Multiple Choice
If a 3.90 m solution boils at 103.45 °C, what is the actual value of the van't Hoff factor, i, given that the boiling point of pure water is 100.00 °C and the ebullioscopic constant (Kb) is 0.512 °C/m?
14. Solutions
Boiling Point Elevation
Multiple Choice
At an elevation of 1.45×10^4 ft, what is the approximate boiling point of water?
A
105°C
B
100°C
C
95°C
D
90°C
Verified step by step guidance1
Understand that the boiling point of water decreases with an increase in altitude due to lower atmospheric pressure.
Recall that at sea level (1 atm pressure), the boiling point of water is 100°C.
Recognize that at higher elevations, such as 1.45×10^4 ft, the atmospheric pressure is lower, which causes the boiling point to decrease.
Use the general rule of thumb that for every 500 ft increase in elevation, the boiling point of water decreases by approximately 0.5°C.
Calculate the decrease in boiling point by dividing the elevation (1.45×10^4 ft) by 500 ft and multiplying the result by 0.5°C to find the approximate boiling point at this elevation.
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