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19 Cards in this Set
- Front
- Back
Buffer (Buffer solution)
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A solution that prevents a change in pH greater than 1
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Contents of a Buffer solution
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A weak acid that can react with added base, and a weak base that can react with added acid. The acid and base components must not react with each other
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A buffer solution usually consists of . . .
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. . . equal quantities of a weak acid and its conjugate base, or a weak base and its conjugate acid
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Henderson-Hasselbalch Equation - definition
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Used to calculate the pH of a buffer containing known concentrations of conjugate base and conjugate acid
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Henderson-Hasselbalch Equation - formula
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pH = pKₐ + log ([conj base] / [conj. acid])
or pH = pKₐ ([A-] / [HA]) |
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Equivalence point of a titration
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When the stoichiometric amount of titrant added exactly neutralizes the analyte
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End point of a titration
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When the indicator changes color during a titration
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Buffer capacity
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The quantity of acid or base added to the buffer that the buffer can accommodate with undergoing significant change (more than 1 pH unit)
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Titration curve
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A graph of pH as a function of the volume of titrant added
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Solubility Product Constant: symbol
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Ksp
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Solubility Product Constant: definition
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The magnitude of Ksp indicates the extent to which the solid solute dissolves to ions in solution
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Solubility Product Constant: Formula
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if the balanced equations is:
AxBy(s) ⇋ xA^(n+)(aq) + yB^(m-)(aq) then Ksp = [Aⁿ⁺]^x[B^m-]^y |
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The is no denominator in the formula for the Solubility Product Constant because . . .
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. . . the reactant is always a pure solid
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Solubility Product constant: formula in words
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Ksp equals the product of the equilibrium molar concentrations of the cation and the anion, each raised to the power given by the coefficient in the balanced equation representing the solubility equilibrium
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Solubility
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The amount of solute per unit volume of solution (mol/L) that dissolves to form a saturated solution
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Solubility product constant - meaning
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The equilibrium constant for the chemical equilibrium that exists between a solid ionic solute and its ions in a saturated solution
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Common ion effect
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The presence of a second solute that provides a common ion that lowers the solubility of an ionic compound
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Amphoteric
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Can react with both H₃O⁺ and OH⁻ ions
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Regarding solubility, comparing Q and Ksp
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1. Q < Ksp: solution is unsaturated, no precipitate forms
2. Q = Ksp: solution is saturated 3. Q > Ksp: solution is supersaturated, precipitate forms |