V= 30.0ml Concentration= 0.1001 M 1.) Using the volume and concentration of Ca(OH)2 recorded in your...
V= 30.0ml Concentration= 0.1001 M
1.) Using the volume and concentration of Ca(OH)2 recorded in your experiment, calculate the
volume of 0.0750 M phosphoric acid required to exactly react with it. This is the equivalence
point of your titration.
2.) Calculate the percent error of volumes at the equivalence point
Homework Answers
equation of reaction :
3 Ca(OH)2 + 2 H3PO4
Ca3(PO4)2 + 6 H2O
Moles of Ca(OH)2 = Molairity * Volume = 0.1001 * 30 * 10-3 = 3.003 * 10-3 moles
Moles of H3PO4 = Moles of Ca(OH)2 * 2/3 (from the equation) = Molarity * Volume
3.003 * 10-3 * 2 / 3 = 0.0750 * V
Solving, we get: V = 26.693 ml
Add Answer to:
V= 30.0ml Concentration= 0.1001 M
1.) Using the volume and concentration of Ca(OH)2 recorded in
your...
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the titration.
How many moles of base were required to react completely with the
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How many moles of HCl were present in the original 25.00 mL of
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04 Question (a points) aSee page 166 Watch the...
An aqueous solution of Ca(OH)2with a concentration of 0.161 M was used to titrate 25.00 mL...
An aqueous solution of Ca(OH)2with a concentration of
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An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration. An aqueous solution of Ca(OH)2with a
concentration of 0.161 M was used to titrate 25.00 mL of
aqueous HCl. 18.63 mL of the Ca(OH)2was required to
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A) How many moles of base...
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help please and thanks
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1. Use the data given to calculate the following parts: a. Using your data for the...
1. Use the data given to calculate the following parts:
a. Using your data for the value for VEP1, calculate the
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clearly, with units and correct significant figures.
b. Using your data for the value for VEP2, calculate the
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An aqueous solution of Ca(OH)2with a concentration of
0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
How many moles of base were required to react completely with the
acid in this reaction?
How many moles of HCl were present in the original 25.00 mL of
acid?
What is the molarity of the original HCl solution?
04 Question (a points) aSee page 166 Watch the...
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
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An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration. An aqueous solution of Ca(OH)2with a
concentration of 0.161 M was used to titrate 25.00 mL of
aqueous HCl. 18.63 mL of the Ca(OH)2was required to
reach the endpoint of the titration.
A) How many moles of base...
help please and thanks
4. A group of students conducted a titration of 25.00-ml saturated Ca(OH)2 solution with 0.0480M HCI. The students found that 10.10-mL of acid was required to reach the equivalence point. Calculate the molar concentration of OH and Ca, the molar solubility, and K. of the analyte. Show detailed calculation for each Detailed Method of Calculation (OH) in the analyte: Ca?) in the analyte: molar solubility of Ca(OH)2: Ksp of Ca(OH)2:
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