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What is the information needed to know if Ksp will increase or decrease with temperature? What is the effect on Ksp when temperature is increased?

What is the information needed to know if Ksp will increase or decrease with temperature? What is the effect on Ksp when temperature is increased?

Chemistry
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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Given: Concentration, Volume, Temperature (20C)

Calculated: Molarity, Concentration of OH- and Ca2+

 What is the information needed to know if Ksp will increase or decrease with temperature? What is the effect on Ksp when temperature is increased?

Procedure Part I: Standardization of the Hydrochloric Acid 1. Obtain about 100 mL of hydrochloric acid. Prepare a buret for titration with the HCl by rinsing first with distilled water and then again with the acid. Be sure to fill the buret tip. Record the initial volume. 2. Place a about 0.3 grams of sodium carbonate into a weighing boat and record the mass. Transfer about half into an Erlenmeyer flask and re-record the mass. Add about 20 mL of water to the flask along with a few drops of methyl orange. 3. Titrate the sodium carbonate to the end point, carefully recording the final volume. 4. Repeat steps 2&3 for a 2nd trial. Part II: Standardization of the Calcium Hydroxide 1. Obtain about 60 mL of the calcium hydroxide solution. Pour the mixture through filter paper to remove any undissolved solids. Record the temperature of the solution. 2. Wearing a rubber glove, discard the filter paper into the dry waste container and repeat the filtration with a new piece of filter paper. 3. Measure exactly 20.00 mL of the filtrate and pour into a 125 mL Erlenmeyer and add about 5 drops of indicator. Use distilled water to rinse residual liquid from the cylinder into the flask. 4. Prepare the buret for titration with the hydrochloric acid. Fill the buret with the standardized acid solution and record the initial volume. 5. Titrate the calcium hydroxide to the end point, carefully recording the final volume. 6. Repeat the titration for a 2nd trial. 7. Dispose of any extra base solution in the liquid waste coutainer. 8. Thoroughly rinse all glassware.
Transcribed Image Text:Procedure Part I: Standardization of the Hydrochloric Acid 1. Obtain about 100 mL of hydrochloric acid. Prepare a buret for titration with the HCl by rinsing first with distilled water and then again with the acid. Be sure to fill the buret tip. Record the initial volume. 2. Place a about 0.3 grams of sodium carbonate into a weighing boat and record the mass. Transfer about half into an Erlenmeyer flask and re-record the mass. Add about 20 mL of water to the flask along with a few drops of methyl orange. 3. Titrate the sodium carbonate to the end point, carefully recording the final volume. 4. Repeat steps 2&3 for a 2nd trial. Part II: Standardization of the Calcium Hydroxide 1. Obtain about 60 mL of the calcium hydroxide solution. Pour the mixture through filter paper to remove any undissolved solids. Record the temperature of the solution. 2. Wearing a rubber glove, discard the filter paper into the dry waste container and repeat the filtration with a new piece of filter paper. 3. Measure exactly 20.00 mL of the filtrate and pour into a 125 mL Erlenmeyer and add about 5 drops of indicator. Use distilled water to rinse residual liquid from the cylinder into the flask. 4. Prepare the buret for titration with the hydrochloric acid. Fill the buret with the standardized acid solution and record the initial volume. 5. Titrate the calcium hydroxide to the end point, carefully recording the final volume. 6. Repeat the titration for a 2nd trial. 7. Dispose of any extra base solution in the liquid waste coutainer. 8. Thoroughly rinse all glassware.
2. Your K, is temperature dependent. What further information would you need to see if it would increase with temperature or decrease? If you carried out the experiment in a room at 30°C, would the K, increase or decrease?
Transcribed Image Text:2. Your K, is temperature dependent. What further information would you need to see if it would increase with temperature or decrease? If you carried out the experiment in a room at 30°C, would the K, increase or decrease?
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