Intro to Acids and Bases Review Sheets

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Review Sheet: Unit 11
KEY
Name______________
Name these Acids:
hydroiodic acid
HI
___________________
nitric acid
HNO3 ___________________
H2SO3
H3PO4
sulfurous acid
____________________
phosphoric acid
____________________
Write formulas for these acids:
HF
hydrofluoric acid: ___________
H3PO3
phosphorous acid:______________
Name these bases and salts:
potassium hydroxide
KOH __________________
MgSO4
magnesium sulfate
__________________
Calculate:
1.
the pH of a 1.4 x 10-2 M NaOH solution
! H + # !OH % # = 1.0 & 10 %14
" $"
$
! H + # !1.4 & 10 %2 # = 1.0 & 10 %14
" $"
$
pH = ! log "# H + $% = ! log "#7.1 & 10 !13 $% =
2.
pH = 12
the [H+] of a solution with pH = 3.2
pH = ! log "# H + $%
3.
! H + # =7.1 & 10 %13 M
" $
3.2 = ! log "# H + $%
" H + $ = 6.3 & 10 !4 M
# %
the [OH-] of a solution with a [H+] of 9.3 x 10-4 M
! H + # !OH % # = 1.0 & 10 %14
" $"
$
! 9.3 & 10 %4 # !OH % # = 1.0 & 10 %14
"
$"
$
CHEMISTRY: A Study of Matter
© 2004, GPB
11.20a
!OH % # = 1.1 & 10 %11
"
$
4.
In a titration, 25.0 mL of a 0.20 M NaOH solution is used to
neutralize 10.0 mL of HCl.
a. Write the equation for this neutralization reaction:
NaOH + HCl  H2O + NaOH
b. Calculate the molarity of the acid:
moles H +
moles OH !
( M A )(V A ) =
( M B )(VB )
1 moleA
1 moleB
1moles H +
1moles OH !
( M A )(10.0mL) =
(0.20 M )(25.0mL)
1 moleA
1 moleB
5.
M A = 0.50 M HCl
In a titration, 24.2 mL of 0.120 M Mg(OH)2 were required to
neutralize 33.1 mL of H3PO4.
a. Write the equation for this neutralization reaction:
2 H3PO4 + 3 Mg(OH)2
 6 H2O + Mg3(PO4)2
b. What is the molarity of the acid?
3 moles H +
2 moles OH !
( M A )(33.1mL) =
(0.120 M )(24.2mL)
1 moleA
1 moleB
M A = 0.0585 M H 3 PO4
6.
What is the word equation for the neutralization of a strong acid and
strong base?
acid + base  salt + water
7.
hydrogen ions
In a neutral solution, moles of ___________
equal the moles of
hydroxide
ions
____________________.
8.
neutral
A pH of 7 indicates that a solution is ________________;
a ph <7
acidic
would mean the solution is ______________;
and a pH >7 is a(n)
basic
___________________solution.
9.
Contrast a strong acid with a weak acid:
Strong acids ionize completely whereas weak acids do not.
CHEMISTRY: A Study of Matter
© 2004, GPB
11.20b
Define:
1. titration-
2. electrolyte-
3. end point-
4. salt-
A laboratory method to determine the concentration of an unknown solution of
acid or base using a standard.
A substance whose water solution conducts an electric current.
The point in a titration when the indicator changes color.
A compound formed from the positive ion of a base and the negative ion of an
acid during a neutralization reaction.
5. Arrhenius definition of an acid and a baseAn acid releases hydrogen ions in a water solution and a base releases hydroxide
ions in a water solution.
6. operational definition-
An operational definition describes a substance by its properties or
characteristics.
Fill in the blanks:
1.
sour
Acids have a _______________
taste, react with metals to produce
indicators
hydrogen gas, turn _______________
______________
different colors
electrolytes
according to pH, and are _______________
because their water
solutions conduct electricity. On the other hand, bases have a
bitter
slippery
______________
taste, feel ______________,
turn
indicators
_______________ different colors according to pH, and are
electrolytes
_______________
because their water solutions conduct electricity.
2.
Most cleaning products are ( acidic, basic ) while most foods are
(acidic, basic).
3.
hot pink
blue
Bases turn litmus _____________,
phenolphthalein ___________,
green
red
and cabbage juice ____________.
Acids turn litmus ___________,
red (or pink)
colorless
phenolphthalein _____________,
and cabbage juice ____________.
CHEMISTRY: A Study of Matter
© 2004, GPB
11.20c
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