Compute the boiling point of this Solution:

25.5g C7H11NO7S (4-nitro-2-toluenesulfonoic acid dihydrate) in 1.00*10^2g H2O (nonionizing solute)

The freezing point of H2O is lowered 1.86 Celsius per mole of solute.

The boiling pint os H2O is raised 0.512 Celsius per mole of solute.

To compute the boiling point of the solution, you need to determine the change in boiling point based on the molality of the solute.

1. Calculate the molality of the solute:
Molality (m) = moles of solute / mass of solvent (in kg)

First, convert the given mass of C7H11NO7S to moles:
molar mass of C7H11NO7S = 227.24 g/mol
moles of C7H11NO7S = 25.5 g / 227.24 g/mol

Next, convert the given mass of H2O to kilograms:
mass of H2O = 100 g = 0.1 kg

Now, compute the molality:
m = moles of C7H11NO7S / mass of H2O
m = (25.5 g / 227.24 g/mol) / 0.1 kg

2. Calculate the change in boiling point:
ΔTb = Kb × m

Given that the boiling point elevation constant (Kb) for water is 0.512 °C/molal (given in the question), and you have already calculated the molality (m) in step 1.

ΔTb = 0.512 °C/molal × m

3. Calculate the boiling point of the solution:
Boiling point of the solution = boiling point of pure solvent + ΔTb

The boiling point of pure water is 100 °C. Since the change in boiling point (ΔTb) is positive, it raises the boiling point.

Boiling point of the solution = 100 °C + ΔTb

Now you can substitute the calculated values into the equation to obtain the boiling point of the solution.

To compute the boiling point of the given solution, we need to use the boiling point elevation formula.

The boiling point elevation formula is given by:

ΔTb = Kbm

Where:
ΔTb is the boiling point elevation
Kb is the molal boiling point elevation constant (0.512 °C/m for water)
m is the molality of the solution (mol solute/kg solvent)

To find the molality (m), we need to calculate the number of moles of solute and the mass of the solvent.

First, let's calculate the number of moles of solute (C7H11NO7S):
Given mass of C7H11NO7S = 25.5 g
Molar mass of C7H11NO7S = 257.24 g/mol

Number of moles of C7H11NO7S = mass / molar mass
= 25.5 g / 257.24 g/mol

Next, we calculate the mass of the solvent (H2O):
Given mass of H2O = 1.00 x 10^2 g

Now, we find the molality (m):
molality (m) = moles of solute / mass of solvent (in kg)
= moles of solute / (mass of solvent / 1000)

Finally, we substitute the values in the boiling point elevation formula to find the boiling point elevation (ΔTb). Since we are given the freezing point depression, we can find the boiling point elevation by doubling the value:

Boiling point elevation (ΔTb) = 2 * (Kb * m)

Now we can calculate the boiling point elevation and add it to the boiling point of pure water (100 °C) to find the boiling point of the solution.

25.5 g CËÈHËËNOËÈS

(4-nitro-2-toluenesulfonoic acid dihydrate) in 1.00 X 10³ g HËÃ0 (nonionizing solute)

25.5 g c7h11no7s