Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
327 Cards in this Set
- Front
- Back
|
What is nitrate?
|
NO subscript 3 wth a - charge
|
|
|
Nitrite?
|
NO 2 - charge
Nitrate= NO3 - charge |
|
|
Sulfate?
|
SO 4 and a charge of -2.
|
|
|
Sulfite?
|
SO3 and a charge of -2.
|
|
|
Phosphate?
|
PO with a subscript of 4 and a charge of -3.
|
|
|
Phospite?
|
PO 3 and a charge of -3.
|
|
|
Phospide? Sulfide? Nitirde?
|
P with a charge of -3, S with a charge of -2, and N with a charge of -3.
|
|
|
Carbonate?
|
CO with a subscript of 3 and a charge of -2.
|
|
|
Carbonite?
|
CO with a subscript of 2 and a charge of -2.
|
|
|
Carbonide?
|
C with a charge of 4.
|
|
|
ammonium?
|
NH4 +
|
|
|
Chlorate and carbonate?
|
ClO witha subscript of 3 and a charge of -.
CO with a subscript of 3 and a charge of -2. |
|
|
Chlorite? Hydrogen carbonate?
|
ClO 2 and a charge of -.
HCO3 with a charge of -. |
|
|
Cyanide?
|
CN-
|
|
|
Acetate?
|
C2 H3 O2 with a charge of -
|
|
|
Hydrogen sulate?
|
HSO with a subscript of 4 and a charge of -.
|
|
|
Hydrogen carbonate?
|
HCO with a subscript of 3 and a charge of -.
|
|
|
Sulfite and Hydrogen sulfite?
|
SO 3 -2.
HSO3 with a charge of - |
|
|
Phospate?
|
PO4 with a charge of -3.
|
|
|
Hydrogen phospate?
|
HPO4 with a -2.
|
|
|
Dihydrogen Phospate?
|
H2PO4 with a -2
|
|
|
Phosphite?
|
PO3 with a -3.
|
|
|
Chronimum?
|
2 and 3
|
|
|
Copper?
|
1 and 2
|
|
|
Gold?
|
Au 1 and 3
|
|
|
Iron
|
Fe 2 and 3
|
|
|
Lead
|
Pb 2 and 4
|
|
|
Tin
|
Sn 2 and 4
|
|
|
Group 1
|
+ Li Na K Rb and Cs
|
|
|
Group 2
|
2+ Mg Ca Sr Ba
|
|
|
Hydroxide?
|
OH-
|
|
|
Nitrate vs Nitrite
|
NO3- vs NO2-
|
|
|
Chlorate vs Chlorite
|
ClO3- vs ClO2-
|
|
|
Carbonate vs Chlorate
|
CO3 with 2- vs ClO3-
|
|
|
Zinc and Cadmium
|
2+
|
|
|
Group 3A and Al
|
3+
|
|
|
Group 5A N and P
|
3-
|
|
|
Group 6 0 and S
|
2-
|
|
|
Halogens
|
Cl F Br I minus charge
|
|
|
Single Replacement
|
A + BC = AC +B
|
|
|
Boyle's Law
|
P1V1=P2V2
Pressure and volume are inversely related when tempature and moles are constant |
|
|
Charles Law
|
V1/T1= V2/T2
Temperature and volume are directly related when pressure and moles are constant |
|
|
Gay-Lussac's Law
|
P1/T1= P2/T2
Pressure and temperature are directly related when moles and volume are constant |
|
|
Combined Law
|
P1V1/T1= P2V2/T2
|
|
|
Gay-Lussac's Law
|
P1/T1=P2/T2
Temperature and pressure are directly related when volume is held constant |
|
|
Combined Law
|
P1V1/T1= P2V2/T2
|
|
|
760 mm Hg
|
1 atm
|
|
|
covalent compound prefixes
|
mono, di, tri, tetra, penta,
|
|
|
Cjemical Change
|
Change in chemical formula, different properties, new substance, color, texture, solid, bubbles etc.
|
|
|
Conbination Reaction
|
A + B =C
|
|
|
Double Replacement
|
AB + CD= AD + BC
|
|
|
Oxidation involves the loss of =
|
LOE Loss of electrons
OIL RIG Oxidation involves loss electrons Reduction involves gain of electrons |
|
|
Oxidation
|
addition of Oxygen
Loss of hydrogen |
|
|
Reduction
|
Loss of oxygen
Gain of hydrogen |
|
|
STP standard pressure
|
1 atm
|
|
|
STP standard temperature
|
0deg celsius or 273 kelvin
|
|
|
STP
|
compare different amounts of gases at different temps and pressures
0 degrees Centigrade and 1 atm or 760 mm Hg |
|
|
Dalton's Law
|
Total Pressure = P1 + P2
|
|
|
PbO2 What charge Pb?
