MHT CET 202625 AprilEvening Shift
- Exam
- MHT CET
- Year
- 2026
- Date
- 25 April
- Shift
- Evening Shift
- Subject
- Chemistry
- Chapter
- Solutions
MHT CET 2026 · 25 April · Evening Shift · Chemistry · Solutions
What is boiling point of solution containing 7.45\ g of KCl in 500\...
What is boiling point of solution containing of in of water, assuming dissociation of ? (molar mass of , for water )
Options
- A99.8128\ ^{}^{\circ}\text{C}
- B100.1872\ ^{}^{\circ}\text{C}
- C100.0936\ ^{}^{\circ}\text{C}
- D100.3744\ ^{}^{\circ}\text{C}
Correct answer
B. 100.1872\ ^{}^{\circ}\text{C}
Step-by-step solution
Molality of the solution is given by:
For , the dissociation reaction is .
The van't Hoff factor is:
Since and :
The elevation in boiling point is:
\Delta T_b = 1.8 \times 0.52 \times 0.2 = 0.1872\ ^{}^{\circ}\text{C}
The boiling point of the solution is:
T_b = 100\ ^{}^{\circ}\text{C} + \Delta T_b = 100\ ^{}^{\circ}\text{C} + 0.1872\ ^{}^{\circ}\text{C} = 100.1872\ ^{}^{\circ}\text{C}
Answer: 100.1872\ ^{}^{\circ}\text{C}
For , the dissociation reaction is .
The van't Hoff factor is:
Since and :
The elevation in boiling point is:
\Delta T_b = 1.8 \times 0.52 \times 0.2 = 0.1872\ ^{}^{\circ}\text{C}
The boiling point of the solution is:
T_b = 100\ ^{}^{\circ}\text{C} + \Delta T_b = 100\ ^{}^{\circ}\text{C} + 0.1872\ ^{}^{\circ}\text{C} = 100.1872\ ^{}^{\circ}\text{C}
Answer: 100.1872\ ^{}^{\circ}\text{C}