Recent questions tagged additionalproblem

Calculate the mole fraction of ethylene glycol $(C_2H_6O_2)$ in a solution containing 20% of $C_2H_6O_2$ by mass.

asked Aug 8, 2014 by sreemathi.v

1 answer

At 300K,36g of glucose present per litre in its solution has an osmotic pressure of 4.98 bar.If osmotic pressure of solution is 1.52 bar at the same temperature,what would be its concentration?

asked Aug 8, 2014 by sreemathi.v

1 answer

What is the mole fraction of a solute,in 2.5m aqueous solution?

asked Aug 8, 2014 by sreemathi.v

1 answer

A 4% solution of sucrose is isotonic with 3% solution of an unknown organic substance.Calculate the molecular mass of unknown substance .

asked Aug 8, 2014 by sreemathi.v

1 answer

A 0.1539 molal aqueous solution of cane sugar (mol mass =$342gmol^{-1}$) has a freezing point of 271K while the freezing point of pure water is $273.15K$.What will be the freezing point of an aqueous solution containing 5g of glucose (mol mass =$180gmol^{-1}$) per 100g of solution.

asked Aug 8, 2014 by sreemathi.v

1 answer

The freezing point of a solution containing 0.2g of acetic acid is 20.0g of benzene is lowered by $0.45^{\large\circ}$C.Calculate Van't Hoff factor .[For benzene,$K_f=5.12Kkg mol^{-1}]$.What conclusion can you draw from the value of Van't Hoff factor obtained.

asked Aug 8, 2014 by sreemathi.v

1 answer

The freezing point of a solution containing 0.2g of acetic acid is 20.0g of benzene is lowered by $0.45^{\large\circ}$C. Calculate the molar mass of acetic acid from this data?[For benzene,$K_f=5.12Kkg mol^{-1}]$

asked Aug 8, 2014 by sreemathi.v

1 answer

0.5g KCl was dissolved in 100g water and the solution originally at $20^{\large\circ}C$,froze at $-0.24^{\large\circ}C$.Calculate the percentage ionization of salt.$(K_f$ per 1000g of water =1.86K)

asked Aug 8, 2014 by sreemathi.v

1 answer

What concentration of nitrogen should be present in a glass of water at room temperature.Assume a temperature of $25^{\large\circ}C$,a total pressure of atmosphere and mole fraction of nitrogen in air of 0.78.[$K_H$ for nitrogen =$8.42\times 10^{-7}$M/mm Hg]

asked Aug 8, 2014 by sreemathi.v

1 answer

100 mg of a protein is dissolved in enough water to make 10.0mL of a solution.If this solution has an osmotic pressure of 13.3 mm Hg at $25^{\large\circ}C$.What is the molar mass of protein.

asked Aug 8, 2014 by sreemathi.v

1 answer

Calculate the molarity and molality of a 15% solutions (by weight) of sulphuric acid density $1.020g cm^{-3}$.(Atomic masses H=10=16S=32 amu)

asked Aug 8, 2014 by sreemathi.v

1 answer

A solution containing,8g of a substance in 100g of diethyl ether boils at $36.86^{\large\circ}C$,whereas pure ether boils at $35.60^{\large\circ}C$.Determine the molecular mass of the solute.(For ether $K_b=2.02kg mol^{-1})$

asked Aug 8, 2014 by sreemathi.v

1 answer

A 6.90 M solution of KOH in water contains 30% by mass of KOH.Calculate the density of the KOH solution ?[Molar mass of KOH=$56g mol^{-1}$]

asked Aug 8, 2014 by sreemathi.v

1 answer

Urea forms an ideal solution in water .Determine the vapour pressure of aqueous solution containing 10% by mass of urea of $40^{\large\circ}C$.(Vapour pressure of water,at $40^{\large\circ}C$=55.3 mm Hg)

asked Aug 8, 2014 by sreemathi.v

1 answer

Calculate the freezing point of a solution containing 0.520g glucose $(C_6H_{12}O_6)$ dissolved in 80.20g of water.For water $K_f=1.86Kkg mol^{-1}$

asked Aug 8, 2014 by sreemathi.v

1 answer

A 0.2 percent aqueous solution of a non-volatile solute exerts vapour pressure of $1.004$ bar at $100^{\large\circ}$C.What is the molar mass of the solute?

asked Aug 8, 2014 by sreemathi.v

1 answer

Ethylene glycol (molar mass =$62g mol^{-1})$ is a common automobile antifreeze.Calculate the freezing point of a solution containing 12.4 of this substance in 100g of water would it be advisable to keep this substance in the car radiator during summer?

asked Aug 8, 2014 by sreemathi.v

1 answer

The freezing point of 0.02 mole fraction solution of acetic acid in benzene is 277.4K.Assuming molality equal to molarity,calculate $K_c$ for the equilibrium reaction $2CH_3COOH\;\;\leftrightharpoons\;\;(CH_3COOH)_2$.Given : $T_f$(benzene) =$278.4$ and $K_f$(benzene)=5.0K kg $mol^{-1}$.

