# The normal boiling point of water, H2O is 100.00 °C and its Kbp value is 0.512 °C/m. Assuming complete dissociation of the electrolyte, if 13.47 grams of cobalt(II) chloride (CoCl2, 129.8 g/mol) are dissolved in 150.7 grams of water, what is the boiling point of the solution? Answer: ____ °C

Question
4 views

The normal boiling point of waterH2O is 100.00 °C and its Kbp value is 0.512 °C/m.

Assuming complete dissociation of the electrolyte, if 13.47 grams of cobalt(II) chloride (CoCl2129.8 g/mol) are dissolved in 150.7 grams of water, what is the boiling point of the solution?

check_circle

Step 1

The elevation in boiling point can be calculated as follows,

Given,

13.47g is converted into kilograms =0.01347kg of cobalt (II) chloride.

150.7g is converted into kilograms =0.1507kg of water.

The number of moles of cobalt (II) chloride in 1 kg of the solution is:

Step 2

The molality of cobalt (II) chloride in 1kg of the solution can be calculated as:

Step 3

The boiling point elevation constant of water is 0.512 oC.m/molal. Since cobalt (II) chloride dissociates into 3 ions, the Van’t Hoff factor for this compound is 3. Therefore, the boiling point elevation (ΔTb) can be calculated as follows:

ΔTb...

### Want to see the full answer?

See Solution

#### Want to see this answer and more?

Solutions are written by subject experts who are available 24/7. Questions are typically answered within 1 hour.*

See Solution
*Response times may vary by subject and question.
Tagged in