Term
| Molarity (State general equation) |
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Definition
The number of moles of solute in a liter of solution.
M=n/L
M= molarity;
n = moles;
L = liters |
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Term
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Definition
The substance dissolved in another (solvent).
Salt is the solute in salt water. |
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Term
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Definition
A substance, usually a liquid, into which another substance (solute) is dissolved.
Water is the solvent in iced tea. |
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Term
| Solution (Give an example) |
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Definition
A liquid, gas, or solid phase containing two or more components uniformly dispersed.
e.g. air, coffee, saltwater |
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Term
| Calculate the molarity when 5 moles of NaCl is dissolved in 25 liters of water. |
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Definition
M = n/L
M = 5/25
M = 0.2M |
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Term
| Calculate the moles of NaCl in 5 liters of a 2 molar solution. |
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Definition
M = n/L
2 M = n/5 L
10 = moles of NaCl |
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Term
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Definition
Non-metallic oxides which, when reacted with water, form acid solutions.
e.g. CO2 + H2O → H2CO3
SO3 + H2O → H2SO4 |
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Term
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Definition
Metallic oxides which, when reacted with water, form basic solutions.
e.g. Na2O + H2O → 2 NaOH
CaO + H2O → Ca(OH)2 |
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Term
| Why is water a good solvent for ionic compounds? |
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Definition
| Due to hydrogen bonding, water is polar. The negatively charged oxygen attracts a cation, and the positively charged hydrogen, an anion. |
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Term
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Definition
| A curve for a given substance which shows how much dissolves in a given amount of solvent at different temperatures. |
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Term
| How do temperature and pressure affect the solubility of a solid? |
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Definition
| Solubility usually increases with increasing temperature. Pressure has little effect. |
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Term
| How do temperature and pressure affect the solubility of a gas? |
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Definition
| Solubility usually decreases with increasing temperature. Solubility in creases in direct proportion to an increase in pressure. |
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Term
| Which three factors affect the rate of solubility? |
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Definition
pulverizing
stirring
heating |
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Term
| What is a general rule for solubilities of polar and nonpolar compounds? |
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Definition
"Like dissolves like." Ionic and polar solvents dissolve ionic, polar solutes.
e.g. Water dissolves salt.
Nonpolar solvents dissolve nonpolar solutes.
e.g. Acetone dissolves gasoline and cooing oil. |
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Term
| Solubility of nitrates, acetates, and chlorates in water. |
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Definition
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Term
| Solubility of Na, K, and (NH4)+ compounds in water. |
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Definition
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Term
| Solubility of chlorides in water. |
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Definition
| All chlorides are soluble, except Ag, Hg, Pb. |
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Term
| Solubility of sulfates in water. |
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Definition
| All sulfates are soluble, except Pb, Ba, Sr, Ca |
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Term
| Solubility of carbonates, phosphates, sulfides, and silicates in water. |
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Definition
| All insoluble, except Na, K, (NH4)+ |
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Term
| Solubility of hydroxides (OH-) in water. |
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Definition
| All insoluble except Na, K, (NH4)+, Ca, Ba, Sr |
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Term
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Definition
| A dissolved ion which is surrounded by water molecules. It is attracted electrostatically to the polar water molecule. |
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Term
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Definition
Two liquids which dissolve in each other.
e.g. water and alcohol |
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Term
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Definition
Two liquids which do not dissolve in each other.
e.g. oil and vinegar |
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Term
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Definition
| When light is shone through a colloid, the individual zig-zag paths of the particles in the dispersing medium can be observed; like smoke in a dark theater. |
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Term
| Basic facts about Solutions |
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Definition
particle size less than 1 nanometer.
Clear (may be colored)
)articles don't settle
Can pass through membranes
Particles not visible |
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Term
| Basic facts about colloids |
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Definition
particles measure 1-1000 nanometers
Particles don't pass through a membrane
Show Brownian movement and the Tyndall effect
Particles don't settle
Clear
Pass through filter paper |
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Term
| Basic facts about Suspensions |
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Definition
No Brownian movement
Don't pass through filter paper or a memebrane
Cloudy, but particles settle on standing
Particles visible with microscope or eye |
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Term
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Definition
| Small amount of solute in the solvent. |
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Term
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Definition
| Large amount of solute in the solvent. |
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Term
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Definition
| In the presence of undissolved solute, the solution is holding all the solute possible at that temperature. |
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Term
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Definition
| More solute can be dissolved in the solvent at that temperature. |
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Term
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Definition
| Created by cooling a saturated solution. If cooled slowly, the solute stays dissolved. The amount of solute in the solution is greater than the solubility at a given temperature. |
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Term
| Write the equation for percent concentration of a solute in a solution (mass/mass). |
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Definition
| % concentration = (gsolute/gsolution)(100%) |
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Term
| HOw many grams of NaCl are required to prepare 500 g of a 5% solution? |
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Definition
| % Conc. = (gNaCl/gsolution)(100%) 5% = (x/500 g)(100%) 25 g NaCl = x |
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Term
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Definition
The number of moles of solute dissolved in 1 kg of solvent.
molality (m) = moles solute/kg solvent |
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Term
| Calculate the molality of 10 moles of H2SO4 dissolved in 4 kg of water. |
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Definition
| molality = moles solute/kg solvent = 10/4 = 2.5 molal |
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Term
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Definition
| The amount of substance which reacts with or displaces one mole of H+ ions. |
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Term
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Definition
| The number of gram-equivalent weights in a liter of solution. |
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Term
| Wire the equation for molarity changes related to diluting a solution. |
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Definition
(M1)(V1)= (M2)(V2)
M = molarity
V = Volume |
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Term
| 10 liters of a 6 molar solution is diluted to 3 molar. What is the final volume? |
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Definition
(M1)(V1)= (M2)(V2)
(6)(10) = (3) (V2)
V2 = 20 L |
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Term
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Definition
| Properties of solutions that depend primarily on the concentration of solute and not on the type of particle. |
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Term
| List three basic colligative properties of solutions. |
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Definition
vapor pressure lowering
boiling point elevation
freezing point depression |
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Term
| In H2O solutions how many °C is the freezing point depressed for each molal of solute? |
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Definition
| 1.86 °C for each molal of particles of solute |
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Term
| In H2O solutions how many °C is the boiling point elevated for each molal of solute? |
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Definition
| 0.51 °C for each molal of particles of solute |
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Term
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Definition
| A crystal that holds a definite proportion of water in its structure |
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Term
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Definition
| In a crystal structure, ions or atoms form a repeating pattern of unit cells. |
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Term
| List six basic types of unit cells which can make up crystal lattices. |
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Definition
Simple cubic
face-centered cubic
body-centered cubic
tetragonal
hexagonal
monoclinic |
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Term
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Definition
Hydrated crystals which lose their water of hydration on exposure to air at room temperature.
e.g. magnesium sulfate |
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Term
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Definition
Hydrated crystals which absorb water from the air and become wet.
e.g. calcium chloride and magnesium chloride |
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Term
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Definition
| A hydrated crystal which loses its water of hydration. The pure salt loses the crystal structure and crumbles to powder |
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Term
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Definition
| The smallest portion of a crystal lattice that is repeated throughout the crystal |
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