Unit 8: Acids and Bases
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20 Terms
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Neutralization reactions
________ occur when an acid donates its proton to a base.
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weak acids
Indicators are ________ that change colors based on pH change.
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Strong acids
________ will dissolve completely in water and never reach equilibrium.
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1x10^-14
value of Kw constant
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14
pH + pOH =
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1x10^-14
\[H+\]\[OH-\] =
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buffer
A(n) ________ is a solution with a stable pH.
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Polyprotic acids
________ can give up more than one hydrogen in a solution.
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Bases
________ do not dissociate but accepts protons.
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equivalence point
When just enough acid/base is added to an acid/base to neutralize
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half-equivalence point
when exactly half the amount of acid/base is turned into its conjugate in a titration
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pH
Increasing ________ means decreasing [H+] and making a solution less acidic.
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Greater Ka value
________ means more acid dissociation (stronger acid)
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Greater Kb value
________ means more protonatization (stronger base)
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Complete dissociation, only hydrogen and hydroxide ions remail
Strong acid and strong base reaction
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Proton is donated, conjugate of base is created
Strong acid and weak base reaction
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Protons accepted, created conjugate of acid and water
Weak acid and strong base
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Simple proton transfer
Weak acid and weak base reaction
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Ka
equilibrium constant for weak acids
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Kb
equilibrium constant for weak bases
