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Arrhenius Acid
substance that increases the concentration of H+ or H30+ ion concentration in solution
Bronsted-Lowry Acid
substance that is an H+ ion or proton donor(gives away)
Arrhenius Base
substance that increases the concentration of OH- or hydroxide ion concentration in solution
Bronsted-Lowry Base
substance that is an H+ ion or proton acceptor(takes in)
Strong acids that dissolve in water
fragile molecule that ionizes close to 100% and above 80%; considered strong electrolyte: forms high ions
Weak acids that dissolve in water
fragile molecule that ionizes far less than 100% and below 80%; considered weak electrolyte: forms low ions
strong; high
(___ electrolytes) _____ concentration ions = high conductivity
weak; low
(___ electrolytes) _____ concentration ions = low conductivity
Strong bases that dissolve in water
tend to be ionic compounds according to Arrhenius definition; will have high conductivity or strong electrolyte
weak bases that dissolve in water
tend to be molecular compounds according to Bronsted-Lowry definition; will have low conductivity or weak electrolyte
nonelectrolyte
substance that dissolves in water, but does NOT form ion, therfore does not conduct electricity
conductivity
the ability to allow heat or electricity to pass through
Acid
substance that increases H+ or H3O+ concentration in water
usually starts with H atom or ion
Acid Identifier
Concentration/Molarity
designated amount of solute dissolved in a given quantity of solvent or quantity of solution
Molarity
expresses the concentration of a solution as the number of moles of solute in a liter of solution; most common way of describing concentration
dilute mixture
fewer dissolved particles per unit volume
dilution or dilution process
process of decreasing the concentration by adding additional solvent
mixture
two or more pure substances that are not chemically bonded
solution
a homogenous mixture with uniform distribution or even compositions
stock/standard solution
solutions used routinely in the laboratory with known concentration<
M=n/V
molarity equation
V=n/M
volume equation
n=(M)(V)
n equation
concentrated mixture
larger/higher dissolved particles per unit volume; pushes particles closer together
concentration process
process of increasing the concentration by removing solvent
solute
substance found in lower amount within a mixture; usually substance being dissolved
solvent
substance found in higher amount within a mixture; usually substance doing the dissolving
initial concentration
M1 meaning
initial volume
V1 meaning
final concentration
M2
final volume
V2
Neutralization reactions/Acid-Base Neutralization
acids are direct opposites of bases and cancel out when they come in contact; usually an example of double replacement reactions
acid + base
General Acid-Base reaction products
acid + active metal
Acids react with active metal products
single replacement
acids react with active metal reaction type:
active metals
usually element in G1 and sometimes G2 of the periodic table; tend to have high reactivity and low stability
pH
simplified unitless measure of [H+] concentration for a solution
the power of hydrogen
pH meaning
7
what is the safest pH range?
amphoteric
substance that can act as both an acid or base depending upon the reaction conditions; ex. water
simple
0 pH
strong acid
1-4 pH
weak acid
4-6 pH
neutral
7 pH
weak base
8-11 pH
strong base
11-14 pH
pH = -log[H+]
pH equation
[H+] = 10^-pH
[H+] or[H3O+] eqiuation
kw=[H+]/[OH-]
kw equation
[H+] = kw/[OH-]
[H+] equation
[OH-] = kw/[H+]
[OH-] equation
1.0*10^-14
kw value
titration
lab technique using a known concentration to determine an unknown concentration
burette/buret
very accurate volumetric delivery measurement device used in titration
meniscus
small liquid curve within graduated cylinder/buret; readings done in reverse
V = VF-VI
volume equation by buret
acid-base indicators
compound whose color change are sensitive to certain pH
titrant
solution of known concentration or stock/standard solution; delivered form the buret
analyte
solution of unknown concentration; played in the E-flask
Erlenmeyer flask
small neck flask used mostly in titration
parralax
incorrect reading of graduated cylinders/burets; need to read at eye level
endpoint
point where indicator changed color, stop titration
equivalency point
point where the concentration of the acid and concentration of base are equal; pH is 7
pH curve/graph
graph that relates the pH to amount of titrant added
MAVA=MBVB
short titration equation
volx ->molesx ->molesy
long titration equation
Bronsted-Lowry Acid
substance that is a proton/[H+] donor
Bronsted-Lowry base
substance that is a proton/[H+] acceptor
monoprotic acids
acids that can release 1 hydrogen, released one at a time
diprotic acids
acids that can release two hydrogen, released one at a time
triprotic acids
acids that can release three hydrogen, released one at a time
conjugate acid
species that remains after the proton has been donated
conjugate base
species that remains after the proton has been accepted
buffers
substances that resist changes to pH; made from acid and its conjugte base or vise versa