pH changes by changing color. Most indicators have a pH range of 2. 3 Types of titration curves may be made: Strong acid + weak base = pH at equivalence point is less than 7. Strong acid + strong base = pH at equivalence point is 7. Weak acid + strong base = pH at equivalence point is greater than 7. We may now term formerly “insoluble salts” as slightly soluble. This salts experience very little dissociation before equilibrium is reached. Solubility product constant (Ksp): Equilibrium for slightly soluble ionic compounds in H2O. Higher the Ksp, the more soluble the salt is. Ksp shows how quickly equilibrium is reached based on amount of products that form before it is reached. Solid and pure liquid concentrations are still not considered when solving for Ksp. O^2 and S^2 are very strong bases, so they automatically react with H2O. Therefore, they will never exist in a solution alone. Rather, they readily form SH or OH in solution. S is used to compare solubility of salts regardless of how many ions are in each salt. Ksp may not do this. To compare Ksp the salts must have equal numbers of ions. Solubility of ionic salts: Does not change in the presence of a strong acid if the acid’s anion is present in the salt as well. Salts become more soluble in presence of a strong acid if they have an anion of a weak acid though. Adding a common ion may decrease the solubility of salts.
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