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Questions >> CBSE XII >> Chemistry >> Solutions

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

1 answer

A sample of sulphuric acid is 98% $H_2SO_4$ by weight (density =$1.10gmL^{-1})$.Calculate normality

asked Aug 6, 2014 by sreemathi.v

1 answer

A sample of sulphuric acid is 98% $H_2SO_4$ by weight (density =$1.10gmL^{-1})$.Calculate Molarity

asked Aug 6, 2014 by sreemathi.v

1 answer

1.8g of glucose (molar mass =180) are dissolved in 60g of water.Calculate the mole fraction of glucose and water

asked Aug 6, 2014 by sreemathi.v

1 answer

1.8g of glucose (molar mass =180) are dissolved in 60g of water.Calculate the molality

asked Aug 6, 2014 by sreemathi.v

1 answer

1.23g of sodium hydroxide (molar mass =40) are dissolved in water and the solution is made to $100cm^3$.Calculate the molarity of solution.

asked Aug 6, 2014 by sreemathi.v

1 answer

Determine the osmotic pressure of a solution prepared by dissolving 25 mg of $K_2SO_4$ in 2 litre of water at 25$^{\large\circ}$ C, assuming that it is completely dissociated.

asked Aug 6, 2014 by sreemathi.v

1 answer

Determine the amount of $CaCl_2$ (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27$^{\large\circ}$ C.

asked Aug 6, 2014 by sreemathi.v

1 answer

The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen at 298 K are $3.30 \times 10^7$ mm and $6.51 \times 10^7$ mm respectively, calculate the composition of these gases in water.

asked Aug 6, 2014 by sreemathi.v

1 answer

Benzene and toluene form ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at 300 K are 50.71 mm Hg and 32.06 mm Hg respectively. Calculate the mole fraction of benzene in vapour phase if 80 g of benzene is mixed with 100 g of toluene.

asked Aug 6, 2014 by sreemathi.v

1 answer

Vapour pressures of pure acetone and chloroform at 328 K are 741.8 mm Hg and 632.8 mm Hg respectively. Assuming that they form ideal solution over the entire range of composition, plot $p_{total}, p_{chloroform}$, and $p_{acetone}$ as a function of $x_{acetone}$. The experimental data observed for different compositions of mixture is:

asked Aug 6, 2014 by sreemathi.v

1 answer

100 g of liquid A (molar mass $140 g mol^{–1}$) was dissolved in 1000 g of liquid B (molar mass $180 g mol^{–1}$). The vapour pressure of pure liquid B was found to be 500 torr. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 torr.

asked Aug 6, 2014 by sreemathi.v

1 answer

Henry’s law constant for the molality of methane in benzene at 298 K is $4.27 \times 10^5$ mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.

asked Aug 6, 2014 by sreemathi.v

1 answer

Vapour pressure of water at 293 K is 17.535 mm Hg. Calculate the vapour pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water.

asked Aug 5, 2014 by sreemathi.v

1 answer

19.5 g of $CH_2FCOOH$ is dissolved in 500 g of water. The depression in the freezing point of water observed is 1.00$^{\large\circ}$ C. Calculate the van’t Hoff factor and dissociation constant of fluoroacetic acid.

asked Aug 5, 2014 by sreemathi.v

1 answer

Calculate the depression in the freezing point of water when 10 g of $CH_3CH_2CHClCOOH$ is added to 250 g of water. $K_a = 1.4 \times 10^{–3}, K_f = 1.86 K kg mol^{–1}$.

asked Aug 5, 2014 by sreemathi.v

1 answer

The depression in freezing point of water observed for the same amount of acetic acid, trichloroacetic acid and trifluoroacetic acid increases in the order given above. Explain briefly.

asked Aug 5, 2014 by sreemathi.v

1 answer

Calculate the amount of benzoic acid $(C_6H_5COOH)$ required for preparing 250 mL of 0.15 M solution in methanol.

asked Aug 5, 2014 by sreemathi.v

1 answer

Nalorphene $(C_{19}H_{21}NO_3)$, similar to morphine, is used to combat withdrawal symptoms in narcotic users. Dose of nalorphene generally given is 1.5 mg. Calculate the mass of $1.5 \times 10^{–3} m$ aqueous solution required for the above dose.

asked Aug 5, 2014 by sreemathi.v

1 answer

Calculate the mass percentage of aspirin ($C_9H_8O_4$) in acetonitrile ($CH_3CN$) when 6.5 g of $C_9H_8O_4$ is dissolved in 450 g of $CH_3CN$.

asked Aug 5, 2014 by sreemathi.v

1 answer

If the solubility product of CuS is $6 \times 10^{–16}$, calculate the maximum molarity of CuS in aqueous solution.

asked Aug 5, 2014 by sreemathi.v

1 answer

If the density of some lake water is $1.25g mL^{–1}$ and contains 92 g of $Na^+$ ions per kg of water, calculate the molality of $Na^+$ ions in the lake.

asked Aug 5, 2014 by sreemathi.v

1 answer

In the following compound, identify is it insoluble, partially soluble and highly soluble in water? Pentanol.

asked Aug 5, 2014 by sreemathi.v

1 answer

In the following compound, identify is it insoluble, partially soluble and highly soluble in water? $CHCl_3$

asked Aug 5, 2014 by sreemathi.v

1 answer

In the following compound, identify is it insoluble, partially soluble and highly soluble in water? Ethylene glycol

asked Aug 5, 2014 by sreemathi.v

1 answer

In the following compound, identify is it insoluble, partially soluble and highly soluble in water? Formic acid

asked Aug 5, 2014 by sreemathi.v

1 answer

In the following compound, identify is it insoluble, partially soluble and highly soluble in water? Toluene

asked Aug 5, 2014 by sreemathi.v

1 answer

In the following compound, identify is it insoluble, partially soluble and highly soluble in water? Phenol

asked Aug 5, 2014 by sreemathi.v

1 answer

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