Complete the following table and answer the questions, showing all of your calculations. Trial Equivalence point (mL) 1 10.5 ml 2 10 ml 3 11.8 ml Questions: 1. Calculate the [OH-] in the saturated solution from the results of your titrations. 2. Calculate the [Ca2+] in the saturated solution. 3. Calculate the Kp for calcium hydroxide. 4. Find the accepted value of the Kp for calcium hydroxide and compare it with your value. Discuss the discrepancy and suggest possible sources of experimental error.
Complete the following table and answer the questions, showing all of your calculations. Trial Equivalence point (mL) 1 10.5 ml 2 10 ml 3 11.8 ml Questions: 1. Calculate the [OH-] in the saturated solution from the results of your titrations. 2. Calculate the [Ca2+] in the saturated solution. 3. Calculate the Kp for calcium hydroxide. 4. Find the accepted value of the Kp for calcium hydroxide and compare it with your value. Discuss the discrepancy and suggest possible sources of experimental error.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![Determining the Ksp of Calcium Hydroxide
Calcium hydroxide is an ionic solid that is sparingly soluble in water. A saturated, aqueous, solution of Ca(OH)2
is represented in equation form as shown below.
Ca(OH)2 (s) → Ca²+ (aq) + 2OH(aq)
The solubility product expression describes, in mathematical terms, the equilibrium that is established between
the solid substance and its dissolved ions in an aqueous system. The equilibrium expression for calcium
hydroxide is shown below.
Ksp = [Ca²+][OH-]²
The constant that illustrates a substance's solubility in water is called the Ksp. All compounds, even the highly
soluble sodium chloride, have a Ksp. However, the Ksp of a compound is commonly considered only in cases
where the compound is very slightly soluble and the amount of dissolved ions is not simple to measure.
Your primary objective in this experiment is to test a saturated solution of calcium hydroxide and use your
observations and measurements to calculate the Ksp of the compound. You will do this by titrating the prepared
Ca(OH)2 solution with a standard hydrochloric acid solution. By determining the molar concentration of
dissolved hydroxide ions in the saturated Ca(OH)2 solution, you will have the necessary information to calculate
the Ksp.
OBJECTIVES
In this experiment, you will
• Titrate a saturated Ca(OH)2 solution with a standard HCl solution.
• Determine the [OH-] for the saturated Ca(OH)2 solution.
• Calculate the Ksp of Ca(OH)2.
solution 0.050M hydrochloric
acid, HC.
50 те са сонда
2
13
Intereuptent CRED
MOLD
Figure 1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbb8a976c-eb7b-4ed9-b029-cfa72f795dab%2Fb775ca9b-cce8-4e68-b38a-04ad192f5ab3%2F2gwujxw_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Determining the Ksp of Calcium Hydroxide
Calcium hydroxide is an ionic solid that is sparingly soluble in water. A saturated, aqueous, solution of Ca(OH)2
is represented in equation form as shown below.
Ca(OH)2 (s) → Ca²+ (aq) + 2OH(aq)
The solubility product expression describes, in mathematical terms, the equilibrium that is established between
the solid substance and its dissolved ions in an aqueous system. The equilibrium expression for calcium
hydroxide is shown below.
Ksp = [Ca²+][OH-]²
The constant that illustrates a substance's solubility in water is called the Ksp. All compounds, even the highly
soluble sodium chloride, have a Ksp. However, the Ksp of a compound is commonly considered only in cases
where the compound is very slightly soluble and the amount of dissolved ions is not simple to measure.
Your primary objective in this experiment is to test a saturated solution of calcium hydroxide and use your
observations and measurements to calculate the Ksp of the compound. You will do this by titrating the prepared
Ca(OH)2 solution with a standard hydrochloric acid solution. By determining the molar concentration of
dissolved hydroxide ions in the saturated Ca(OH)2 solution, you will have the necessary information to calculate
the Ksp.
OBJECTIVES
In this experiment, you will
• Titrate a saturated Ca(OH)2 solution with a standard HCl solution.
• Determine the [OH-] for the saturated Ca(OH)2 solution.
• Calculate the Ksp of Ca(OH)2.
solution 0.050M hydrochloric
acid, HC.
50 те са сонда
2
13
Intereuptent CRED
MOLD
Figure 1
![Complete the following table and answer the questions, showing all of your calculations.
Trial
Equivalence point
(mL)
1
10.5mb
2
10 тв
3
11.8 ml
Questions:
1. Calculate the [OH-] in the saturated solution from the results of your titrations.
2. Calculate the [Ca²+] in the saturated solution.
3. Calculate the Kp for calcium hydroxide.
sp
sp
4. Find the accepted value of the Kp for calcium hydroxide and compare it with your value.
Discuss the discrepancy and suggest possible sources of experimental error.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbb8a976c-eb7b-4ed9-b029-cfa72f795dab%2Fb775ca9b-cce8-4e68-b38a-04ad192f5ab3%2F2k23nhd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Complete the following table and answer the questions, showing all of your calculations.
Trial
Equivalence point
(mL)
1
10.5mb
2
10 тв
3
11.8 ml
Questions:
1. Calculate the [OH-] in the saturated solution from the results of your titrations.
2. Calculate the [Ca²+] in the saturated solution.
3. Calculate the Kp for calcium hydroxide.
sp
sp
4. Find the accepted value of the Kp for calcium hydroxide and compare it with your value.
Discuss the discrepancy and suggest possible sources of experimental error.
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