Home
Class 12
CHEMISTRY
Calculate molality of 3.5g of ethanoic a...

Calculate molality of 3.5g of ethanoic acid `(CH_(3)COOH)` in 75 g of benzene.

Text Solution

AI Generated Solution

To calculate the molality of ethanoic acid (CH₃COOH) in benzene, we can follow these steps: ### Step 1: Determine the mass of the solute and the solvent. - Mass of ethanoic acid (solute) = 3.5 g - Mass of benzene (solvent) = 75 g ### Step 2: Calculate the number of moles of the solute. To find the number of moles of ethanoic acid, we use the formula: ...
Promotional Banner

Topper's Solved these Questions

  • AMINES

    AAKASH INSTITUTE ENGLISH|Exercise Assignment Section -J (Aakash Challengers Questions)|9 Videos

  • AMINES

    AAKASH INSTITUTE ENGLISH|Exercise Assignment Section - H (Multiple True-False Type Questions)|2 Videos

  • ALDEHYDES, KETONES AND CARBOXYLIC ACIDS

    AAKASH INSTITUTE ENGLISH|Exercise Try Yourself|20 Videos

  • BIOMOLECULES

    AAKASH INSTITUTE ENGLISH|Exercise EXERCISE (ASSIGNMENT) SECTION - D Assertion - Reason Type Questions|5 Videos

Similar Questions

Explore conceptually related problems

Calculate molality of 2.5g of ethanoic acid (CH_(3)COOH) in 75 g of benzene.

Pure benzene freezes t 5.3^(@)C . A solution of 0.223 g of phenylacetic acid (C_(6)H_(5)CH_(2)COOH) I 4.4 g of benzene (K_(f) = 5.12 Kkg mol^(-1)) freezes at 4.47^(@)C . From the observation one can conclude that :

Two grams of benzoic acid (C_(6)H_(5)COOH) dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K . Molal depression constant for benzene is 4.9 K kg^(-1)"mol^-1 . What is the percentage association of acid if it forms dimer in solution?

Two grams of benzoic acid (C_(6)H_(5)COOH) dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K . Molal depression constant for benzene is 4.9 K kg^(-1)"mol^-1 . What is the percentage association of acid if it forms dimer in solution?

Calculate pH of 0.05 M Acetic acid solution , if K_(a)(CH_(3)COOH) = 1.74 xx 10^(-5) .

The freezing point of a solution of 2.40 g of biphenyl ( C_(12)H_(10) ) in 75.0 g of benzene ( C_(6)H_(6) ) is 4.40^(@)C . The normal freezing point of benzene is 5.50^(@)C . What is the molal freezing point constant (@C//m) for benzene ?

2g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25g of benzene shows a depression in freezing point equal to 1.62K .Molal depression constant for benzene is 4.9Kkgmol^(-1) .What is the percentage association of acid if it forms dimer in solution?

2g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25g of benzene shows a depression in freezing point equal to 1.62K .Molal depression constant for benzene is 4.9Kkgmol^(-1) .What is the percentage association of acid if it forms dimer in solution?

The freezing point of a solution contaning 0.3 g of acetic acid in 43 g of benzene reduces by 0.3^(@) . Calculate the Van's Hoff factor "( K_(f) for benzene = 5.12 K kg mol^(-1) )"

A solution is prepared by adding 64 g of CH_(3)OH to 180 g of water. Calculate the mole fraction of CH_(3)OH . (Molar mass of CH_(3)OH = 32 g ) .