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A solution is prepared by dissolving certain amount of solute in $500 g$ of water. The percentage by mass of a solute in solution is $2.38$ . Calculate mass of solute.

Important Questions on Solutions

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

Molality is defined as

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

5.2

molal aqueous solution of methyl alcohol,

{CH}_{3} OH

, is supplied. What is the mole fraction of methyl alcohol in the solution?

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

Calculate the mass percentage of

3 g

of solute

A

dissolved in

18 g

of water.

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

3.0 g

of oxalic acid

[{({CO}_{2} H)}_{2} \cdot 2 H_{2} O]

is dissolved in a solvent to prepare a

250 mL

solution. The density of the solution is

1.9 g / mL

. The molality and normality of the solution, respectively, are closest to

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

100 m L

of a water sample contains

0.81 g

of calcium bicarbonate and

0.73

g of magnesium bicarbonate. The hardness of this water sample expressed in terms of equivalents of

C a C O_{3}

is:
(molar mass of calcium bicarbonate is

162 g m m o l^{- 1}

and magnesium bicarbonate is

146 g m o l^{- 1})

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

Which of the following factors affect molarity of solution?

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

Which of the following statements is true?

$1$ ) $200 mL$ of $0.2 M$ $NaOH$ has a same number of moles of solute as $1000 mL$ of $1 M NaOH$ .
$2$ ) $200 mL$ of $1 M NaOH$ has a same number of moles as $1000 mL$ of $0.2 M NaOH$ .
$3$ ) $100 mL$ of $0.2 M NaOH$ has a same number of moles as $1000 mL$ of $1 M NaOH$ .
$4$ ) $2000 mL$ of $0.2 M NaOH$ has a same number of moles as $1000 mL$ of $1 M NaOH$ .

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

4.5 g

of compound

A (M . W . = 90)

was used to make

250 mL

of its aqueous solution. The molarity of the solution in

M

x \times 10^{- 1} .

The value of

x

is_____ (Rounded off to the nearest integer)

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

The mole fraction of urea in an aqueous urea solution containing

900 g

of water is

0.05

. If the density of the solution is

1.2 g {c m}^{- 3}

, the molarity of urea solution is _______. (Round off the answer to the nearest decimal)
(Given data: Molar masses of urea and water are

60 g {m o l}^{- 1}

and

18 g {m o l}^{- 1}

, respectively)

HARD

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

An antifreeze solution is prepared from

222.6 g

of ethylene glycol

(C_{2} H_{6} O_{2})

and

200 g

of water. Calculate the molality of the solution. If the density of the solution is

1.072 g {mL}^{- 1}

, then what shall be the molarity of the solution?

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

A mixture has

18 g

of water and

414 g

of ethanol. The mole fraction of water in the mixture is (assume ideal behaviour of the mixture)

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The molarity of a solution obtained by mixing

750 mL

0.5 (M) HCl

with

250 mL

2 (M) HCl

will be

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

Density of

3 M

solution of

NaCl

1.25 g / mL .

The mass of the solvent in the solution is;

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

3 \cdot 42 \times 10^{- 2} kg

Sugar (molar mass

342

) is dissolved in water to produce

234.2 g

of sugar syrup, what is the molality of sugar syrup ?

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

When the concentration is expressed as the number of moles of solute per kilogram of the solvent, it is known as;

EASY

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

The mole fraction of a solute in a $100$ molal aqueous solution ________ $\times 10^{- 2} .$

(Round off to the Nearest Integer).

[Given : Atomic masses: $H : 1.0 u, O : 16.0 u$ ]

HARD

Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

A $6.50$ molal solution of $KOH (aq .)$ has a density of $1.89 g {cm}^{- 3}$ . The molarity of the solution is $mol {dm}^{- 3}$ . (Round off to the Nearest Integer).

[Atomic masses: $K : 39.0 u; O : 16.0 u; H : 1.0 u$ ]

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

A solution of two components containing

n_{1}

moles of the

1^{st}

component and

n_{2}

moles of the

2^{nd}

component is prepared.

M_{1}

and

M_{2}

are the molecular weights of component 1 and 2 respectively. If

d

is the density of the solution in

{gml}^{- 1}, C_{2}

is the molarity and

x_{2}

is the mole fraction of the

2^{nd}

component, then

C_{2}

can be expressed as :

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

The mass percentage of nitrogen in histamine is ________

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Chemistry>Physical Chemistry>Solutions>Methods of Expressing Concentration of Solutions

The molarity of

{H N O}_{3}

in a sample which has density

1.4 g / m L

and mass percentage of

63 %

is ________ (Molecular Weight of

{H N O}_{3} = 63

)

A solution is prepared by dissolving certain amount of solute in 500 g of water. The percentage by mass of a solute in solution is 2.38. Calculate mass of solute.

Important Questions on Solutions

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A solution is prepared by dissolving certain amount of solute in $500 g$ of water. The percentage by mass of a solute in solution is $2.38$ . Calculate mass of solute.