Acid Base Titrations

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Acid Base Titrations
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In a titration the molarity of one chemical is
determined by reacting it with another and
knowing the molarity of the other chemical.
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Special Equipment is used for a titration
Burette
Erlenmeyer Flask
Magnetic Stirrer
Pipette
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Digital Balance
Solid acid to make a standard solution
Volumetric Flask
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Titration Calculation 1. 6.50 mL of 0.100 M
H2C2O4 is required to neutralize 10.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2C2O4 2KOH ? K2C2O4
2H2O 0.00650 L 0.0100 L 0.100 M ? M this
is a molarity question molarity draw a
line KOH
KOH square brackets means the molarity
or concentration of what is inside.
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Titration Calculation 1. 6.50 mL of 0.100 M
H2C2O4 is required to neutralize 10.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2C2O4 2KOH ? K2C2O4
2H2O 0.00650 L 0.0100 L 0.100 M ? M You
need to get moles KOH over litres KOH You need to
start with H2C2O4 and then use stoichoimetry KOH
0.00650 L H2C2O4

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Titration Calculation 1. 6.50 mL of 0.100 M
H2C2O4 is required to neutralize 10.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2C2O4 2KOH ? K2C2O4
2H2O 0.00650 L 0.0100 L 0.100 M ? M KOH
0.00650 L H2C2O4 x 0.100 mole
1 L
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Titration Calculation 1. 6.50 mL of 0.100 M
H2C2O4 is required to neutralize 10.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2C2O4 2KOH ? K2C2O4
2H2O 0.00650 L 0.0100 L 0.100 M ? M KOH
0.00650 L H2C2O4 x 0.100 mole x 2 mole
KOH 1 L 1 mole H2C2O4
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Titration Calculation 1. 6.50 mL of 0.100 M
H2C2O4 is required to neutralize 10.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2C2O4 2KOH ? K2C2O4
2H2O 0.00650 L 0.0100 L 0.100 M ? M KOH
0.00650 L H2C2O4 x 0.100 mole x 2 mole
KOH 1 L 1 mole H2C2O4 0.0100
L
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Titration Calculation 1. 6.50 mL of 0.100 M
H2C2O4 is required to neutralize 10.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2C2O4 2KOH ? K2C2O4
2H2O 0.00650 L 0.0100 L 0.100 M ? M KOH
0.00650 L H2C2O4 x 0.100 mole x 2 mole
KOH 1 L 1 mole H2C2O4 0.0100
L 0.130 M
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If you get data in a table, you need to subtract
the final burette reading from the initial to get
the volume of acid or base added. A burette is a
device used to deliver a volume of solution and
determine the amount that was added. If you get
more than one run or trials, average them but
reject any volumes that are way off. Use some
common sense. Burette Volume in
mL Initial 0.00 8.95 17.41 Final 8.95
17.41 25.85 Volume Added 8.95 mL 8.46 mL 8.44
mL reject average 8.46 8.44 8.45
mL 2
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Now it's your turn to try one!
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Titration Calculation 2. 8.45 mL of 0.200 M
H2SO4 is required to neutralize 25.0 mL of KOH
solution in a titration. Calculate the base
concentration. H2SO4 2KOH ? K2SO4
2H2O 0.00845 L 0.0250 L 0.200 M ? M KOH
0.00845 L H2SO4 x 0.200 mole x 2 mole
KOH 1 L 1 mole H2SO4 0.0250
L 0.135 M
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Calculate the mass of H2C2O4.2H2O required to
make 100.0 mL of a 0.1000 M standard solution to
use in your titration lab tomorrow.
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Calculate the mass of H2C2O4.2H2O required to
make 100.0 mL of a 0.1000 M standard solution to
use in your titration lab tomorrow. 0.100 L
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Calculate the mass of H2C2O4.2H2O required to
make 100.0 mL of a 0.1000 M standard solution to
use in your titration lab tomorrow. 0.100 L
x 0.1000 mol 1 L
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Calculate the mass of H2C2O4.2H2O required to
make 100.0 mL of a 0.1000 M standard solution to
use in your titration lab tomorrow. 0.100 L
x 0.1000 mol x 126.06 g 1 L 1 mole
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Calculate the mass of H2C2O4.2H2O required to
make 100.0 mL of a 0.1000 M standard solution to
use in your titration lab tomorrow. 0.100 L
x 0.1000 mol x 126.06 g 1.261 g 1
L 1 mole