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58 Cards in this Set
- Front
- Back
What is an Arrhenius acid?
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a substance that increases the concentration of H+ ions in water (i.e. HA)
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What is an Arrhenius base?
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a substance that increases the concentration of OH- ions in water (i.e. MOH)
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What is the common ion effect?
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the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance
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What does the pressence of a common ion do?
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suppresses the ionization of a
weak acid or a weak base |
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What is a Bronsted acid?
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a proton (H+) donor
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What is a Bronsted base?
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a proton (H+) acceptor (if it's strong it could be aka a proton "grabber")
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What ability does a buffer solution have?
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to resist changes in pH upon the addition of small amounts of either acid or base (so the change in pH, relative to an un-buffered solution is slight)
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What is a buffer solution composed of?
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a weak acid and a salt containing the conjugate base
OR a weak base and a salt containing the conjugate acid OR a weak acid/base and an appropriate amount of a strong base/acid (like HCl) |
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True or False? A base will not have unpaired (lone pair) electrons.
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False
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What charges can a base have?
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neutral or negative
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How much of a strong acid protonates (transfers protons to) a weak base?
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100%
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What does every Bronsted acid/base have?
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a conjugate base/acid
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What are conjugate acid-base pairs?
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chemical species whose formulas differ only by one proton
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What can an amphiprotic substance do?
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act as either a proton donor or proton acceptor
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How do strong and weak electrolytes dissociate?
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strong = 100% dissociation
weak = not completely dissociated |
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What are the 6 strong acids that were asked to be memorized?
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HCl, HBr, HI, HNO3, HClO4, H2SO4 (only the first proton is considered strong)
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True or False? Bases with alkali or alkaline earth metals are strong.
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True
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How strong of electrolytes are weak and strong acids/bases?
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weak acids/bases = weak electrolytes
strong acids/bases = strong electrolytes |
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Where does the equilibrium lie/predominate in any acid-base pairing?
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with the weaker acid and weaker base
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True or False? The weak acid is always paired with the weak base and that the strong acid is always paired with the strong base.
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True (so once you know one, you will know the others)
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True or False? Strength of an acid/base is the same as concentration.
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FALSE
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What is the strongest acid that can exist in aqueous solution?
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H3O+
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What is the strongest base that can exist in aqueous solution?
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OH-
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What is the ion-product constant?
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(Kw) = the product of the molar concentrations of H3 O+ and OH- ions at a particular temperature (at 25 degrees C = 1.0 * 10^-14)
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What are the formulas for pH and pOH and what do they add to?
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pH = -log[H+]
pOH = -log[OH-] pH + pOH = 14 |
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How do you find [H+] / [OH-] if given pH / pOH?
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[H+] = 10^-pH
[OH-] = 10^-pOH |
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True or False? Each number increase/decrease on the pH sale represents a 10-fold increase/decrease.
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True
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As Ka (the acid-dissociation/ionization constant) increases, what happens to pKa and weak acid strength?
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pKa decreases and weak acid strength increases
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What is the % ionization formula?
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( [H+] at equilibrium / initial [acid] ) * 100%
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What happens to % ionization as weak acid is diluted with water?
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it increases
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What happens to weak base strength as Kb (the base ionization constant) increases?
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it increases
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What does Kw equal in relation to Ka and Kb for weak acids/bases and their conjugates?
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Kw = Ka * Kb
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What affects pH (cation or anion) for neutral, acidic, and basic solutions?
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Neutral Solutions – The cation and anion do not affect pH.
Basic Solutions: – The anion affects pH. Acidic Solutions: – The cation affects pH. |
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What is the Inductive Effect?
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“Movement or withdrawal” of electrons from neighboring bonds by either electronegative atoms or positive-charged atoms.
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When is the solution basic, acidic, and neutral for solutions in which the cation AND anion affect pH?
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Basic: Kb for the anion > Ka for the cation
Acidic: Kb for the anion < Ka for the cation Neutral: Kb for the anion ≈ Ka for the cation |
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What 3 factors does the acidity of hydrogen (the ease in which the proton dissociates from the molecule) depend on when hydrogen is bonded to another element?
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H-X bond strength, H-X bond polarity, & the stability of the conjugate base (X−) (high stability = no base activity)
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When does acidity increase for binary acids?
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from left to right across a row (H-X bond polarity increases) AND from top to bottom down a group (H-X bond strength decreases)
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When will the O-H bond be more polar and easier to break?
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If Z is very electronegative or Z is in a high oxidation state (more oxygens bonded to it).
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When does acid strength increase for oxyacids?
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with increasing electronegativity and oxidation #'s of Z
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What is a Lewis acid?
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a substance that can accept a pair of electrons
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What is a Lewis base?
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a substance that can donate a pair of electrons
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What happens to a buffer solution when a strong acid/base is added?
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Strong acid: excess protons are neutralized by the weak base
Strong base: excess hydroxide ions are neutralized by the weak acid |
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What is the Henderson-Hasselbalch equation?
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pH = pKa + log( [conjugate base]/[acid] )
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What is buffer capacity?
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the amount of acid or base neutralized by the buffer before there is a significant change in pH
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True or False? The greater the amounts of conjugate acid-base pair, the greater the buffer capacity.
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True
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What happens to a buffer solution when a strong acid/ base is added?
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Strong acid: weak acid increases, weak base decreases
Strong base: weak base increases, weak acid deceases |
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When is the reaction complete in an acid-base titration?
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at the equivalence point
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What is equal at the equivalence point?
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mol acid = mol base
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In a strong acid-strong base titration, what is the relationship between [H+] and [OH-] before and after equivalence point?
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Before the equivalence point: [H+] > [OH−]
After the equivalence point: [H+] < [OH−] |
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What is the pH at the equivalence point in a weak acid-strong base titration?
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pH > 7
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What is equal at the "half-way equivalence point?
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[A-] = [HA]
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True or False? Ionic Compounds are infinitively soluble in water.
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False
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What is the Solubility Product Constant (Ksp)?
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the product of the molar concentrations of constituent ions IN A SATURATED SOLUTION raised to their stoichiometirc powers (it provides a measure of a compound’s solubility)
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What is molar solubility?
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the number of moles of solute dissolving to form a liter of saturated solution (in M) (it refers to the “parent” compound)
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What is solubility?
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the amount (grams) of substance that dissolves to form saturated solution (in g/L)
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What does the presence of a common ion do to the solubility of a salt?
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it decreases it
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What happens to the solubility of "insoluble" bases in acidic solutions?
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it increases
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What is the relationship between Ksp and Q for unsaturated, saturated, and supersaturated solutions?
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Ksp > Q for Unsaturated
Ksp = Q for Saturated Ksp < Q for Supersaturated (precipitate forms) |