A solution of citric acid, C6H8O7, in 50.0 g of acetic acid has a boiling point elevation of ΔT = 1.76 °C. What is the molality of the solution if the molal boilin# g-point-elevation constant for acetic acid is Kb = 3.07 1°C kg2>mol.

Video transcript

Hey everyone, we're told that a solution of ascorbic acid was repaired in 100 and 80 g of water. The solution was found to have a boiling point of 100 and 1.25 degrees Celsius. Find the morality of the solution. Given that the value of K. B, which is our base association constant for water is 0.52 degrees Celsius times kilogram per mole. So here they've given us the boiling point of our solution And we know that the boiling point of water is 100°C. So we can go ahead and solve for the boiling point elevation, which is the boiling point of our solution minus the boiling point of our pure solvent. Now plugging in these values, we have 100 and 1.25 degrees Celsius for our boiling point solution And we're going to subtract 100°C. This gets us to a boiling point elevation Of 1.25°C. Now that we have this value, we can go ahead and use this for the following formula, which is the elevation of boiling point is equal to our KB times our morality. So plugging in our values, we know that our boiling point elevation is 1.25°C And this is going to be equal to our KB, which was said to be 0.52°C times kilogram per mole. And this is going to be multiplied by our morality, solving for morality, we're going to divide both sides By 0.52°C kilogram per mole And this will get us to a morality of 2. moles per kilogram, which is going to be our final answer. Now, I hope this made sense and let us know if you have any questions.