Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.97PAE
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![1. Write the reaction for the dissolution of Ca(OH)2, as well as the Ksp expression for the reaction.
2. Write the neutralization reaction between Ca(OH)₂ and HCI. Include both the molecular
reaction, as well as the net ionic reaction.
3. A student titrate a saturated solution of Ca(OH)2 with 0.0100 M HCl. A 10.00 mL sample of the
Ca(OH)₂ solution required 20.04 mL of HCI to reach the endpoint of the titration.
a. Calculate the moles of HCI added in the titration, and then calculate the moles of OH-
present in the saturated solution.
b. Calculate [OH] and [Ca²+] in the saturated solution.
c. Calculate Ksp for Ca(OH)2.
4. When peforming multiple trials at different temperatures, a student obtained the following
trendline equation. Calculte AH and AS.
y = 1737x- 18.31](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb81558ef-0edc-4b96-8c9b-c81d5284a907%2Fa19a9405-ba95-4de9-b55f-1ece56b751ff%2Fn0zlc7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. Write the reaction for the dissolution of Ca(OH)2, as well as the Ksp expression for the reaction.
2. Write the neutralization reaction between Ca(OH)₂ and HCI. Include both the molecular
reaction, as well as the net ionic reaction.
3. A student titrate a saturated solution of Ca(OH)2 with 0.0100 M HCl. A 10.00 mL sample of the
Ca(OH)₂ solution required 20.04 mL of HCI to reach the endpoint of the titration.
a. Calculate the moles of HCI added in the titration, and then calculate the moles of OH-
present in the saturated solution.
b. Calculate [OH] and [Ca²+] in the saturated solution.
c. Calculate Ksp for Ca(OH)2.
4. When peforming multiple trials at different temperatures, a student obtained the following
trendline equation. Calculte AH and AS.
y = 1737x- 18.31
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