Name? |
Pb 4+
Lead (IV) oxide |
|
|
SnF2 What charge is Sn?
Name? |
Sn 2
Tin (I1) flouride |
|
|
PbO What charge Pb?
|
Pb 2+
Pb (II) |
|
|
K and NO3
|
KNO3 No parenthesis single element
|
|
|
Common covalent compounds
|
CS2 carbon disulfide rayon
Co2 carbon dioxide dry ice carbonation NO nitrogen oxide stabilizer N2O dinitrogen oxide laughing gas |
|
|
Bonding patterns nonmetals in covalent compounds
H |
1 bond
|
|
|
Boron
|
3 bonds
|
|
|
Carbon and Silicon?
|
4 bonds
|
|
|
N and P
|
3 bonds
|
|
|
O and S
|
2 bonds
|
|
|
hexa hepta octa nona deca
|
678910
|
|
|
mono di tri tetra penta
|
12345
|
|
|
ionic or covalent
Na3P CuSO4 SO3 |
Na3P ionic
CuSO4 ionic SO3 covalent |
|
|
760 torr
|
1 atm or 760 mm Hg
|
|
|
STP or Avogadro?
|
convert to L
1 mole of gas is 22.4L at STP of 0 degrees Centigrade and 1atm or 760 mm Hg |
|
|
Avogadro Law
|
V1/N1= V2/N2 when T and P are constant. Refers to the density of the gas. d=m/v grams/mL
|
|
|
Elements exist in Diatomic covalent molecules
|
H, N, O, F, Cl, Br, I
add subscript of 2 |
|
|
Li+ 3P
How many electrons Na+ 11P |
2EGroup 1 Pos charge electron arrange He
10EGroup 1 Pos charge electron arrange Ne |
|
|
N3- 7P
(How many electrons |
10 electrons
Group 5 Negative (3-) charge electron arrange Neon |
|
|
O2- 8P
How many electrons |
10E Group 6 Negative (2-) charge electron arrange Neon
|
|
|
Cation is the
|
positive ion
|
|
|
Anion is the
|
negative ion or the negative polyatomic ion.
|
|
|
Pb 4+ and SO3 2-
|
Pb(SO3)2
Lead (IV) Sulfite |
|
|
Pb4+ and PO4 3-
|
Pb3(PO4)4
Lead (IV) phosphate |
|
|
Al 3+ NO3 -
|
AL(NO3)3
Aluminum nitrate |
|
|
sulfur dioxide
|
preserving fruit, vegetables, bleaching textiles, disinfectant
|
|
|
nonpolar covalent bond
|
similar electronegativity
|
|
|
Smaller atoms have greater
|
electronegativity
|
|
|
Non metals have greater
|
e;ectronegativity values
|
|
|
Electronegativity increases from
|
bottom to top in a group and from right to left in a period
|
|
|
No electronegativity values for
|
Noble gases
|
|
|
Noble gases so stable they don't form compounds.
|
Because they form an octet of valence electrons except for He with 2 electrons in first energy level
|
|
|
Ionic bonding requires the transfer of electrons
|
from metals to nonmetals
|
|
|
Ionic transfer of electrons from metal to nonmetal creates a
|
cation
|
|
|
Cations are
|
positive ions.
