Log in
HomeStudy Guides420,000CA160,000

CHM110H5 Study Guide - Final Guide: Stoichiometry, Junkers J.I, Boiling Point

159 views5 pages
School
UTM
Department
Chemistry
Course
CHM110H5
Professor
All

For unlimited access to Study Guides, a Grade+ subscription is required.

Document Summary

The purpose of this experiment is to determine the ksp and standard thermodynamic parameters for dissolving ca(oh)2. This was done by doing six titrations (per person), three at room temperature and three at either boiling point or between 60 and 70 degrees celsius with 0. 0200m. This experiment had three main components, preparing the saturated solution of ca(oh)2, titration with hcl at room temperature and a titration with hcl at boiling point temperature or. To prepare the saturated solution of ca(oh)2, a prepared sample vial containing approximately 2g of ca(oh)2 was obtained and was then transferred into a 250ml beaker in the fume hood. Approximately 100ml was then added to the beaker and a magnetic stirring bar. The solution was let to stir at room temperature for approximately 15 minutes and then was let to stand undisturbed to allow for most of the salt to settle. A titration with hcl at room temperature was then performed.

Get access

Grade+
$40 USD/m
Billed monthly
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
10 Verified Answers

Related Documents

CHM110H5 Lecture Notes - Lecture 3: Pipette, Phenolphthalein, Filter Paper
amaranthjackal900
CHM110H5 Lecture Notes - Lecture 1: Pipette, Filter Paper, Titration
apricotreindeer105
CHM110H5
Final Exam
Study Guide
CHM110H5 Study Guide - Midterm Guide: Calcium Hydroxide, Burette, Titration
harlequinhound715

Related Questions

I have a lab report to write on an experiment titled Thermodynamics of a compound. We titrated 10ml of Ca(OH)2 with 8.7 ml 0.1M HCl at room temperature. Then we heated (to boiling) a different batch and performed three titrations that took an average 0f 2.0ml HCl. We are supposed to figures out the concentrations of Ca and OH and get the ksp to use in deltaG =-RTlnKsp. We will use the room temp of 293.7K and a second time with the heated temp of 373K. Eventually we are to find entropy and gibbs free energy but I am still stuck at finding ksp. I know that the moles of hydroxide are twice the calcium .I figured the moles of HCl to be 0.0087Lx 0.1M = 0.00087 and thus equal to the moles of base at equivalence point so do I divide by 2 or multiply by 2 to get [Ca] [OH]2 to get ksp. And then I think there is another step in there. Do I use the volume of base somewhere?

In our lab experiment, we filtered CaCl and CaOH2 solutions that we prepared the previous week and transferred both of the filtrates using a 25 ml pipette into two erlenmeyer flasks. We then prepared the standard HCl by pipeting 100 ml of HCl to prepare 250 ml of 0.04M HCl from the 0.1 M HCl solution that we initially had. We pipeted 100 ml of HCl into a 250 ml volumetric flask and diluted to the mark. The buret was filled with the prepared HCl and both the CaCl and CaOH2 were titrated until a yellow endpoint was reached, this titration was repeated three times for each solution. The data that I obtained was:

CaCl= Initial(ml)--Final (ml) --- Volume of HCl(ml)

1.30 --24.2--22.9

0.50 --23.5 --23.0

1.60 --23.2 -- 21.6

Ca(OH)2= initial--final-- volume of HCl

1.00-- 28.3-- 27.3

2.00-- 28.8-- 26.8

2.00-- 28.1 --26.1

Q1. For each sample titrated, calculate the mean and standard deviation of your two or more titration volumes.

Q2. Using mean titration volumes, calculate the hydroxide concentration in each of the two saturated Ca(OH)2 solutions.

In our lab experiment, we filtered CaCl and CaOH2 solutions that we prepared the previous week and transferred both of the filtrates using a 25 ml pipette into two erlenmeyer flasks. We then prepared the standard HCl by pipeting 100 ml of HCl to prepare 250 ml of 0.04M HCl from the 0.1 M HCl solution that we initially had. We pipeted 100 ml of HCl into a 250 ml volumetric flask and diluted to the mark. The buret was filled with the prepared HCl and both the CaCl and CaOH2 were titrated until a yellow endpoint was reached, this titration was repeated three times for each solution.

The result for solubility of Ca(OH)2= 0.1571

solubility for CaCl2=0.1299

Q. Do you expect the solubility product of CaCl and CaOH2 after titration with HCl to be consistent or inconsistent? Explain why.