Unit 12 (Solutions Acids And Bases) Chapter 12 (Sections

unit 12 (solutions, acids and bases) chapter 12 (sections 1-3), chapter 13 (section 2), chapter 14 (section 1), and chapter 15 (section 1) s

Unit 12 (Solutions, Acids and Bases)
Chapter 12 (Sections 1-3), Chapter 13 (Section 2), Chapter 14 (Section
1), and Chapter 15 (Section 1) Study Guide
1.
A ___mixture________________ is a combination of two or more
substances that are not chemically combined and can be separated
by physical means.
2.
What type of mixture has components in a nonuniform arrangement?
__heterogeneous_____ uniform arrangement? __homogeneous_____________________
3.
What is another name for a homogeneous mixture of a substance in a
single phase? ___solution_________________
4.
Sugar dissolved in water is an example of what type of
solute-solvent combination? __solid-liquid______________________
5.
Ethanol dissolved in gasoline is an example of what type of
solute-solvent combination? __liquid-liquid_____________________
6.
CO2 gas dissolved in Coca-cola is an example of what type of
solute-solvent combination? __gas-liquid______________________
7.
Match the following:
8.
amalgam _aqueous___________ solution with water as solvent
9.
electrolyte _electrolyte___________ solutions in which the solute
dissolves to give ions
10.
tincture _alloy___________ solid solution of two or more metals
11.
aqueous _tincture___________ solutions in which alcohol is the
solvent
12.
alloy amalgam ___________ specific alloys in which one of the
metals is mercury
13.
If the particles in a solvent are so large that they settle out
unless the mixture is constantly stirred or agitated, the mixture
is called a ___suspension_______________.
14.
Particles that are intermediate in size between those in solutions
and suspensions form mixtures known as __colloidal_____________
dispersions, or _colloids_______________.
15.
The Tyndall effect is a property that can be used to distinguish
between a __solution_______ and a _colloid________________.
16.
A substance that dissolves in water to give a solution that
conducts electric current is called an ___electrolyte_________________.
Give an example.
17.
A substance that dissolves in water to give a solution that does
not conduct electric current is called an __nonelectrolyte___________________.
Give an example.
18.
What three factors affect the rate of dissolving of a solid in a
liquid? ___increasing the surface area of the solute______agitating
a solution_____heating a solvent
_______________________________________________________________________________________________________________________________
19.
A solution that contains the maximum amount of dissolved solute is
described as a _saturated__________________ solution.
20.
A solution that contains less solute than a saturated solution
under the existing conditions is an __unsaturated_______________
solution.
21.
What type of solution contains more solute than a saturated
solution under the same conditions? __supersaturated__________________
22.
_Like___________ dissolves __like________ is a general rule for
predicting whether one substance will form a solution with another
and depends on _type of bonding____________, _polarity or
nonpolarity_______________, and __intermolecular _________________
forces between molecules.
23.
Liquid solutes and solvents that are not soluble with each other
are __immiscible__________ (oil and water) and those that are
soluble are __miscible____________ (vinegar and water).
24.
What particles interact during the dissolving process? __solute
and solvent_____________
25.
___Increases________________ in pressure __increases_________ gas
solubility in liquids.
26.
_Emulsifying agents____________________ are agents that have both
polar and nonpolar ends to join the two unlike molecules together.
27.
What is molarity? _number of moles of solute in one liter of
solution__________________
28.
How many moles of H2SO4 are in 2.50 L of a 4.25 M aqueous
solution? ____10.6 mol_____
29.
What is the molarity of a solution prepared by dissolving 37.94 g
of KOH in some water and then diluting the solution to a volume of
500.00 mL? (MM of KOH = 56.11 g/mol) ______1.352 M_____________________
30.
What is molality? _concentration of a solution expressed in moles
of solute per kilogram of solvent________________
31.
Determine the molal concencentration of a solution containing 81.3
g of ethylene glycol (62.08 g/mol) dissolved in 166 g of water. _7.89
m________________
32.
What effect would adding salt to water have on water’s boiling
point? _elevates__________
33.
What effect would adding sugar to water have on water’s freezing
point? __depresses____
34.
What are these properties called? _colligative properties__________________
________
35.
__Acids_____________ taste sour and __bases__________ taste
bitter.
36.
__Basic_____________ solutions feel slippery.
37.
Acids react with __bases_____________ to produce salt and water.
38.
An _Arrhenius_________________ acid is a chemical compound that
increases the concentration of hydrogen ions, H+, in aqueous
solution.
39.
An Arrhenius base is a substance that increases the concentration
of __hydroxide_____________ ions, _OH-____, in aqueous solution.
40.
Look over the notes for common industrial acids and their uses.
41.
What is an indicator? _compounds whose colors are sensitive to pH___________________
42.
A _Bronsted-Lowry______________________ acid is a molecule or ion
that is a __proton____________ (H+) donor. A __Lewis_________________
acid is an atom, ion, or molecule that accepts an __electron_______________pair
to form a covalent bond.
43.
A _Bronsted-Lowry___________________ base is a molecule or ion
that is a __proton_____________ acceptor. A ____Lewis__________________
base is an atom, ion, or molecule that donates an _electron__________
pair to form a covalent bond.
44.
Any solution in which [H3O+] is greater than [OH-] is __acidic________________
and any solution in which [H3O+] is less than [OH-] is ___basic________________.
45.
The pH scale rages from ___0________ to __14________.
46.
An acidic solution would have a pH __less_______ than 7 and a
basic solution would have a pH _greater__________ than 7.
47.
pH + pOH = _14________.
48.
What is the formula for calculating pH? _-log[H3O+]________________
pOH? __ -log[OH-]_______________
49.
What is the pH of a solution with a [H+] of 8.26 x 10-5? ___4.08_____________________