contestada

What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18°C? [R = 0.08206 L • atm/K • mol]

Respuesta :

Answer:

P = 17.9618 atm

Explanation:

The osmotic pressure can be calculated and treated as if we are talking about an ideal gas, and it's expression is the same:

pV = nRT

However the difference, is that instead of using moles, it use concentration so:

p = nRT/V ----> but M = n/V so

p = MRT

We have the temperature of 18 °C (K = 18+273.15 = 291.15 K) the value of R = 0.08206 L atm / K mol, so we need to calculate the concentration, and we have the mass of HCl, so we use the molar mass of HCl which is 36.45 g/mol:

n = 13.7/36.45 = 0.3759 moles

M = 0.3759/0.5 = 0.7518 M

Now that we have the concentration, let's solve for the osmotic pressure:

p = 0.7518 * 0.08206 * 291.15

p = 17.9618 atm

Eduard22sly

The osmotic pressure of the solution is 35.82 atm.

We'll begin by calculating the number of mole of HCl.

  • Mass = 13.7 g
  • Molar mass of HCl = 1 + 35.5 = 36.5 g/mol
  • Mole of HCl =?

Mole = mass / molar mass

Mole of HCl = 13.7 / 36.5

Mole of HCl = 0.375 mole

Next, we shall determine the molarity of the HCl solution.

  • Mole of HCl = 0.375 mole
  • Volume = 0.5 L
  • Molarity of HCl =?

Molarity = mole / Volume

Molarity of HCl = 0.375 / 0.5

Molarity of HCl = 0.75 M

Finally, we shall determine the osmotic pressure of the solution.

  • Molarity (M) = 0.75 M
  • Temperature (T) = 18 °C = 18 + 273 = 291 K
  • Van't Hoff's factor (i) = 2 (electrolyte)
  • Gas constant (R) = 0.08206 atm.L/Kmol
  • Osmotic pressure (π) =?

π = iMRT

π = 2 × 0.75 × 0.08206 × 291

π = 35.82 atm

Therefore, the osmotic pressure of the solution is 35.82 atm

Learn more about osmotic pressure:

https://brainly.com/question/25904085

Otras preguntas