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20 Cards in this Set
- Front
- Back
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Name this compound as an acid.
HCN |
cyanide
-ide = hydro...ic acid hydrocyanic acid |
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Name this compound as an acid.
H3PO4 |
Phosphate
-ate = -ic acid phosphoric acid |
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Name this compound as an acid.
(SO3)2- |
sulfite
-ite = -ous acid sulfurous acid |
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What is the reaction in which 2 water molecules produce ions?
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self-ionization of water
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What is the ion-product constant for water (Kw)?
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Kw = [H+] x [OH-] = 1.0e-14M2
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Acid or Base?
pH = 3.2 |
Acid
Acidic solutions: pH < 7.0 [H+] > 1.0x(10)-7 |
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What is the equation involving [H+] to find the pH value?
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pH = -log[H+]
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What is the pH of a solution if [OH-]=4.0e-11?
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Kw = [4.0e-11]x[H+] = 1.0e-14
so... 1.0e-14/4.0e-11 = 2.5e-4 = [H+] pH = -log[2.5e-4] = 3.60 (no units for pH) |
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Monoprotic, diprotic, or triprotic?
H3PO4 |
triprotic
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Arrhenius Acids and Bases
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*acids: hydrogen ion (H+) producers
*bases: hydroxide ions (OH-) producers |
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What is an exception to the Arrhenius Acid and Base rules?
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NH3 is a base in water and has no hydroxide
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STRONG ACIDS
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HCl (hydrochloric acid)
H2SO4 (sulfuric acid) HNO3 (nitric acid) *almost everything else is a weak acid* |
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Define acids and bases under the Bronsted Model.
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*Acids donate protons (hydrogen-ion donor)
*Bases accept protons (hydrogen-ion acceptor) *This explains the behavior of ammonia* -Ammonia acts as a base b/c it accepts a hydrogen ion from water NH3 + H20 = (NH4)+ +OH- -water, the hydrogen-ion donor, is a Bronsted acid |
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conjugate acid
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particle formed when a base gains a hydrogen ion
e.g. (NH4)+ is conjugate acid of the base NH3 |
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conjugate base
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particle that remains when an acid has donated a hydrogen ion
e.g. OH- is the conjugate base of the acid water |
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conjugate acid base pair
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2 substances related by the loss or gain of a single (NOT 2) hydrogen ions
HCl + H20 = H30+ + Cl- acid base conj.acid conj.base |
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amphoteric
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substance that can act as both an acid and a base (e.g. water)
*in reaction w/ HCl, water accepts a proton and is therefore a base *in reaction w/ NH3, water donates a proton and is therefore an acid |
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Define a Lewis acid.
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substance that can accept a pair of electrons to form a covalent bond
*electron-pair acceptor |
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Define a Lewis base.
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substance that can donate a pair of electrons to form a covalent bond
*electron-pair donor |
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Give an example of Bronsted compared to Lewis.
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H+ + OH- = H20
*Here the hydroxide ion is a Lewis base. It is also a Bronsted-Lowry base. The hydrogen ion is both a Lewis acid and Bronsted acid |