|
|
|
Name of cation first, then name of
|
anion
|
|
|
Only 1 ion
|
silver, cadmium, and zinc
Au, Cd, and Zn |
|
|
Iron (III) oxide
|
Fe2O3
|
|
|
Barium Flouride
|
BaF2
|
|
|
Tin (IV) chloride
|
SnCl4
|
|
|
Atoms of nonmetals have high ionization energies and do not easily loose electrons. Instead, they
|
share electrons for stability
|
|
|
If atoms share electrons, they form
|
molecules
|
|
|
SnF2
|
Sn2+ and F-
Tin (II) flouride |
|
|
Cu2O
|
Cu + and O2
Copper (I) oxide |
|
|
FeSO4
|
Fe2+ and SO4 2-
Iron (II) Sulfate |
|
|
If first element metal
|
Compound is ionic
|
|
|
If first element is nonmetal
|
Compound covalent
|
|
|
More than one positive ion
|
Roman numeral
|
|
|
More than one positive ion
|
Roman numeral
|
|
|
More than one positive ion
|
Roman numeral
|
|
|
More than one positive ion
|
Roman numeral
|
|
|
dintrogen oxide
|
laughing gas
|
|
|
dintrogen oxide
|
laughing gas
|
|
|
silicon dioxide
|
glass
|
|
|
dintrogen oxide
|
laughing gas
|
|
|
silicon dioxide
|
glass
|
|
|
dintrogen oxide
|
laughing gas
|
|
|
silicon dioxide
|
glass
|
|
|
sulfur hexaflouride
|
electrical circuits
|
|
|
silicon dioxide
|
glass
|
|
|
sulfur hexaflouride
|
electrical circuits
|
|
|
H how many bonds
|
one
|
|
|
H how many bonds
|
1
|
|
|
sulfur hexaflouride
|
electrical circuits
|
|
|
sulfur hexaflouride
|
electrical circuits
|
|
|
H how many bonds
|
one
|
|
|
H how many bonds
|
1
|
|
|
How many bonds Hydrogen?
|
ONE
|
|
|
How many bonds boron?
|
THREE
|
|
|
How many bonds Carbon and Si?
|
four
|
|
|
How many bonds H2?
|
one
|
|
|
How many bonds C?
|
four
|
|
|
How many bonds N and P?
|
three
|
|
|
How many bonds O and S?
|
two
|
|
|
How many bonds halogens?
|
One
|
|
|
How many bonds H?
|
one bond
|
|
|
what is a double bond?
|
When 2 pairs of electrons are shared
|
|
|
What is a triple bond?
|
When 3 pairs of electrons are shared
|
|
|
How many bonds C and Si?
|
Four bonds
|
|
|
How many bonds N and P?
|
Three bonds
|
|
|
Which atoms are most likely to form multiple bonds?
|
CONS
carbon, oxygen, nitrogen, and sulfur |
|
|
Which atoms are not likely to form multiple bonds?
|
Hydrogen and halogens
|
|
|
How many bonds do O and S form?
|
2 bonds
|
|
|
How many bonds do the halogens form?
|
one bond
|
|
|
less than .4
|
nonpolar covalent
|
|
|
More than .4
|
Polar covalent
|
|
|
More than 1.8
|
ionic
|
|
|
An example of gas in gas
and what is the solute and solvent |
Air is gas in gas. Solute is oxygen and solvent is nitrogen
|
|
|
An example of gas in liquid
|
Soda water and the solute is CO2 and the solvent is H2O
|
|
|
Another gas in liquid
|
Household ammonia
Solute is ammonia and solvent is H2O |
|
|
Liquid in liquid
|
Vinegar
Solute is acetic acid and solvent is H2O |
|
|
Solid in liquid
|
Seaweed
Solute is NaCl and solvent is H2O |
|
|
Solid in liquid
|
Tincture of Iodine
Solute is iodine solid and liquid is alcohol |
|
|
Liquid in solid
|
Dental Analgam
Solute is liquid mecury and solvent is H2O |
|
|
Solid in solid
|
Brass
Solute is Zinc solid and solvent is Copper solid. |
|
|
Solid in solid
|
Steel
Solute is Carbon solid and solvent is Iron solid |
|
|
Solute is dispersed how in solvent
|
uniformly
|
|
|
Solution is a ____ mixture
|
homogenous
|
|
|
The solute and solvent _______ react with each other.
|
do not
|
|
|
Solute is the -------- quantity and the solvent is the ______quantity.
|
smaller, larger
|
|
|
Solutes and solvents may be solids, --------, and liquids.
|
Gases
|
|
|
Hydrogen bonds occurr when a partially positive H is attracted to the strongly electronegative __________
|
O, N, or F molecules
|
|
|
Hydrogen bonds are much _____ than covalent or ionic bonds
|
weaker
|
|
|
Hydrogen bonding plays an important role in
|
Water, proteins, carbohydrates, and DNA
|
|
|
Ionic compounds undergo________
|
hydration
|
|
|
Like dissolves ______
|
like
|
|
|
Liquids and solids require an attraction between the particles for a _____ to occur.
