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16 Cards in this Set
- Front
- Back
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common ion
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ex. NaF yields Na and F, common ion is F
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common ion effect
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the shift in an equilibrium position caused by the addition or presence of an ion involved in the equilibrium reaction
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buffered solution
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a solution that resists a change in its pH when either OH ions or protons are added
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Henderson Hasselbalch equation
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an equation giving the relationship between the pH of an acid-base system and the concentrations of base and acid; pH= pKa + log([base]/[acid])
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buffering capacity
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the ability of a buffered solution to absorb protons or OH ions without a significant change in pH
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pH curve
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a plot showing the pH of a solution being analyzed as a function of the amount of titrant added
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millimole
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a 1000th of a mole
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equivalence point
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the point in a titration when enough titrant has been added to react exactly with the substance in solution being titrated
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acid-base indicator
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a substance that marks the end point of an acid-base titration by changing color
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phenolphthalein
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an indicator that is colorless in acidic and pink in basic form
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ion product
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the equilibrium constant for the autoionization of water; Kw= [H][OH]
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selective precipitation
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a method of separating metal ions from an aqueous mixture by using a reagent whose anion forms a precipitate with only one or a few of the ions in the mixture
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qualitative analysis
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separating cations into 5 major groups based on solubilities
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complex ion
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a charged species consisting of a metal ion surrounded by ligands
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formation constants
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the equilibrium constant for each step of the formation of a complex ion by the addition of an individual ligand to a metal ion or complex ion in aqueous solutions
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solubility product constant
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the constant for the equilibrium expression representing the dissolving of an ionic solid in water
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