(A)
ACID
(B) BASE
(C) CONJUGATE ACID
(D)CONJUGATE BASE
(E) ARRHENIUS ACID
(F) ARRHENIUS BASE
(G) BROMSTED LOWRY ACID
(H)BROMSTEAD-LOWRY BASE
(J) LEWIS BASE
(I) LEWIS ACID
(K) Example of Arrhenius Acid
(L) Bronstein Lowry Theory
(N) Examples of Lewis Base
(M) Examples of Lewis Acids
(O) AMPHOTERIC COMPOUND
1. ____ Any species that can accept a proton from another molecule. Proton
Acceptor.
2. ____ Any species that can accept a pair of electrons. Electron Pair Acceptor
3. ____ A compound when dissolved in water (aqueous solution) will form
hydrogen H + ions and/or increase the concentration of Hydrogen Ions.
4. ____Can react as either an acid or a base.
5. ____ Any species that can donate a proton H+ to another molecule. Proton
Donor
6. ____ HNO3
7. ____ Substance that dissociates in water to form hydroxide OH- ions. It
increases the concentration of OH- ions in an aqueous solution.
8. ______ Developed in 1923 as an acid base theory that describes acid-base
interactions in terms of proton transfer.
9. ______ Any species that can donate a pair of electrons. Electron Pair Donor
10.
_______ Cu2, Fe2+ and H+
11.
_______ a chemical substance that neutralizes alkalis, dissolves some
metals, and turns litmus red; typically, a corrosive or sour-tasting liquid of
this kind, conducts electricity.
12.
________ any substance that in water solution is slippery to the touch,
tastes bitter, changes the colour of indicators (e.g., turns red litmus paper
blue), reacts with acids to form salts, and conducts electricity.
13.
______ The particle that is left over after an acid loses its hydrogen ion.
Basically, an acid that has given up a proton?
14.
_______ Chemical compound formed when an acid donates a Proton H+
to a base.
15.
NH3
16.
True or False: STRONG ACIDS HAVE A WEAK CONJUGATE BASE?
#17-27 10 points LIST 5 PROPERTIES OF ACIDS AND BASES:
ACID
PH
TASTE
TEXTURE
REACTIVITY
CONDUCTIVITY
__________________
__________________
__________________
__________________
__________________
BASE
__________________
__________________
__________________
__________________
__________________
28. Which model (Arrhenius, Bronstein-Lowry or Lewis) limits the substances that
are defined as bases? _________________________
29. Another name for the Chemical Theory of Electrolytes is the
____________________ Model/Method.
30. What is a monoprotic acid?
__________________________________________________________________
31. What is a diprotic acid?
__________________________________________________________________
32. What is a triphotic acid?
__________________________________________________________________
33. True or False: Polyphrotic acids can lose several protons per molecule and can
further be categorized into diprotic or triprotic acids?
34. Label monoprotic, diprotic, triphotic or amphoteric:
____________Sulfuric Acid
___________ Phosphoric Acid
___________ Nitric Acid
___________ Chromic Acid
___________ Hydrocloric Acid
___________ Oxalic Acid
___________ Water
___________ Citric Acid
35. True or False: Metals are not good conductors. They have no mobile electrons.
36. True or False: Solid salts do not conduct electricity because the ions are not
free enough to move. Only when they are dissolved in water or melted into liquid
can the ions move freely and conduct.
37. True or False: When either the acid or base is of known concentration then it is
a standard solution?
38. True or False: The endpoint is when neutralization is reached in acid-base
titration. ( H+ions = OH- ions)
39. Anhydrous means _______________________________.
40. Any oxide that will produce an acid when dissolved in water is called
_______________________________ (non-metallic oxide + water)
41. Any oxide that will produce a base when dissolved in water (metallic oxide +
water). ___________________________________
42. True or False: The larger the Ka Value, the stronger the acid?
43. A conjugate acid in Bronsted Lowryis a chemical compound formed when an
ACID DONATES a ________________ to a _________________.
44. A conjugate acid formula is: THE FORMULA OF THE BASE PLUS
___________________________________.
45. What is the chemical equation for the ionization of HNO3 in water, and the
name of the conjugate acid-base pair?
46. True or False: Acidic solutions (vs basic solutions) have more hydronium ions
than hydroxide ions.
47. What are the products of a reaction between an acid and a base?
____________________________
48. The concentration of an unknown base is called __________________.
49.What is the formula for the following:
Nitrous Acid = ___________________ Chromic Acid _________________
Oxalic Acid = ____________________ Lead II Hydroxide ______________
Acetic Acid = ____________________ Chlorous Acid __________________
Label Strong Acid, Weak Acid, Strong Base, Weak Base or NEUTRAL:
________ HI
________HNO3
________ HCL
_________NaOH
________Br
_________ HCLO4
________LiOH
_________ Fe(OH)2
____________Ca(OH)2
______________ NH3
_________ H2SO3
______________ HNO2
_____________ HBr
_________ HCLO4
________ HF
________ C2H2O4
_____________ NaBr
Name the 6 strong acids:
1
2
3
4
5
6
Name the 6 strong bases
1
2
3
4
5
6
This reacts with a base to form salts ____________________
This reacts with an acid to form salts ____________________
What is the NET equation for neutralization?
What is binary vs. oxyacid?
What is a monoprotic acid and 2 examples:
1
2
What is a polyprotic acid and give 2 exampls:
1
2
The stronger the acid the _________________ its conjugate base. Why?
The stronger the base, the _______________ its conjugate base. Why?
What is the equation for the self ionization of water?
What do square brackets represent?
What is PH?
What is pOH?
Acid
Conjugate Base
Equation
H2SO3
HSO3
H2SO3 ------HSO3 + H+
H3PO4
_______________
_______________________________
_________
F
_______________________________
_________
NO3
_______________________________
H2PO4
_______________
_______________________________
H2O
_______________
_______________________________
________
SO4-2
_______________________________
HPO4-2
_______________
_______________________________
NH4+
_______________
_______________________________
A _______________________ reaction is when an acid and a base are reacted
together to produce water and a salt.
__________________ A procedure in which a solution of known concentration is used
to determine the concentration of an unknown solution.
The solution of known concentration is also referred to as the ______________
solution.
The __________________ of a titration occurs when you have added just enough of
the one solution to completely react with the other solution.
A ________________ is used to indicate the end of a titration.
ACID
BASE
ARRHENIUS
BRONSTED-LOWRY
LEWIS
EXAMPLE OF ARRHENIUS:
EXAMPLES OF BRONSTED LOWRY:
EXAMPLES OF LEWIS:
TRUE OR FALSE: CONJUGATES ARE PRODUCTS
TRUE OR FALSE BRACKETS MEAN CONCENTRATION
WHAT IS THE SELF IONIZATION OF WATER?
TRUE OR FALSE: THE MORE STABLE THE CONJUGATE, THE STRONGER
THE ACID.
TRUE OR FALSE: STRONGER ACID = WEAKER BASE
TRUE OR FALSE: MORE OXYGEN = STRONGER ACID IN SENSE OF
OXYACIDS.
TRUE OR FALSE: INCREASES IN OXYGEN INCRASE THE
ELECTRONEGATIVITY. IT PULLS THE OH OFF THE BOND AND THIS
RESULTS IN WEAKER BASE AND STRONGER ACID.