Chem Equilibrium Quiz #2
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Last updated 3:33 AM on 12/22/22
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21 Terms
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Properties of Acids
* produce H+ (as H3O+) ions in water
* taste sour
* corrode metals
* electrolytes
* react with bases to form a salt and water
* pH is less than 7
* turns blue litmus paper red
* taste sour
* corrode metals
* electrolytes
* react with bases to form a salt and water
* pH is less than 7
* turns blue litmus paper red
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Properties of Bases
* produce OH- ions in water
* taste bitter, chalky
* are electrolytes
* feel soapy, slippery
* react with acids to form salts and water
* pH greater than 7
* Turns red litmus paper blue
* taste bitter, chalky
* are electrolytes
* feel soapy, slippery
* react with acids to form salts and water
* pH greater than 7
* Turns red litmus paper blue
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Arrhenius Theory of Acids and Bases
Acid: Produces H+ ions
Base: Produces OH- ions
\
Limitation: %%Ammonia%%
Base: Produces OH- ions
\
Limitation: %%Ammonia%%
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Bronstead-Lowry Theory of Acids and Bases
Acid: ==Proton Donor==
Base: ^^Proton Acceptor^^
\
Proton: A proton is really just a hydrogen atom that has lost its electron.
Base: ^^Proton Acceptor^^
\
Proton: A proton is really just a hydrogen atom that has lost its electron.
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Conjugate Acid-Base Pairs
Two substances that are related by the gain or the loss of a proton
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pH
* H2O can function as an acid and base
* in pure water there can be amphirotic
* in pure water there can be amphirotic
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Ion -Product Constant of Water (Kw)
Kw= \[H+\]\[OH-\]
=1.00 x 10-14
=1.00 x 10-14
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The nature of solutions
Acidic \[H+\] > \[OH-\]
\
Neutral \[H+\] = \[OH-\]
\
Basic \[H+\] < \[OH-\]
\
Neutral \[H+\] = \[OH-\]
\
Basic \[H+\] < \[OH-\]
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Weak Acid
an acid that ionizes to the limited extent in water
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Strong Acids
an acid that dissociates completley into ions in water
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Acid-Dissociation Constant Ka:
The equilibrium constant for the dissociation of an acid into ions or the ionization of an acid.
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Monoprotic Acid
an acid that yields one proton H+, when it ionizes
\
HA + H2O
\
HA + H2O
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Polyprotic acids
contain more than one acidic proton, break apart in multiple steps
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About Ka
Stronger acids → higher \[H+\] →Larger Ka values
Weak acids → lower \[H+\] → smaller Ka values
Weak acids → lower \[H+\] → smaller Ka values
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Percent Dissociation
the ratio of the concentration of ionized acid at equilibrium to the acid’s initial concentration expressed as a percentage
\
Percent Dissociation = \[A-"\]
------ x 100%
\[HA\] Initial
\
Weak acids →lower % dissociation → smaller Ka values
\
Percent Dissociation = \[A-"\]
------ x 100%
\[HA\] Initial
\
Weak acids →lower % dissociation → smaller Ka values
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General Equation for Base Ionization
B + H2O
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Facts:
* the ==conjugate of a strong acid== is always a ^^weak base^^
* the conjugate of a ^^strong base^^ is always a ==weak acid==
* the conjugate of a ^^strong base^^ is always a ==weak acid==
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==Strong Acids==
* HX (all but F)
* HNO3
* H2SO4
* HClO3
* HClO4
* HNO3
* H2SO4
* HClO3
* HClO4
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^^Strong Bases^^
* LiOH
* NaOH
* KOH
* RbOH
* CsOH
* Mg(OH)2
* Ca(OH)2
* Sr(OH)2
* Ba(OH)2
* NaOH
* KOH
* RbOH
* CsOH
* Mg(OH)2
* Ca(OH)2
* Sr(OH)2
* Ba(OH)2
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\[non-ionized\]
| \[H+\]/\[OH-\] - Original Concentration |
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\[Initial\]
Calculated (n) + \[OH-\]/\[H+\]