asked Aug 8, 2014 by sreemathi.v

1 answer

100mg of a protein is dissolved in just enough water to make 10.0mL of solution.If this solution has an osmotic pressure of 13.3mm Hg at $25^{\large\circ}C$,what is the molar mass of the protein?(R=0.0821Latm $mol^{-1}K^{-1}$,760mm Hg =1atm)

asked Aug 8, 2014 by sreemathi.v

1 answer

Calculate the freezing point depression expected for 0.0711m aqueous solution of $Na_2SO_4$.If this solution actually freezes at $-320^{\large\circ}C$,what would be the value of van't Hoff factor? ($K_f$ for water is $1.86^{\large\circ}Cmol^{-1}$)

asked Aug 8, 2014 by sreemathi.v

1 answer

The boiling point elevation of 0.30g acetic acid in 100g benzene is 0.0633K.Calculate the molar mass of acetic acid from this data?What conclusion can you draw about the molecular state of the solute in the solution?[Given $K_b$ for benzene = $2.53\;K kgmol^{-1}]$

asked Aug 7, 2014 by sreemathi.v

1 answer

Calculate the temperature at which a solution containing 54g of glucose,$C_6H_{12}O_6$ in 250g of water will freeze ($K_f$ for water =$1.86K kg mol^{-1}$)

asked Aug 7, 2014 by sreemathi.v

1 answer

If boiling point of an aqueous solution is $100.1^{\large\circ}$C.What is its freezing point?Given,latent heat of fusion and vaporisation of water as 80 cal $g^{-1}$ and 540 cal $g^{-1}$ respectively.

asked Aug 7, 2014 by sreemathi.v

1 answer

The legal limit for human exposure to CO in the work place is 35ppm.Assuming that the density of air is $1.3g/L$,how many grams of CO are in 1.0L of air at the maximum allowable concentration?

asked Aug 7, 2014 by sreemathi.v

1 answer

A soda water bottle was opened and the soft drink is allowed to come at $27^{\large\circ}$C with the air containing carbon dioxide at $3.8\times 10^{-4}$atm.What would be the concentration of carbon dioxide in the soda water after it had stood open and come to equilibrium.Give value of Henry's constant for aqueous solution of carbon dioxide at $26^{\large\circ}$C is $3.1\times 10^{-2}$ mol lit $^{-1}$ atm$^{-1}$.

asked Aug 7, 2014 by sreemathi.v

1 answer

The Freezing point of ether was lowered by $0.60^{\large\circ}$C on dissolving 2.0gm of phenol in 100g of ether.Calculate the molar mass of phenol and comment on the result.Given $K_f$(ether)=$5.12Kkg mol^{-1}$

asked Aug 7, 2014 by sreemathi.v

1 answer

The molal elevation constant for water is $0.510Kmol^{-1}kg$.Calculate the boiling point of solution made by dissolving 6g urea in 200g water.

asked Aug 7, 2014 by sreemathi.v

1 answer

The freezing point of a solution containing 0.2g of acetic acid in 20.0g benzene is lowered by $0.45^{\large\circ}$C.Calculate the degree of association of acetic acid in benzene.Assume acetic acid dimerizes in benzene $K_f$ for benzene is $5.12Kmol^{-1}kg$.

asked Aug 7, 2014 by sreemathi.v

1 answer

Calculate the freezing point of an aqueous solution of a non-electrolyte having an osmotic pressure 2.0atm at 300K.$K_f=1.86Kmol^{-1}kg$ and $S=0.0821$litre atm $K^{-1}mol^{-1}$

asked Aug 7, 2014 by sreemathi.v

1 answer

Two liquids A and B form ideal solution.At 300K,the vapour pressure of solution containing 1 mol of A and 3 mol of B is 550mm Hg.At the same temperature,if one more mole of B is added to this solution,the vapour pressure of the solution increases by 10mm Hg.Determine the vapour pressures of A and B in their pure states.

asked Aug 7, 2014 by sreemathi.v

1 answer

A very small amount of a non-volatile solute (that does not dissociate) $P_s$ dissolved in $56.8cm^3$ of benzene (density =$0.889gcm^{-3}$).At room temperature,vapour pressure of this solution is 98.88mm Hg while that benzene is 100mm Hg.Find the molality of this solution.If the freezing temperature of this solution is 0.73 degree lower than that of benzene,what is the value of $K_f$ for benzene .

asked Aug 7, 2014 by sreemathi.v

1 answer

Calculate the weight of a non volatile solute having molecular weight 40,which should be dissolved in 114gm octane to reduce its vapour pressure to 80%.

asked Aug 7, 2014 by sreemathi.v

1 answer

The degree of dissociation of $Ca(NO_3)_2$ in a dilute aqueous solution containing 7g of salt per 100g of water at $100^{\large\circ}$C is 70%.Calculate the vapour pressure of solution.

