Asolution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 l of solution. the osmotic pressure of this solution is 0.750 atm at 25.0°c. what is the molecular weight (g/mol) of the unknown solute? g

The molar mass of unknown solute is 195.44 g/mol.

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

where,

= osmotic pressure of the solution = 0.750 atm

i = Van't hoff factor = 1 (for non-electrolytes)

c = concentration of solute = ?

R = Gas constant =

T = temperature of the solution =

Putting values in above equation, we get:

The concentration of solute is 0.0307 mol/L

This means that, 0.0307 moles are present in 1 L of solution.

To calculate the molecular mass of solute, we use the equation:

Moles of solute = 0.0307 mol

Given mass of solute = 6g

Putting values in above equation, we get:

Hence, the molar mass of unknown solute is 195.44 g/mol.

the dissociation of nickel hydroxide is follows:

the concentration of hydroxide ion is

the equilibrium constant value of nickel hydroxide is = 6.1 * 10^-^1^6 and thus equilibrium equation can be written as:

thus, concentration of ni is 0.23 * 10^-^4 mol /l