125 mL Erlenmeyer flask
50.0 mL of distilled water
10 mL pipet with pump
waste beaker
Procedure:
1.Fill the buret with the acid solution.
2.Pipet 10.0 mL of calcium hydroxide into the flask.
3.Add approximately 10.0 mL of water to the flask.
4.Add 4 drops of bromophenol blue to the flask.
5.Titrate the base to an endpoint and record the volume of acid added.
6.Dispose of the flask contents into a waste beaker.
7.Repeat steps 2-6 four more times.
Analysis:
1.Present your data in a table. Use the following table as a guide:
Trial 1 Trial 2
Initial volume of HCl(mL)
Final volume of HCl(mL)
Volume of HCl added(mL)
Hi Cna someone please tell me what I must out into the Trial 1 column? It would be greatly appreciated.
theLab: Determining the Ksp For Ca(OH)2
Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide.
Experimental Design: A saturated solution of calcium hydroxide is titrated with a hydrochloric acid solution of known concentration to a bromophenol blue endpoint (yellow).
Materials:
50.0 mL of 0.10 M HCl(aq)
bromophenol blue indicator
50.0 mLsaturated calcium hydroxide
50.0 mL buret
125 mL Erlenmeyer flask
50.0 mL of distilled water
10 mL pipet with pump
waste beaker
Procedure:
1.Fill the buret with the acid solution.
2.Pipet 10.0 mL of calcium hydroxide into the flask.
3.Add approximately 10.0 mL of water to the flask.
4.Add 4 drops of bromophenol blue to the flask.
5.Titrate the base to an endpoint and record the volume of acid added.
6.Dispose of the flask contents into a waste beaker.
7.Repeat steps 2-6 four more times.
Analysis:
1.Present your data in a table. Use the following table as a guide:
Trial 1 Trial 2
Initial volume of HCl(mL)
Final volume of HCl(mL)
Volume of HCl added(mL)
6 answers
If you have all of the information posted, then 500 mL of the saturated solution of Ca(OH)2 must have used 0.10 x 0.050 L = 0.005 mols HCl. The reaction is
Ca(OH)2 + 2HCl ==> CaCl2 + 2H2O.
Therefore, mols Ca(OH)2 must be 1/2 of the HCl mols or 0.005/2 = 0.0025.
From there you can calculate (Ca^+2) and (OH^-) and Ksp. Post your work if you get stuck or if I have misinterpreted the problem. Can it be chance that you used EXACTLY 50.0 mL HCl or is that what you started with?
Ca(OH)2 + 2HCl ==> CaCl2 + 2H2O.
Therefore, mols Ca(OH)2 must be 1/2 of the HCl mols or 0.005/2 = 0.0025.
From there you can calculate (Ca^+2) and (OH^-) and Ksp. Post your work if you get stuck or if I have misinterpreted the problem. Can it be chance that you used EXACTLY 50.0 mL HCl or is that what you started with?
Let me repost the important information only:
Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide.
Materials are:
*50.0 mL of 0.10 M HCl(aq)
*bromophenol blue indicator
*50.0 mLsaturated calcium hydroxide
*50.0 mL buret
*125 mL Erlynmyer Flask
*50.0 mL of distilled water
*10.0 mL pipet with pump
*waste beaker
The procedure for the lab is:
1.Fill the buret with the acid solution.
2.Pipet 10.0 mL of calcium hydroxide into the flask.
3.Add approximately 10.0 mL of water to the flask.
4.Add 4 drops of bromophenol blue to the flask.
5.Titrate the base to an endpoint and record the volume of acid added.
6.Dispose of the flask contents into a waste beaker.
7.Repeat steps 2-6 four more times.
The following is what I am having trouble with.
Present your data in a table.Use the following table as a guide:
Trial 1 Trial 2 Trial 3
*Initial volume
of HCL(mL)
*Final volume
of HCL (mL)
*Volume of
HCL added (mL)
I am having difficulty regarding the trial 1 column. What is my initial volume of HCL(mL) supposed to be?
Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide.
Materials are:
*50.0 mL of 0.10 M HCl(aq)
*bromophenol blue indicator
*50.0 mLsaturated calcium hydroxide
*50.0 mL buret
*125 mL Erlynmyer Flask
*50.0 mL of distilled water
*10.0 mL pipet with pump
*waste beaker
The procedure for the lab is:
1.Fill the buret with the acid solution.
2.Pipet 10.0 mL of calcium hydroxide into the flask.
3.Add approximately 10.0 mL of water to the flask.
4.Add 4 drops of bromophenol blue to the flask.
5.Titrate the base to an endpoint and record the volume of acid added.
6.Dispose of the flask contents into a waste beaker.
7.Repeat steps 2-6 four more times.
The following is what I am having trouble with.
Present your data in a table.Use the following table as a guide:
Trial 1 Trial 2 Trial 3
*Initial volume
of HCL(mL)
*Final volume
of HCL (mL)
*Volume of
HCL added (mL)
I am having difficulty regarding the trial 1 column. What is my initial volume of HCL(mL) supposed to be?
The table doesnt want to be neat but the trial 1, trial 2 and trial 3 should be shifted more to the right side
The initial volume of HCl is the reading of the buret at the beginning of the titration. It may or may not be zero. Then you have a final volume HCl. The volume of HCl added, then, is the difference between the two columns; i.e., the final volume reading minus the initial volume reading. For example, you may have started with a buret reading of 0.75 mL. That will be the initial volume of HCl. Then suppose you titrated with HCl and the indicator changed at 24.55 mL. That will be the final volume. Then the volume HCl used will be
24.55 - 0.75 = 23.80 mL.
24.55 - 0.75 = 23.80 mL.
Here are my results:
*Initial volume
of HCL(mL)
Trial 1- 0.0
Trial 2- 2.51
Trial 3- 4.95
Trial 4- 7.4
Trial 5- 9.9
*Final volume
of HCL (mL)
Trial 1- 2.51
Trial 2- 4.95
Trial 3- 7.4
Trial 4- 9.9
Trial 5- ?
*Volume of
HCL added (mL)
Trial 1- 2.51
Trial 2- 2.44
Trial 3- 2.45
Trial 4- 2.50
Trial 5- ?
How would I get Final volume of HC (mL) and Volume of HCL added (mL) for trial 5?
*Initial volume
of HCL(mL)
Trial 1- 0.0
Trial 2- 2.51
Trial 3- 4.95
Trial 4- 7.4
Trial 5- 9.9
*Final volume
of HCL (mL)
Trial 1- 2.51
Trial 2- 4.95
Trial 3- 7.4
Trial 4- 9.9
Trial 5- ?
*Volume of
HCL added (mL)
Trial 1- 2.51
Trial 2- 2.44
Trial 3- 2.45
Trial 4- 2.50
Trial 5- ?
How would I get Final volume of HC (mL) and Volume of HCL added (mL) for trial 5?
1 answer