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Lab 10, Post-Lab and Data

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Lab 10: Solubility Product and the Common Ion Effect
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Solubility Product a_n4 the Common Ion Effect
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REPORT FORM
Part B: Preparation and Standardization of the HCl Solutiot/,
Concentrat_io~ ~_f.,S~a~~ard NaOH
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- ·, -Aliqupt,of Standard NaOH Used . ::t.1 • b
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Volume HCl
'Z.Y.
mL
Molarity of HCl
o. o1Jl. mL
'1rtitial Voium~:
f,
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O-S'S
mL
t.S. -:1
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T ial 3
Trial 2
Trial 1
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mL
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2.g. ··1~· •. m:L
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o .,oi3 l. mL
Average concentration of HCl O, o"f ~"Z.. .M
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- - +_ _ mL
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Part C: Titration of Ca(OH)2 Solution
Solution Titration-Aliquot size . ., Z/i '0
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ml:;•
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·,. 0.'2 :'
mL · , .
/2..j
mL
VolumeHCl
12 · 6
mL
Molarity of OH-
o. toS
mL
Initial Volume:
O.JOS
Average Solubility
. -·
Trial 2
· · '"Tr'ial 1: · .;
Final,V
olume:
r
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Average[OH- 1]
1
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5
·,,.
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1
JJ./
mL
mL
/2.b
mL
0./05
O· Ol 1-o,3 M
-~ Ks calculation (show your work and c~mpare answer to literature value)
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mL
mL
- - + - - - mL
Average [Ca+21 0, 0 r'26'
M
C
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mL
Cl
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Lab 10: Solubility Product and the Common Ion Effect
~-7-2
Part D: Titration of Ca(OH) 2 Solution in the Presence of Ca+
Solution Titration-Aliquot size
ZS•
ml
0
Trial 2
Trial 1
Initial Volume:
tz. 1,;
ml
12,r
21.'f
Volume HCl
"· ,r
ml
f. '1.
ml
ml
O, ~iii-
mL. ,
.3
Final Volume:
J
o. o3 '1/..
Molarity of OHAverage [OH- 1]
ml
a. o~~1f
Average Solubility
ml
ml
ml
ml
mL
mL
2
M
' · . 'A~erage [Ca+
9~ C?'lse ~M
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==: . 0. 01 ,'"'"
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l<sp calcul~tion (show your work and.,c9mpare answer to literature
. . value)
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Compare the'solubilities in Part C arid.Part D, and discuss. ·
Compare the
K.p from
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Part C and Part D, and discuss.
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Lab 10: Solubility Product and the Common Ion Effect
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Post-LC1:b Questions
1. Convert your answers for the solubility of calciu~ hydroxide in Part C to grams per liter.
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2. What is the pH at the_equivalence point f~r each titration? Look up bromqcresol purple inqicator and
explain why this is a' good ~hoice for this titration.
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3. Calculate l<sp for MnCO3 if 1.07 mg/L are required_to make a saturated solutfo!l·
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4. Why is it essential that the 'filtrate be as clear as possible?
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5. Why would an acid-base titration pro),ably· be imj:;ractica_t fw the me!1~urement of the
Mg(QBh?, ($ee introduction for a hint.) -
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Lab 1O: Solubility Product and the Common Ion Effect
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6. The pH at the equivalence pomt 1s appropriate for the indicator bromocresol,Pµ, P. h
H transition
above), but it is suggested that phenolphthalein could be used instead. Look _up t e p
range for phenolphthalein, and explain why it would also be an acceptep choice .
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8. If the solution is, poorly filtered, the filtrate ~ppea,r s cloudy. Why is this? Woul!f ~he Ksl? c~kulated
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from this data be higher or lower than the hue va.lue?: .
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9. Find the mathematical equation that is used to c;alculate the ionic strength of a solution. Show that the
ionic strength is the same in both parts of this ·experiment.
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