Concentration Terms

Q.

Calculate molar mass of CO(NO3)2.6H2O

Q.

A 5% solution (by mass) of cane sugar in water has freezing point of 271 K. Calculate the freezing point of 5% glucose in water if freezing point of pure water is 273.15 K.

Q.

The partial pressure of ethane over a solution containing 6.56 × 10⁻³ g of ethane is 1 bar. If the solution contains 5.00 × 10⁻² g of ethane, then what shall be the partial pressure of the gas?

Q.

Differentiate between molarity and molality of a solution. How can we change the molality value of a solution into a molarity value?

Q. Calculate molality of 2.5 g of ethanoic acid $\left[C{H}_{3}COOH\right]$ in 75 g of benzene.

1. $0.552molk{g}^{-1}$
2. $0.556molk{g}^{-1}$
   
3. $0.551molk{g}^{-1}$
   
4. $0.558molk{g}^{-1}$
   

Q.

Fresh fruit contains 68% of water and dry fruit contains 20% of water. Then how much dry fruits have in 100 kilograms of fresh fruits?

Q.

Calculate the total number of electrons in 18 ml of water

Q.

Calculate the mass of oxalic acid (${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4.2{\mathrm{H}}_2\mathrm{O}$) needed to prepare 250 ml, 1 M aqueous solution of oxalic acid.

Q.

How does Temperature affect Molarity and Molality?

Q. Of the following four aqueous solution, total number of those solutions whose freezing point is lower than that of $0.10M{C}_2{H}_{5}OH$ is/are (integer answer)
$\left(i\right)0.10MB{a}_3\left(P{O}_4{)}_2\right(ii\left)0.10MN{a}_{2}S{O}_4\right(iii\left)0.10MKCl\right(iv)0.10ML{i}_{3}P{O}_4$

Q.

The amount of anhydrous Na₂CO₃ present in 250 ml of 0.25 M solution is

1. 6.625 g

2. 6.225 g

3. 66.25 g

4. 6.0 g

Q.

When 20 g of naphthoic acid (C11H8O2) is dissolved in 50g of benzene (Kf = 1.72 K kg mol-1), a freezing point depression of 2K is observed. The van't Hoff factor (i) is -

1. 0.5

2. 2

3. 3

4. 1

Q.

Which of the following is dependent on temperature?

1. Molarity

2. Mole fraction

3. Weight percentage

4. Molality

Q. The mole fraction of a solute in a solution is 0.1. At 298 K, molarity of this solution is the same as its molality. Density of this solution at 298 K is 2.0 g $c{m}^{-3}$. The ratio of the molecular weights of the solute and solvent, $\left(\frac{M{W}_{solute}}{M{W}_{solvent}}\right)$, is

Q.

From 392 mg of H2SO4 , 1.204 *10^21 molecules are removed. How many moles are left ?

Q. One litre of 1 molar $H_{2}S{O}_4$ solution has been diluted by 5 litre water, the normality of the solution is

1. 10N
2. 0.2N
3. 0.33N
4. 5N

Q.

Molarity of 4% (w/v) solution of NaOH is

1. 0.5

2. 0.001

3. 1.0

4. 0.1

Q.

How much NaOH is required to neutralise 1500 cm³ of 0.1 N HCl?

1. 60 g

2. 4 g

3. 6 g

4. 40 g

Q.

Find molarity, molality, and normality of ${\mathrm{H}}_2{\mathrm{SO}}_4$ in $98\%$ w/w solution.$(\mathrm{\rho }=1.8{\mathrm{gml}}^{-1})$.

Q. The normality of $0.3\text{M}$ phosphorous acid is

1. $0.1\text{N}$
2. $0.9\text{N}$
3. $0.3\text{N}$
4. $0.6\text{N}$

Q.

A $5.2$ molal aqueous solution of methyl alcohol $\left({\mathrm{CH}}_3\mathrm{OH}\right)$ is supplied. What is the mole fraction of methyl alcohol in the solution?

Q.

If 3.01*10²⁰ molecules are removed from 98mg of H₂​​​​​SO₄ then no. Of moles of H₂SO_​​​4 left are?

Q.

The number of atoms present in 0.1 mole of p_{​​​​​​4 is}

Q. 1 mole is equal to how many electrons

Q.

How many water molecules are present in one mL of water (d=1g/mL)?

Q.

How many grams of dibasic acid (Mol. Wt = 200) should be present in 100mL of its aqueous solution to give decinormal strength?

1. 1g
2. 10g
3. 20g
4. 2g

Q.

Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.

Q.

Calculate the number of moles in 1 × 10²³ molecules of CO₂

Q.

Commercialy available concentrated HCl contains 38% HCl by mass ?

1) What is the molarity of the solution ? ( d = 1.19 g/mL)

2) What volume of concentrated HCl is required to make 1 L of 0.1 M of HCL ?

Q.

25 ml of 3.0 M HNO₃ are mixed with 75 ml of 4.0 M HNO₃. If the volumes are additive, the molarity of the final mixture would be:

1. 3.25 M

2. 4.0 M

3. 3.75 M

4. 3.50 M