Term
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Definition
1. weigh out in grams
2. put it in a flask or beaker
3. dilute it to 1 L (with distilled water) |
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| What is the equation for determining molarity or concentration? |
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Definition
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Term
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Definition
| the concentration of a solution expressed as moles of solute/per liter of solution |
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Definition
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Definition
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Definition
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Definition
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Definition
| contains more than the maximum amt of solute for a given amt of solvent |
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Definition
| contains less than the maximum amt of solute for a given amt of solvent |
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Definition
| contains the maximum amt of solute for a given quantity of solvent |
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Term
| FACTORS WHICH DETERMINE SOLUBILITY? |
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Definition
-stirring or agitation
-temperature increase
-smaller particle size |
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Term
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Definition
The amt of solute that can be dissolved in a given amt of solvent
and
the property of a substance to dissolve in another |
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Definition
| the component of a solution which is dissolved in the other |
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Definition
| The component of a solution which dissolves the other |
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Definition
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Term
ACID/BASE TEST:
PHENOPHTHALEIN |
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Definition
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Term
ACID/BASE TEST:
ELECTROLYTE |
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Definition
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Term
ACID/BASE TEST:
reaction w/ water |
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Definition
a-forms hydronium ion, H3 O+
b-forms hydroxide ion, OH- |
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Term
ACID/BASE TEST:
reaction w/ metals |
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Definition
a-forms metallic salt + H2
b-none |
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Term
ACID/BASE TEST:
reaction w/ carbonates |
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Definition
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Term
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Definition
| the breaking up of an acid or bases into its constituent ions |
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Term
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Definition
-compounds of hydrogen combined w/ a halogen
-or NO3-, SO4--, or CLO4-
-All these exhibit a high rate of dissociation making them good electrolytes |
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Term
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Definition
-compounds of hydrogen combined with CO3--, PO4---, C2H3O2-
-These exhibit a moderate to low rate of dissociation |
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Term
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Definition
-hydroxides of alkali and alkaline earth metals.
-All exhibit a high rate of dissociation making them good electrolytes |
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Term
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Definition
| NH4OH, Al(OH)3, Fe(OH)3. These exhibit a moderate to low rate of dissociation |
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Term
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Definition
| the measurement of the number of H30+ (H+) ions in an acid solution or OH- ions in a basic solution |
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Term
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Definition
| strong acids-->1 2 3<-- 4 5 6 neutral 8 9 10 11 -->12 13 14<--strong bases |
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Term
| In numerical representation, pH is defined as... |
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Definition
| the negative log of the hydronium ion of an acid solution, or the negative log of the hydroxide ion concentration of a basic solution |
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Term
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Definition
| an acid which donates more than 1 hydrogen ion when it dissociates |
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Definition
| a base which donates more than 1 hydroxide ion when ti dissociates |
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Term
ACID-BASE DEFINITIONS:
arrehnius |
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Definition
a-H+ producer
b-OH- producer |
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Term
ACID-BASE DEFINITIONS:
bronstead/lowry |
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Definition
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Term
ACID-BASE DEFINITIONS:
lewis |
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Definition
a-electron pair acceptor
b-electron pair donor |
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Term
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Definition
| a substance which changes color in the presence of an acid or a base |
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Term
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Definition
| the particle formed when a base gains an H+ ion |
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Term
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Definition
| the particle remaining when an acid has donated an H+ ion |
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Term
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Definition
| two substances related by the loss or gain of a single H+ ion |
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Definition
-A solution of weak acid and one of its salts,
-or a weak base and one of ts salts. --Buffer solutions resist changes in pH. |
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Term
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Definition
| Reactions of acids and bases to produce salts and water |
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Term
| How does one name a base? |
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Definition
1. name the metal
2. add "hydroxide" |
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Term
| Name 3 polyhydroxic bases |
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Definition
| Mg(OH)2, Al(OH)3, Fe(OH)3, Ca(OH)2, Sr(OH)2 |
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Term
| name 3 strong bases (Formulas/examples) |
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Definition
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Term
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Definition
| Mg(OH)2, Ca(OH)2, Sr(OH)2 |
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Term
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Definition
| molecules composed of hydrogen and one or more electronegative elements |
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Term
| binary acid formulas always begin with (examples!) |
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Definition
Hydrogen
HCl, HBr, HF<-- weak acid |
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Term
Define: oxoacids
(examples!) |
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Definition
Molecules composed of H, O, and a third element
HNO3, H2SO4, H3PO4 |
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Term
| Acids dissociate when ____, forming ____ |
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Definition
hydrolyzed
positive hydrogen ions and negative anions |
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Term
Name three strong acids:
one must be polyprotic
must name charges on all three
must name/give formula/reaction for all three |
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Definition
-Hydrochloric acid...H+ + Cl- = HCl
-Sulfuric acid...H+ + SO4-- = H2SO4 <---POLYPROTIC
-Nitric acid...H+ + NO3- = HNO3 |
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Term
Name three weak acids:
two must be polyprotic
must name charges on all three
must name/give formula/reaction for all three |
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Definition
-phosphoric acid...H+ + PO4---=H3PO4 <--polyprotic
-carbonic acid... H+ + CO3-- = H2CO3 <--polyprotic
-acetic acid...H+ + C2H3O2- = C2H3OOH |
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Term
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Definition
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Term
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Definition
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Term
| When the anion in an acid ends in "ide," how do you name it? |
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Definition
1. begin the name w/ "hydro"
2. change the anion name ending to "ic" |
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Term
| When the anion in an acid ends in "ite," how do you name it? |
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Definition
| write the anion root + "ous" |
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Term
| When the anion in an acid ends in "ate," how do you name it? |
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Definition
| write the anion root + "ic" |
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Term
| Define: the ionization constant |
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Definition
the ratio of
the product of
the concentrations
of the dissociated ions
of an acid or base
to the concentration
of the undissociated acid or base |
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Term
| Define: the ionization constant for an aicd: |
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Definition
Ka = [H+][Anion]
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[HA] ...meaning acid molarity |
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Term
| Define: the ionization constant for a base |
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Definition
Kb = [OH-][Cation]
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[Cation OH]...meaning base molarity |
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Term
| As ___ increases, the acid or base is stronger |
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Definition
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Term
| For monoprotic acids and monohydroxic bases, what is different about the ionization constant? |
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Definition
| the numerator of both expressions is = to [H+]squared for acids [OH-]squared for bases |
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