Home
Class 12
CHEMISTRY
An aqueous solution containing 12.48g of...

An aqueous solution containing 12.48g of barium chloride in 1.0 kg of water boils at 373.0832 K. Calculate the degree of dissociation of barium chloride. [Given `K_(b)` for `H_(2)O =0.52 Km^(-1)`, Molar mass of `BaCl_(2) =208.34 "g mol"^(-1)`]

Text Solution

AI Generated Solution

To solve the problem of finding the degree of dissociation of barium chloride in an aqueous solution, we can follow these steps: ### Step 1: Calculate the elevation in boiling point (ΔT_b) The boiling point of pure water is 373.15 K. The boiling point of the solution is given as 373.0832 K. \[ \Delta T_b = T_b (\text{solution}) - T_b (\text{pure water}) = 373.0832 \, \text{K} - 373.15 \, \text{K} = -0.0668 \, \text{K} \] ...
Promotional Banner

Topper's Solved these Questions

  • SOLUTIONS

    ICSE|Exercise Follow up Problems |58 Videos

  • SOLUTIONS

    ICSE|Exercise EXERCISE (PART-I Objective Questions)|26 Videos

  • SOLID STATE

    ICSE|Exercise ISC EXAMINATION QUESTIONS PART-I (Numerical Problems)|6 Videos

  • SOME IMPORTANT ORGANIC NAME REACTIONS

    ICSE|Exercise Questions |278 Videos

Similar Questions

Explore conceptually related problems

A solution containing 1g of sodium chloride in 100g of water freezes at - 0.604^@C . Calculate the degree of dissociation of sodium chloride. (Na = 23, Cl = 35.5, Kf for water = 1.87 k "mol"^(-1) )

An aqueous solution of 3.12g of BaCl_(2) in 250g of water is found to boil at 100.0832^(@)C . Calculate the degree of dissociation of BaCl_(2) . Given that the value of K_(b)(H_(2)O)=0.52 K//m .

A solution containing 0.11kg of barium nitrate in 0.1kg of water boils at 100.46^(@)C . Calculate the degree of ionization of the salt. K_(b) (water) = 0.52 K kg mol^(-1) .

3.100 g of BaCl_(2) in 250g of water boils at 100.83^(@)C . Calculate the value of van't Hoff factor and molality of BaCl_(2) in this solution. ( K_(f) for water = 0.52 Km^(-1) , molar mass of BaCl_(2) = 208.3" g mol"^(-1) ).

An aqueous solution of glucose containing 12 g in 100 g of water was found to boil at 100.34^(@)C . Calculate of K_(b) for water in K mol^(-1)Kg .

A solution containing 0.85 g of ZnCl_(2) in 125.0g of water freezes at -0.23^(@)C . The apparent degree of dissociation of the salt is: (k_(f) for water = 1.86 K kg mol^(-1) , atomic mass, Zn = 65.3 and Cl = 35.5)

The freezing point of solution containing 0.2 g of acetic acid in 20.0 g of benzene is lowered by 0.45^(@)C . Calculate the degree of association of acetic acid in benzene. (K_(f)=5.12 K^(@) mol^(-1) kg^(-1))

The freezing point of solution containing 0.2 g of acetic acid in 20.0 g of benzene is lowered by 0.45^(@)C . Calculate the degree of association of acetic acid in benzene. (K_(f)=5.12 K^(@) mol^(-1) kg^(-1))

A solution containing 12.5 g of non-electrolyte substance in 185 g of water shows boiling point elevation of 0.80 K. Calculate the molar mass of the substance. ( K_b=0.52 K kg mol^(-1) )

A solution containg 12 g of a non-electrolyte substance in 52 g of water gave boiling point elevation of 0.40 K . Calculate the molar mass of the substance. (K_(b) for water = 0.52 K kg mol^(-1))