|
solution
|
|
|
______ and _______ substances will dissolve in water.
|
ionic and polar
|
|
|
Nonpolar dissolves in _______
|
nonpolar
|
|
|
Solutes called ________ dissolve in water, they separate into ions which are able to conduct electricity.
|
electrolytes
|
|
|
Nonelectrolytes are ______ that do not separate into ions.
|
solutes
|
|
|
A strong ----------is a compound that dissociates in water. The _____ separate from the solution and conduct electricity
|
electrolyte, ions
|
|
|
In dissociation the ________ must balance.
|
electrical charges
|
|
|
A weak ______ dissolves in H2O mostly as whole_____ and a few ions.
|
electrolyte, molecules
|
|
|
A _____ is a compound that dissolves in water as molecules.
|
nonelectrolyte
|
|
|
HF is a weak ______
|
electrolyte
|
|
|
Solutions of strong electrolytes contain only
|
ions
|
|
|
Solutions of _________
contain a few ions and mostly molecules |
weak electrolytes
|
|
|
An equivelant is the amount of that ion equal to one mole of positive or negative _______
|
charge.
|
|
|
Na + or CL-
|
one equivalent regardless of the charge
|
|
|
Solubiltiy is the _____ of solvent that can dissolve in a given solvent.
|
amount
|
|
|
Factors affecting solubility include: type of solute, type of solvent, and _________.
|
termperature
|
|
|
An unsaturated solution does not contain the
|
maximum amount of solute.
|
|
|
A _________ solution contains all the solute that can dissolve.
|
saturated
|
|
|
Solutions usually contain more dissolved solute at higher ________.
|
temperatures
|
|
|
When a saturated solution is carefully cooled, it becomes a _______ cause it contains more solute than the solubility allows.
|
supersaturated
|
|
|
A supersaturated solution is ________
|
Unstable
|
|
|
The solubility of gas in water ______ as temperature ______
|
decreases, increases
|
|
|
The solubility of gas in liquid is directly related to the pressure of that gas above liquid.
|
Henry's Law
|
|
|
The amount of the solute dissolved in a given amount of solution.
|
Concentration
|
|
|
5g Glucose and 25g H2O
What is the solute? |
Solute is glucose and solvent is H2)
|
|
|
Nonpolar substance needs _______ solvent
|
nonpolar
|
|
|
C or H or N2 only
|
nonpolar
|
|
|
C6H6 benzene
|
nonpolar
|
|
|
CH3CH2OH alcohol
|
polarity can't dissovle in H20
|
|
|
Hydrogen bond force unique and very strong, not in structure but in
|
molecules
|
|
|
Hydrogen bonds in sugars and ____________
|
amino acids
|
|
|
Need __________ for hydrogen bonds
|
N, O, or F
|
|
|
Polyatomic atoms form ions and dissolve in
|
water
|
|
|
Nonelectrolytes
|
Sucrose, glucose, and alcohol
|
|
|
I EQ= 1000
|
mEq
|
|
|
The concentration of a solution is
|
The amount of solute/the amoutn of solution x 100%
|
|
|
Volume per centage =
|
Volume of the solute/volume of the solution X 100%
|
|
|
m/v% =
|
grams of solute/mL solution X
100% |
|
|
To find mass of solute
|
Use m/v%
|
|
|
A solution is a ______ of 2 or more substances in a single phase.
|
mixture
|
|
|
The _____ is the major component in the solution. The material the solute is dissolved into.
|
solvent
|
|
|
The maximum amount that can be dissolved into a particular solvent to form a stable solution at specified temperature
|
solubility
|
|
|
Substances that can dissolve in any proportion, so that it is difficult to tell which is the solvent or solute.
|
Miscible
|
|
|
dissociate completely (or nearly so) into ions.
|
strong electrolytes
|
|
|
Partial dissociation
|
Weak electrolytes
|
|
|
No dissociation
|
Nonelectolytes
|
|
|
Some compounds dissolve in water but do not conduct electricity. They are called
|
nonelectrolytes.
