Question

A solution containing 0.11 kg of Ba(NO3)2 in 0.1 kg of water boils at 100.46C calculate...

A solution containing 0.11 kg of Ba(NO3)2 in 0.1 kg of water boils at 100.46C calculate the degree of ionization of the salt (kb-0.5 kg.C/mol)?

Homework Answers

Answer #1

Boiling point elevation, deltaT= i* kb*m (1), kb=0.5 kg/deg.c/mole, i= van;t Hoff factor and

boiling point elevation = boiling point of solution- boiling point of water= 100.46-100=0.46 deg.c

m= molality= moles of Ba(NO3)2/ kg of solvent

moles= mass/ molar mass of Ba(NO3)2, molar mass of Ba(NO3)2= 261.34 g/mole

moles of Ba(NO3)2= 0.11 kg *1000g/kg/261.34 =0.42 moles

molality= moles of solute/ kg of solvent = 0.42/0.1= 4.2 moles of Ba(NO3)2/ kg of water

with these values, Eq.1 when used

0.46= i*0.5 kg/mole.deg.c* 4.2 moles/kg of water

i= 0.22,the degree of ionization

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A solution containing 1.5 g of barium nitrate, Ba(NO3)2 in 0.1 Kg of water freezes at...
A solution containing 1.5 g of barium nitrate, Ba(NO3)2 in 0.1 Kg of water freezes at -0.43 degrees Celsius. Calculate the apparent degree of dissociation of the salt. (Kb of water = 1.86 degrees Celsius
40g Ba(NO3)2 is dissolved in 1Kg of water ate 313.15K. a) Compute the equilibrium vapor pressure...
40g Ba(NO3)2 is dissolved in 1Kg of water ate 313.15K. a) Compute the equilibrium vapor pressure above the solution if none of the Ba(NO3)2 ionizes. Assume the solution behaves ideally in the Roult's law regime. The equilibrium vapor pressure above pure water at 313.15K is 55.324 torr. b) What would the vapor pressure be if barium nitrate ionizes completely? c) The actual vapor pressure is found to be 54.909 torr. Calculate the percent ionization for barium nitrate. d) Calculate Gmixing...
Calculate the molar solubility of Ba(IO3)2 in a solution that is also 0.0600 M in Ba(NO3)2....
Calculate the molar solubility of Ba(IO3)2 in a solution that is also 0.0600 M in Ba(NO3)2. (Ksp (Ba(IO3)2) = 1.57 x 10-9 )
10.5mg of solid NaF is added to a 50mL solution that is 0.0050M in Ba(NO3)2 and...
10.5mg of solid NaF is added to a 50mL solution that is 0.0050M in Ba(NO3)2 and 0.0050M in Pb(NO3)2​. For BaF2(S) Ksp= 1.7x10-6 and for PbF2(S) Ksp= 3.6x10-8. (1a) Write the equilibrium expression(s) for all possible reactions that could take place in this solution to form insoluble ionic salts: (1b) Calculate Qsp for each insoluble salt: (1c) What substance will precipitate from solution if more NaF were added? If so, at what concentration [F-]?
A solution is made by dissolving 15.1 g of barium hydroxide, Ba(OH)2, in enough water to...
A solution is made by dissolving 15.1 g of barium hydroxide, Ba(OH)2, in enough water to make exactly 100. mL of solution. Calculate the molarity of each species: Ba(OH)2 _______ mol/L Ba2+ _________ mol/L OH- _________ mol/L
A solution is made by dissolving 23.2g of Chromium (II) nitrate, CR(NO3)2, in enough water to...
A solution is made by dissolving 23.2g of Chromium (II) nitrate, CR(NO3)2, in enough water to make 250. ml of solution. Calculate the molartity of each species: Cr(NO3)2= mol/L Cr^2+= mol/L NO3- = mol/L
A chemist makes a solution of Mg(NO3)2 by dissolving 20.9 g Mg(NO3)2 in water to make...
A chemist makes a solution of Mg(NO3)2 by dissolving 20.9 g Mg(NO3)2 in water to make 100.0 mL of solution. What is the concentration of NO3− ions in the solution? Assume that Mg(NO3)2 is the only solute in the solution. The molar mass of Mg(NO3)2 is 148.33 g/mol.
Explain why the conductivity of 0.073 M Ba(NO3)2(aq) is greater than that of 0.073 M KBr(aq)....
Explain why the conductivity of 0.073 M Ba(NO3)2(aq) is greater than that of 0.073 M KBr(aq). A) The total ion concentration of the Ba(NO3)2 is greater than the KBr. In addition, some or all of the ions in Ba(NO3)2 have higher charge than those of KBr. Both of these factors increase the conductivity of the Ba(NO3)2 solution. B) Electrolytes with a NO3– anion will always have a higher conductivity when compared to any other electrolyte. Thus the Ba(NO3)2 will always...
A. If an aqueous solution is prepared with molality= 4.58 moles of glycerine/100 kg water, calculate...
A. If an aqueous solution is prepared with molality= 4.58 moles of glycerine/100 kg water, calculate the freezing point of the solution. Kf for water = 1.86C/m. (Glycerine is a molecular solute) b. if an aqueous solution is prepared with molality = 8.21 moles of magnesium chloride/100kg water, calculate the freezing point of the solution. Note : the ionic formula of this salt is MgCl2. C. Calculate the boiling pointof the solution described in question 2b. Given Kb for water=0.520C/m.
an aqueous solution of Ba(OH)2 by pipetting 25.00 mL of 0.0970 M Ba(NO3)2 into an Erlenmeyer...
an aqueous solution of Ba(OH)2 by pipetting 25.00 mL of 0.0970 M Ba(NO3)2 into an Erlenmeyer flask and that contains 25.00 mL of 0.105 M KOH. a) Calculate the molar concentrations of Ba2+(aq) and OH1-(aq) in their 50.00 mL solution. b) Use the molar concentrations of Ba2+(aq) and OH1-(aq) as determined above and the Ksp to show why a precipitate does not form. You must include a calculation as part of your answer. The value of Ksp for Ba(OH)2, is...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT