Home
Class 12
CHEMISTRY
Kb for diethylether is 2.16 K kg "mol"^(...

`K_b` for diethylether is 2.16 K kg `"mol"^(-1)`. Calculate the molar mass of solute when 0.4g of solute present in 40 g of ether, increased the boiling point of ether by 0.17 K.

Text Solution

AI Generated Solution

To solve the problem, we will use the formula for boiling point elevation and the definition of molality. Here’s a step-by-step breakdown: ### Step 1: Understand the given data - \( K_b \) (boiling point elevation constant for diethyl ether) = 2.16 K kg/mol - Mass of solute (solute) = 0.4 g - Mass of solvent (diethyl ether) = 40 g - Change in boiling point (\( \Delta T_b \)) = 0.17 K ...
Promotional Banner

Similar Questions

Explore conceptually related problems

A solution of an organic compound is prepared by dissolving 30 g in 100 g water. Calculate the molecular mass of compound and the osmotic pressure of solution at 300 K , when the elevation in boiling point is 0.52 and K_(b) for water is 0.52 K m^(-1) .

Calculate the boiling point of urea solution when 6 g of urea is dissolved in 200 g of water. ( K_(b) for water = 0·52 K kg mol^(-1) , boiling point of pure water = 373 K, mol.wt. of urea = 60)

If 1 g of solute (molar mass = 50 g mol^(-1) ) is dissolved in 50 g of solvent and the elevation in boiling point is 1 K. The molar boiling constant of the solvent is

The boiling point of pure water is 373 K. calculate the boiling point of an aqueous solution containing 18 g of glucose (M.W. = 180) in 100g of water. Molal elevation constant of water is 0.52 K kg "mol"^(-1) .

(a) A solution containing 0.5g of naphithalene in 50g C Cl_(4) yield a boiling point elevation of 0.4K , while a solution of 0.6g of an unknown solute in the same mass of the solvent gives a boiling point elevation of 0.65K . Find the molar mass of the unknown solute. (b) The boiling point of a solution of 0.1g of a substance in 16g of ether was found to be 0.100^(@)C higher that of pure ether. What is the molecular mass of the substance. K_(b) (ether) =2.16K kg "mol"^(-1)

The freezing point of ether was lowered by 0.60^(@)C on dissolving 2.0g of phenol in 100g of ether. Calculate the molar mass of phenol and comment on the result. Given: K_(f) (ether) = 5.12 K kg mol^(-1) .

A solution of sucrose (molar mass =342 g mol^(-1) ) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The depression in freezing point of the solution obtained will be ( K_(f) for water = 1.86K kg mol^(-1) )

A solution was prepared by dissolving 6.0 g an organic compound in 100 g of water. Calculate the osmotic pressure of this solution at 298 K ,when the boiling point of the Solution is 100.2^(@)C . ( K_(b) for water = 0.52 K m^(-1) ), R=0.082 L atm K^(_1) mol^(-1) )

(a) Define the terms osmosis and osmotic pressure. Is the osmotic pressure of a solution a colligative property? Explain. (b) Calculate the boiling point of a solution prepared by adding 15.00g of NaCl to 250.0g of water. ( K_(b) for water =0.512K kg "mol"^(-1) , Molar mass of NaCl=58.44g )