Term
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Definition
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Term
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Definition
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Term
| For what pH values is a solution acidic? |
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Definition
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Term
| For what pH values is a solution neutral? |
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Definition
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Term
| For what pH values is a solution basic? |
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Definition
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Term
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Definition
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Term
| For what pOH values is a solution acidic? |
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Definition
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Term
| For what pOH values is a solution neutral? |
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Definition
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Term
| For what pOH values is a solution basic? |
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Definition
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Term
| How are pH and pOH of a solution related? |
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Definition
The sum of the two values = 14
pH + pOH = 14 |
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Term
| How are the concentrations of [H+] and [OH-] related in a solution? |
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Definition
The product of the concentrations = 1 x 10-14
[H+][OH-] = 1 x 10-14 |
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Term
Match pH value to distilled water.
a.) pH=2
b.) pH=7
c.) pH=12 |
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Definition
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Term
Match pH value to lye.
a.) pH=2
b.) pH=7
c.) pH=12 |
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Definition
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Term
Match pH value to stomach juice.
a.) pH=2
b.) pH=7
c.) pH=12 |
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Definition
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Term
| For a solution with a pH of 3, find pOH |
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Definition
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Term
| For a solution with a pH of 3, find [H+] |
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Definition
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Term
| For a solution with a pH of 3, find [OH-] |
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Definition
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Term
| Solubility Product Constant - Ksp |
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Definition
| An equilibrium exists in a saturated solution between dissolved and undissolved solute. "Ksp" is the equilibrium constant for this reaction. |
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Term
| Write the solubility product expression for AgCl double arrow Ag+ = Cl- |
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Definition
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Term
In a saturated solution of BaSO4, [Ba2+] = 2 x 10-5.
Find Ksp. |
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Definition
Each molecule of BaSO4 that ionizes produces equal concentrations of ions; therefore;
[Ba2+] = [SO42-]
Ksp = [Ba2+][SO42-]
Ksp=[2 x 10-5][2 x 10-5]
Ksp = 4 x 10-10 |
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Term
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Definition
| When an ionization reaction is at equilibrium, and additional ion is added, the reverse reaction rate increases to consume the added ion. |
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Term
NaCl ↔ Na+ = Cl-
What happens when Cl- is added to this system at equilibrium? |
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Definition
| According to the common ion effect, the reverse reaction will speed up, consuming Na+ and Cl-, and more NaCl will be formed. |
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Term
| Six common characteristics of ACIDS |
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Definition
form H2O solutions
conduct electricity
react with active metals
turn blue litmus red
neutralize bases
sour taste |
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Term
| Seven common characteristics of BASES |
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Definition
form H2O solutions
conduct electricity
turn red litmus blue
feel slippery
caustic
neutralize acids
bases + fats form soap |
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Term
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Definition
nitric
hydrochloric
sulfuric
hydriodic
hydrobromic
perchloric |
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Term
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Definition
hydrofluoric
acetic
carbonic
and most others |
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Term
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Definition
oxalic
phosphoric
sulfurous |
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Term
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Definition
hydroxides of:
potassium
sodium
barium s
trontium
calcium
also:
KOH
NaOH |
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Term
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Definition
H3O+ ion found in water solutions of acids.
Water molecule with a proton attached. |
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Term
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Definition
| acid + base → salt + water |
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Term
| Write the equation for hydrochloric acid and sodium hydroxide. |
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Definition
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Term
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Definition
| An acid yields protons in solution. (H+ ions) A base yields hydroxide ions in solution. (OH- ions) |
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Term
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Definition
An acid is a proton donor.
A base is a proton acceptor. |
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Term
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Definition
An acid is an electron pair acceptor.
A base is an electron pair donor. |
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Term
| Conjugate Base: Write conjugate base of HCl. |
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Definition
| When a Bronsted acid donates a proton, it becomes its conjugate base. Conjugate base of HCl is Cl-. |
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Term
| Conjugate Acid: Write conjugate acid of I- |
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Definition
| When a Bronsted base accepts a proton, it becomes its conjugate acid. Conjugate acid of I- is HI. |
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Term
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Definition
A substance which changes color along the pH scale.
e.g. litmus, phenolphthalein, methyl orange, bromthymol blue |
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Term
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Definition
| A process of finding the unknown concentration of a solution by allowing it to react with another solution of known volume and concentration. |
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Term
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Definition
| The point during a titration at which the acid reacts completely with the base. The indicator changes color. |
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Term
| Write the equation to calculate concentrations and volumes in titration reactions. |
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Definition
MA X VA = MB x VB
molarity = M
volume = V
acid = A
base = B |
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Term
| Calculate the volume of 10 M NaOH needed to titrate 5L of 2M HCl |
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Definition
MA X VA = MB X VB
2M X 5L = 10M X VB
1L = volume of base |
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Term
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Definition
| Equilibrium systems which resist changes in pH upon the introduction of acids or bases (due to the common ion effect). e.g. a weak acid (acetic acid) and its salt (sodium acetate) |
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Term
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Definition
| The passage of a direct electric current through an ionic solution, producing chemical changes at the electrodes. |
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