Examples: sugar ethanol ethylene glycol |
|
|
Carry messages to and from the brain as electrical signals
Maintain cellular function with the correct concentrations electrolytes |
electrolytes
|
|
|
Molarity=
|
concentration
|
|
|
PROBLEM: Dissolve 5.00 g of NiCl2•6 H2O in enough water to make 250 mL of solution. Calculate the Molarity.
|
M= 5g/.250 liters
5 g x 1mole/237.7 grams= .02 moles .02moles/.250 lites= .0841 M |
|
|
What mass of oxalic acid, H2C2O4, is
required to make 250. mL of a 0.0500 M solution? |
.250 liters X .05M// 1 liters= .0125 moles
.0125 moles x 90 grams/mole= 1.13 grams |
|
|
How many grams of NaOH are required to prepare 400. mL of 3.0 M NaOH solution?
|
.4 liters x 3 mol/liter x 40grams/mole= 48 grams
|
|
|
Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g of H2O. Calculate molality and % by mass of ethylene glycol.
|
concentration or molality =
1 mole glycol/.25kg H2O % glycol= 62 g / 62 g + 250g x 100% |
|
|
m/m m/v v/v
|
grams of solute/ grams of solvent
grams of solute/ 100 mL mL of solute/ mL of solvent |
|
|
A solution contains 15 g Na2CO3 and 235 g of H2O? What is the mass % of the solution?
|
15/235+15 X 100 = 6.38%
|
|
|
How many grams of NaCl are needed to prepare 250 g of a 10.0% (by mass) NaCl solution?
|
250 g x 10 g/100g solution
25 g NaCL |
|
|
Problem: You have available 12.0 M HCl (conc. HCl) and wish to prepare 0.500 L of 0.750 M HCl for use in an experiment. How do you prepare such a solution?
Cconc Vconc = Cdil Vdil |
c1v1=c2v2
c1= 12M HCL v1=? c2= .75M v2= .5 liters v1= c2v2/c1= .75X X .5/12= .03125= 31.25 ml |
|
|
PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do?
|
v1= .05 liters
c1= 3M v2+ ? c2= .5M v1c1=v2c2 v2= .05 X 3/ 5M =.3 or 300 mL |
|
|
You have a stock bottle of hydrochloric acid, which is 12.1 M. You need 400 mL of 0.10 M HCl. How much of the acid and how much water will you need?
|
12.1C1= 12.1M
V1= ? C2= .10 M V2= .400 L .1X .400/ 12 =.033 liters |
|
|
Colloids
|
Large molecules such as proteins or groups of molecules or ions. Homoegeneous mixtures that do not separate or settle out.They can pass through filters, but not semipermeable membrane
|
|
|
Colloidal particles are small enought to pass through filters, but too----- to pass through semipermeable membranes
|
Large
|
|
|
Suspensions are heterogenous, nonuniform mixtures that are different from solutions or ______
|
colloids
|
|
|
The particles of a suspension are so ---------- that they can be seen with the naked eye.
|
large
|
|
|
Particles do not settle
|
Solutions and colloids, but particles in suspensions settle rapidly.
|
|
|
Particles do not settle
|
Colloids and solutions
|
|
|
Particles settle rapidly
|
Suspensions
|
|
|
Particles cannot be separated by filters or semipermeable membranes
|
Solutions
|
|
|
Particles can be separated by semipermeable membranes but not by filters
|
Colloid
|
|
|
Particles can be separated by filters
|
Suspension
|
|
|
Colloids
|
Larger molecules or goups of molecules or ions.
|
|
|
Suspension
|
Very large particles. May be visible.
|
|
|
Solution
|
Small particles, such as ions, atoms, or small molecules.
|
|
|
On adding a solute to a solvent, the properties of the solvent are modified.
Vapor pressure decreases Melting point decreases Boiling point increases Osmosis is possible (osmotic pressure) . |
COLLIGATIVE PROPERTIES.
