Acid and Bases Flashcards

Terms Definitions
phosphoric
H3PO4
neutral
pH=7
HNO3
H2SO4
H2SO3
Sulfurous Acid
pOH formula
pOH=-log10[OH-]
[OH-]=10^-pOH
NaOH
Sodium hydroxide
HC6H7O6
ascorbic acid
base pH
8-14
Litmus pH
7
pH (expression)
-log[H30+]
RbOH
Strong Base
HCN
weak acid
HNO_3
nitric acid (Strong)
NH3
ammonia, weak base
KOH
potassium hydroxide
strong base
Strong Base
Strong/Weak Base/Acid?
RbOH
HNO2 (nitrous acid)
H2CO3
Lewis base
electron pair DONOR.
Hydronium Ion
an +H3O unit
diprotic acid
two acidic protons
Bronsted-Lowry base
a proton acceptor
what is alkalotic HCO3-?
27
HCl
Strong acid H+(aq) + Cl-(aq)
Base ions
solution w/many OH- ions
pOH
Means potential of hydroxide ions
COOH
Caboxylic acids have _______________ group
Other Helpful Equations
pH + pOH=14
Kw=[H+][OH-]= 10^-14
strong acids
completely ionize in aqueous solutions
characteristic of acid
sour taste
contain H+
conduct electricity
reacts with CO3(2-) to produce CO2
react with metals to produce H2
Phenolphthalein
indicator that remains colorless in the presence of acids but turns pink in the presence of bases
Name a specific carbonic anhydrase inhibitor
acetazolamide
amphoteric
describes water and other substances that can act as both acids and bases
Salt
A compound formed when negative ions from an acid combine with positive ions from a base.
stronger
The higher Kb the ___ the base.
indicator
an organic molecule that changes color in an acid and base and contains primarily carbon and hydrogen
Strong Bases I
NaOH, LiOH, KOH, RbOH, CsOH
properties of bases
taste bitter
feels slippery
turns red litmus paper blue
conducts electrical current
pH scale
measure of the concentration of hydrogen ions in a solution
The point of neutralization is the _____ point of the titration
end
Acid
solution with a ph of below 7-0
Lewis acid
electron pair acceptor, empty atomic orbital
electrolyte
a compound that ionizes in water, allowing the solution to conduct electricity
Hydrogen ions
Acids produce _____ when dissolved in water
Ph meter
an instrument which gives the exact measurement of the acidity of a solution
Polar Molecule
A molecule with opposite charges on each end
conjugate base
everything that remains of the acid molecule after a proton is lost
Conjugate Acid
the species that results from the addition of a proton to a Bronstead base
stronger the acid
The more polar the H-X bond
binary acid
an acid that contains only two different elements
weak acid
acid that ionizes only partially in dilute aqueous solution
pH <7.35low cloridenormal anion gap
Type II RTA-proximal tubule
end point
The point at which the indicator used in a titration changes color.
pH meters
are used to make rapid, accurate pH measurements
Non Electrolyte
is a solution that does not conduct electricity
In this process, the cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water
salt hydrolysis
How do we estimate the pH of an aqueous solution of an amphiprotic salt?
pH=1/2(pKa1+pka2)
neutralization reaction
acid and base react to form salt and often H2O. The salt may precipitate out or remain ionized in solution. General formula: HA + BOH <-> BA + H2O
low pH
0-6.9; it is acidic and has a high number of H⁺
titrant
The acid or base that you add to the unknown species in a titration. You know the precise concentration of the titrant.
SaO2 tells you about
Hemoglobin. Giving O2 doesn't help if you don't have the hemoglobin to carry it.
ion-product constant of water
The product of [H3O+] X [OH-] in solution=(1.00 x 10-7) X (1.00 x 10-7) = 1.00 x 10-14
Examples of Common Bases
* detergents
* soap
* lye (NaOH)
* household ammonia (aqueous)
If CO2 is high what signs will the pt exhibit?
Obtunded, sleepy, difficulty arousing.
weak acid Ka equation; how does Ka correspond to strength of acid
Ka = [H3O+][A-]/[HA] ; small Ka = weak acid, it will dissociate less
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Term:
Definition:
Definition:

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