Chem Exam Chapter 14&15

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