Title | Thermodynamics Worksheet.docx |
---|---|
Course | General Chemistry |
Institution | Concordia University Wisconsin |
Pages | 3 |
File Size | 126.2 KB |
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Lab Report...
Determining the Thermodynamics of Ca(OH)2 Dissolution in Water Names: Day and time of lab: Wednesday 01:00pm-03:00pm Date Experiment Performed: February 18 2020
Determining the solubility of Ca(OH)2 in room temperature water Temperature of the “room temperature” solution (21oC) Trial 1
Trial 2
10.00
10.00
10.00
Initial reading on buret, mL
0.10
0.00
0.00
Final reading on buret, mL
17.5
17.2
17.3
Volume of HCl used in titration, mL
17.4
17.2
17.3
[OH –] in room temperature saturated solution, M
4.23 × 10−2
4.40 × 10−2
4.26 × 10−2
Molar solubility (s) of Ca(OH)2 at room temperature, M
2.12 × 10−2
2.2 × 10−2
2.13 × 10−2
Volume of filtered Ca(OH)2 used in titration, mL
Average molar solubility of Ca(OH)2 at room temperature, M
2.15 × 10−2
Ksp for Ca(OH)2 at room temperature
3.97 × 10−5
ΔGofor the dissolution of Ca(OH)2 at
24.8
Trial 3
room temperature, kJ.mol-1
1
Determining the Thermodynamics of Ca(OH)2 Dissolution in Water Determining the solubility of Ca(OH)2 in boiling water Temperature of the boiling solution (98.1oC) Trial 1 Volume of filtered Ca(OH)2 used in titration, mL Initial reading on buret, mL
Trial 2
Trial 3
10.00
10.00
10.00
0.00
13.55
22.91
Final reading on buret, mL
9.43
22.91
31.98
Volume of HCl used in titration, mL
9.43
9.36
9.07
[OH –] in boiling saturated solution, M
2.29 × 10−2
2.25 × 10−2
2.21 × 10−2
Molar solubility (s) of Ca(OH)2 in boiling water, M
1.15 × 10−2
1.13 × 10−2
1.11 × 10−2
Average molar solubility of Ca(OH)2 in boiling water, M
1.13 × 10−2
Ksp for Ca(OH)2 at boiling
5.70 × 10−6
ΔGofor the dissolution of Ca(OH)2 in the
37.3
boilingsolution, kJ.mol-1
Other thermodynamic quantities: ΔSo, kJ.mol-1.K-1 ΔS = − 0.162kJ mol·K
ΔHo, kJ.mol-1 ΔH = − 22.8kJ mol
Example Calculations: 1. Show how you found the value of [OH –] in the room temperature solution. [OH ] M= −Lmol 17.4mL HCL × = 0.0174L HCL
1L
1000mL −
x
0.0243M OH =
0.0174L HCL −
0.0243M OH =x × 0.0174L HCL x = 0.000423mol OH− − 1000mL OH 10.00mL × = 0.0100L 1L 0.000423mol
OH−
x= 0.0100L x= 4.23 × 10−2 M OH− 2. Show how you found the molar solubility of Ca(OH)2 in the room temperature solution. −2 4.23 x 10−210 2
Molar Solubility of Ca(OH) = 2.12 x M Ca(OH) 2 = 2 3. Show how you found the Ksp value for Ca(OH)2 at room temperature. − −2 = Ave of [OH ] 4.30 x 10 Ksp = [OH ] 21 − 3eq Ksp = (4.30 x 10 ) 21 −2 3eq Ksp = 3.97 x 10−5 4. Show how you found the ΔGo value for the dissolution of Ca(OH)2 at room temperature. ΔG = − RTlnK kJ
−5
ΔG = − (0.008314 )(294K)(ln 3.97 x 10 ) K·mol kJ
ΔG = 24.8
mol
5. Show how you found ΔHo and ΔSofor the dissolution of Ca(OH)2. ΔS =ΔG 1− ΔG 2 ΔT 2 − ΔT 1 molkJ kJ
(24.771 − 37.255 )
ΔS = (371.1K − 294K) mol
ΔS = − 0.162kJ mol·K
ΔH = ΔG + TΔS mol + kJ
0kJ
ΔH = (24.8 ) (294K)(− .162 ) ΔH = − 22.8kJ mol mol·K...