asked Aug 7, 2014 by sreemathi.v

1 answer

$0.1M$ $KMnO_4$ is used for the following titration $S_2O_3^{2-}+KMnO_4^-+H_2O\rightarrow MnO_2(s)+SO_4^{2-}+OH^-$.What volume of the solution in mL will be required to react with 0.158 of $Na_2S_2O_3?

asked Aug 7, 2014 by sreemathi.v

1 answer

Find the molality of a solution containing a non-volatile solute if the vapour pressure is 2% below the vapour pressure of pure water.

asked Aug 7, 2014 by sreemathi.v

1 answer

The vapour pressure of pure benzene at $25^{\large\circ}C$ is 639.7mm of mercury and the vapour pressure of a solution of a solute in benzene at the same temperature is $631.9$mm of mercury.Calculate the molality of the solution.

asked Aug 7, 2014 by sreemathi.v

1 answer

How many millilitres of 0.5M $H_2SO_4$ are needed to dissolve 0.5g of copper (II) carbonate ?

asked Aug 7, 2014 by sreemathi.v

1 answer

Molarity of $H_2SO_4$ is 18M.If density is $1.8gcm^{-3}$,calculate its concentration in $mol kg^{-1}$ solvent $(H_2O)$ (ie) Molality.

asked Aug 7, 2014 by sreemathi.v

1 answer

An antifreeze solution is prepared from 222.6 of ethylene glycol and 200g of water.If the density of the solution is $1.072gmL^{-1}$,then what shall be the molarity of solution.

asked Aug 7, 2014 by sreemathi.v

1 answer

An antifreeze solution is prepared from 222.6 of ethylene glycol and 200g of water.Calculate the molality of the solution.

asked Aug 7, 2014 by sreemathi.v

1 answer

The freezing point of 0.02mole fraction solution of acetic acid in benzene is 277.4K.Assuming molality equal to molarity,calculate $K_c$ for the equilibrium reaction $2CH_3COOH \;\;\leftrightharpoons\;\;(CH_3COOH)_2$.

asked Aug 6, 2014 by sreemathi.v

1 answer

To $500cm^3$ of water $3.0\times 10^{-3}$kg of acetic acid is added .If 2.3% of acetic acid is dissociated.What will be the depression of freezing point?$K_f$ and density of water are $1.86$K kg/mol and $0.997g/cm^3$ respectively.

asked Aug 6, 2014 by sreemathi.v

1 answer

The freezing point of a solution containing 0.2g of acetic acid in 20.0g benzene is lowered by $0.45^{\large\circ}$C.Calculate the degree of association of acetic acid in benzene.Assume acetic acid dimerises in benzene.$K_f$ for benzene =$5.12Kmol^{-1}Kg$

asked Aug 6, 2014 by sreemathi.v

1 answer

If boiling point of an aqueous solution is 100.1$^{\large\circ}C$,what is its freezing point.Given,latent heat of fusion and vaporization of water as $80cal g^{-1}$ and $540cal g^{-1}$ respectively.

asked Aug 6, 2014 by sreemathi.v

1 answer

A very small amount of a non-volatile solute (that does not dissociate) is dissolved in $56.8cm^3$ of benzene (density $=0.889gcm^{-3}$).At room temperature vapour pressure of this solution is 98.88mm Hg while that of benzene is 100 mm Hg.Find the molality of this solution.If the freezing temperature of this solution is 0.73 degree lower than that of benzene .What is the value of $K_f$ for benzene?

asked Aug 6, 2014 by sreemathi.v

1 answer

Find the molality of a solution containing a non-volatile solute if the vapour pressure is 2% below the vapour pressure of pure water.

asked Aug 6, 2014 by sreemathi.v

1 answer

A 5% solution (wt/volume) of cane sugar is isotonic with 0.877% (wt/volume) of urea solution.Find the molecular weight of urea,if molecular weight of sugar is 342.

asked Aug 6, 2014 by sreemathi.v

1 answer

The Henry's law constant for oxygen dissolved in water is $4.34\times 10^4$ atm at $25^{\large\circ}$C.If the partial pressure of oxygen in air is 0.2atm,under atmospheric conditions,calculate the concentration (in moles per litre) of dissolve oxygen in water in equilibrium with air at $25^{\large\circ}$C.

asked Aug 6, 2014 by sreemathi.v

1 answer

The solubility of oxygen in water is $2.43\times 10^{-3}$ mole/litre at $25^{\large\circ}$C and 1.0atm pressure.Calculate the concentration of oxygen at $25^{\large\circ}$C and 0.2atm pressure.

asked Aug 6, 2014 by sreemathi.v

1 answer

Calculate the molarity of water if its density is $1000g/m^3$

asked Aug 6, 2014 by sreemathi.v

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