Chapter 9: Introduction to Solutions and Aqueous Reactions Flashcards

1
Q

solution

A

A homogeneous mixture of two substances such as salt and water.

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2
Q

solvent

A

The major component of the mixture.

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3
Q

solute

A

The minor component of the mixture.

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4
Q

aqueous solution

A

One in which water acts as the solvent.

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5
Q

dilute solution

A

One that contains a small amount of solute relative to the solvent.

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6
Q

concentrated solution

A

One that contains a large amount of solute relative to the solvent.

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7
Q

molarity

A

The amount of solute (in moles) divided by the volume of solution (in liters). A common way to express solution concentration.

M = mol/L

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8
Q

stock solution

A

Solutions in concentrated forms.

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9
Q

Solution Dilution

A

M1V1= M2V2

mol1 = mol2

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10
Q

electrolytes

A

Substances that dissolve in water to form solutions that conduct electricity.

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11
Q

strong electrolytes

A

Substances such as sodium chloride that completely dissociate into ions when they dissolve in water.

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12
Q

nonelectrolytes

A

Compounds such as sugar that do not dissociate into ions when dissolved in water. It does not conduct electricity.

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13
Q

Acids

A

Molecular compunds that ionize into H+when it dossolves in water.

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14
Q

strong acid

A

One that completely ionizes in solution and are strong electrolytes. Such as HCl.

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15
Q

weak acids

A

Do not completely ionize in water. Composed mostly of the nonionized acid – only a small percentage of the acid molecules ionize.

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16
Q

weak electrolytes

A

Weak acids. Conducts electricity weakly.

17
Q

soluble

A

Compound that dissolves in water.

Compounds containing the following ions are generally soluble

  1. Li+, Na+, K+, and NH4+
    • No exceptions
  2. NO3- and C2H3O2-
    • ​No exceptions
  3. Cl-, Br-, and I-
    • ​When these ions pair with Ag+, Hg22+ or Pb2+, the resulting compounds are insoluble.
  4. SO42-
    • ​​When SO42- pairs with Sr2+, Ba2+, Pb2+, Ag+, or Ca2+, the resulting compound is insoluble.
18
Q

insoluble

A

Compound that does not dissolve in water.

Compounds containing the following ions are generally insoluble.

  1. OH- and S2-
    • ​​When these ions pair with Li+, Na+, K+, or NH4+, the resulting compounds are soluble.
    • When S2- pairs with Ca2+, Sr2+, or Ba2+, the resulting compound is soluble.
    • When OH- pairs with Ca2+, Sr2+, or Ba2+, the resulting compound is slightly soluble.
  2. CO32- and PO43-
    • ​​When these ions pair with Li+, Na+, K+, or NH4+, the resulting compounds are soluble.
19
Q

precipitation reaction

A

A reaction in which a solid forms upon the mixing of two solutions.

20
Q

precipitate

A

A solid, insoluble ionic compond that forms in, and separates from, a solution.

21
Q

molecular equation

A

An equation that shows the complete neutral formulas for each compound in the reaction as if they existed as molecules.

22
Q

complete ionic equations

A

Equation that lists all of the ions present as either reactants or products in a chemical reactions.

23
Q

spectator ions

A

Ions that do not participate in the reaction. Ions in the complete ionic equation that appear unchanged on both sides of the equation.

24
Q

net ionic equations

A

Equations that show only the species that actually change during the reaction. Omit spectator ions.

25
acid base reaction
An acid reacts with a base and the two neutralize each other, producing water (or in some cases a weak electrolyte). Also called neutralization reaction.
26
Arrhenius definition
The definitions of an acid as a substance that produces H+ ions in aqueous solution and a base as a substance that produces OH- ions in aqueous solution.
27
hydronium ions
H3O+, the ion formed from the association of a water molecule with an H+ ion donated by an acid.
28
polyprotic acids
Acids that contain more than one ionizable proton and release them sequentially.
29
Diprotic acid
An acid that contains two ionizable protons.
30
Acids
Hydrochloric acid - HCl Hydrobromic acid - HBr Hydroiodic acid - HI Nitric acid - HNO3 Sulfuric acid - H2SO4 Perchloric acid - HClO4 Acetic acid - HC2H3O2 (weak acid) Hydrofluoric acid - HF (weak acid)
31
bases
Sodium hydroxide - NaOH Lithium hydroxide - LiOH Potassium hydroxide - KOH Calcium hydroxide - Ca(OH)2 Barium hydroxide - Ba(OH)2 Ammonia - NH3 (weak) (Ammonia does not contain OH- but it produces it in a reaction with water that occurs only to a small extent.)
32
Binary acids
Composed of hydrogen and a nonmetal. Hydro + base name of nonmetal + -ic + acid HCl - hydrochloric acid
33
oxyacids
Contain hydrogen and an oxyanion (an anion containing an nonmetal and oxygen). (polyatomic) oxyanions ending with _-ate_: base name of oxyanion + -ic + acid oxyanions ending with _-ite_: base name of oxyanion + -ous + acid * HNO3 (aq)- Nitric acid* * H2SO3 (aq) - sulfurous acid*
34
salt
Ionic compound that usually remains dissolved in the solution.
35
titration
A substance in a solution of known concentration is reacted with another substance in a solution of unknown concentration.
36
Equivalence point