They depend only on the NUMBER of solute particles relative to solvent particles, not on the KIND of solute particles. |
|
|
Osmosis
|
Moving from lower to higher concentration
|
|
|
Osmotic pressure
|
Prevents the flow of additonal water into a concentrated solution.
|
|
|
Acids
|
Have a sour taste. Vinegar is a solution of acetic acid. Citrus
fruits contain citric acid. |
|
|
Acids react with certain _____
to produce hydrogen gas. |
metals
|
|
|
Acids React with ---------------to produce carbon
dioxide gas |
carbonates and bicarbonates
|
|
|
Bases have a _______ taste.
|
bitter
|
|
|
Bases feel ________
|
slippery. Many soaps contain bases.
|
|
|
Acids --------- metals
|
corrode
|
|
|
Acids are ______
|
electrolytes
|
|
|
Acids react with _____ to form salt and water.
|
bases
|
|
|
Acids have a ph of _____
|
<7
|
|
|
Acids Turns blue litmus paper to Turns blue litmus paper to
|
red “Blue to Red A-CID
|
|
|
Common acids include
|
Hydrochoric acid, HCL
Hydrobromic acid HBr Nitric acid HNO3 Nitrous acid HNO2 Sulfuric acid H2SO4 |
|
|
Bases produce ----- ions in water.
|
OH
|
|
|
Bases taste _______
|
bitter and chalky
|
|
|
Bases react with acids to form
|
salt and water
|
|
|
Bases have Ph
|
>7
|
|
|
Bases turns red litmus paper to
|
blue “Basic Blue”
|
|
|
Bases feel soapy or ______
|
slippery
|
|
|
Common bases include
|
NaOH, sodium hydroxide, lye
KOH, potassium hydroxide, liquid soap Ba(OH)2 barium hydroxidestabilizer for plastics Mg(OH)2, magnesium hydroxide “MOM” Milk of magnesia |
|
|
HCL
|
metal cleaning food preparation ore refining stomach acid
|
|
|
Arrhenius defintion of acids
Acid: |
Substance that, when dissolved in water, increases the concentration of hydrogen ions (protons, H+
|
|
|
Arrhenius definiton of bases
|
Base: Substance that, when dissolved in water, increases the concentration of hydroxide ions.
|
|
|
Arrhenius acid is a substance that produces
|
is a substance that produces H+ (H3O+) in water
|
|
|
Arrhemius base
|
is a substance that produces H+ (H3O+) in water
|
|
|
The Arrhenius definition has many limitations:
-- |
It only works in aqueous solutions, but acid-like behavior can occur in other solvents.
|
|
|
The Arrhenius definition has many limitations
|
Many species act as bases without containing OH ions
(such as ammonia, NH3). |
|
|
a more general definition of acids and bases was developed byJohannes Brønsted and Thomas Lowry (1923):
|
Definition #2: Brønsted – Lowry
Acids – proton donor Bases – proton acceptor A “proton” is really just a hydrogen atom that has lost it’s electron! |
|
|
A Brønsted–Lowry acid…
…must have a removable (acidic) proton.a removable (acidic) proton. A Brønsted–Lowry base… …must have a pair of nonbonding electrons. NH3, H2O |
a removable (acidic) proton.
a removable (acidic) proton. |
|
|
The Brønsted definition means NH3 is a -------- in water — and water is itself an ACID
|
BASE
|
|
|
m/m% =
|
mass of solute/mass of solute + mass of solvent X100
|
|
|
Weak electrolytes leave ions and original ______
|
Products (moles)
|
|
|
Strong electrolytes leave
|
2 ions
|
|
|
m/v % =
|
grams/mL
|
|
|
Dilution formula
|
C1V1= C2V2
|
|
|
Molarity after dilution
|
M1V1=M2V2
|
|
|
A measure of the amount of solute that is dissolved in a specific amount of solution
|
Concentration
|
|
|
A process by which a solvent is added to a solution to increase the volume and to dilute or decrease the concentration of the solute
|
dilution
|
|
|
A solution that has a higher particle concentration and higher osmotic pressure than the cells of the body
|
hypertonic solution
|
|
|
A solution that has a lower prarticle concentration and lower osmotic pressure than the cells of the body
|
hypotonic solution
|
|
|
m/m%
|
grams/grams in solution pl;us solvent x 100 or grams of solute in 100 grams
|
|
|
mass/volume %
|
the grams of solute in exactly 100 mL of solution
|
|
|
Molarity
|
the number of moles of solute in exactly one liter of solution
|
|
|
Suspensions
|
A solute in which the solute particles are large enough and heavy enough to to settle out and be retained by both filters and seimi permeable membranes
|
|
|
Volume %
|
% concentration that relates the volume of the concentration to exactl;y 100 mL of the solution
|
|
|
Calculate the molarity of 30 g NaOH in 350 mL of solutioo?
|
30.0 g-NaOH x I mole NaOH = 2 l4 M NaOH
0.350 L solution 40.0 g-NaOH= 2.14 |
|
|
Write an equation for the dissociation of CaOH2?
|
Ca 3+ and OH
|
|
|
A Bronstead-Lowry acid is a proton
|
donor
|
|
|
A Bronstead-Lowry base is a proton
|
acceptor
|
|
|
Acids and bases are both
|
electrolytes
|
|
|
In Arrhenius, acids produce H+, but in _______ they dontate H+
|
Bronstead-Lowry
|
|
|
In Arrhenius, bases provide OH-, but in Bronstead-Lowry they _____ H+
|
accpt
|
|
|
Acids may sting and bases may
|
feel sapy or slippery
|
|
|
Acids turn blue litmus paper red and bases turn litmum paper
|
blue
|
|
|
In phenophtilatlein, acide turn----------------- and bases turn pink
|
colorless
|
|
|
Bronstead-lowry- acids donate H+ but arrenhius produce
|
H+
|
|
|
In Bronstead-Lowry bases accept-----------, but in Arrenhius produce OH-
|
H+
|
|
|
Neutralization involves the neurtalization of both
|
acids and bases
|
|
|
An equivalent, Eq is
|
The amount of ion equal to one mole of positive or negative electrical charge
|
|
|
A strong electrolyte completely disssociates which means
|
it contains only ions in the solution
|
|
|
A weak electrolyte partially dissociates which means
|
it contains molecules mostly and a few ions
|
|
|
A nonelectrolyte contains
|
molecules only.
|
|
|
Strong electrolytes conduct
|
electricity. Weak electrolytes do so poorly and nonelectrolytes not at all.
|
|
|
The number of equivalents in CO3 2- is
|
6
|
|
|
An _____ solution does not contain the maximum solute and the solute will readily _____when added to the solvent
|
unsaturated, dissolve
|
|
|
A solution that contains all of the solute that can dissolve is a _______
|
saturated solution
|
|
|
The rate of reaction that dissolves the saturated solution is equal to the rate of recrystallization.
|
No further change in the amount of dissolved solute possible
|
|
|
The amountof solute dissolved in a certain amount of solution is called the
|
concentration
|
|
|
Concentration= amount of solute/__________
|
amount of solution
|
|
|
% m/m = mass of solute in g /mass of solute in g and the -----------------------------
|
mass of solvent in g X 100%
|
|
|
%v/v = volume of _______/ volume of solution x 100% or the volume of solute in 100mL of solution
|
solute
|
|
|
%m/v= weight or volume calculated by dividing grams of solute by -------------and x 100%
|
volume of solution
|
|
|
Acids react with ______ to produce H2
|
metals
|
|
|
Acids react with _______ and_______ to produce CO2 and water
|
carbonates and bicarbonates
|
|
|
H2SO4 and H2CO3 are diprotic _________
|
They produce 2H+ 2 protons
|
|
|
H3PO4, phosphoric acid is a ___________ acid
|
triprotic
|
|
|
HC2H3O2 is acetic acid which is also called
|
Vinegar, a weak electrolyte.
|
|
|
NH3 does not produce ______
but is a weak. In Arrenhius, NH3 is _____________ |
OH- but is weak base
In Bronstead Lowry can an acid or base |
|
|
A proton is really just a -------------------------that has lost its ----------------------
|
hydrogen atom, electron
|
|
|
proton donor -----------------acidic proton
|
removable
|
|
|
Base H+ acceptor
|
pair of nonbonding electrons
|
|
|
NH3 is amphiprotic
|
can be both an acid and a base
|
|
|
A strong acid is a _______
and gives a ___________ |
good proton donor
weak base |
|
|
ph can have ___________ but not negative number
|
fraction
|
|
|
In ___________ reactions, an acid and a base produce
|
water and a salt
|
|
|
When an acid reacts with a metal, H2 and a -------- are produced.
|
salt
|
|
|
The reaction of an acid with a -------------- or ------------ produces carbon dioxide, salt, and H20.
|
carbonate, bicarbonate
|
|
|
Neutralization means that an ---------------- reacts with a ------------------to produce salt and water.
|
acid, base
|
|
|
A buffer contains either a weak acid and its salt or a weak _____ and its salt
|
base
|
|
|
In titration, an acid is neutralized with a known amount of ------------
|
base
|
