A solution of Na₂S₂O₃ is standardized iodometrically against 0.167 g of KBrO₃. This process requires 50 mL of the ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ solution. What is the normality of the  Na₂S₂O₃?

1. 0.2 N

2. 0.12 N

3. 0.72 N

4. 0.02 N

The ${\mathrm{NH}}_3$ evolved due to complete conversion of N from 1.12 g sample of protein was absorbed in 45 mL of 0.4 N ${\mathrm{HNO}}_3$. The excess acid required 20 mL of 0.1 N $\mathrm{NaOH}$. The % N in the sample is:

1.  8

2.  16

3.  20

4.  25

When a mixture containing HCl and H₂SO₄ weighing 0.1 g undergoes treatment with an excess of AgNO₃ solution, resulting in the formation of 0.1435 g of AgCl, what is the weight percentage of H₂SO₄ in the mixture?

1.  36.5

2.  63.5

3.  50

4.  None of the above

What volume of ${\mathrm{O}}_2\left(\mathrm{g}\right)$ measured at 1 atm and 273 K will be formed by the action of 100 mL of 0.5 N KMnO₄ on hydrogen peroxide in an acid solution?

The skeleton equation for the reaction is

${\mathrm{KMnO}}_4+{\mathrm{H}}_2{\mathrm{SO}}_4+{\mathrm{H}}_2{\mathrm{O}}_2$$\to {\mathrm{K}}_2{\mathrm{SO}}_4+{\mathrm{MnSO}}_4+{\mathrm{O}}_2+{\mathrm{H}}_2\mathrm{O}$

1.  0.12 litre

2.  0.028 litre

3.  0.56 litre

4.  1.12 litre

The equivalent weight of $\mathrm{HCl}$ in the given reaction is: ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7+14\mathrm{HCl} \to 2\mathrm{KCl}+2{\mathrm{CrCl}}_3+3{\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{O}$

1.  16.25

2.  36.5

3.  73

4.  85.1

Equivalent weight of ${\mathrm{FeS}}_2$ in the half reaction, ${\mathrm{FeS}}_2 \stackrel{}{\to } {\mathrm{Fe}}_2{\mathrm{O}}_3+{\mathrm{SO}}_2$ is:

1.  M/10

2.  M/11

3.  M/6

4.  M/1

The molar mass of diacidic organic Lewis base (B), if 12 g of chloroplatinate salt $\left({\mathrm{BH}}_2{\mathrm{PtCl}}_6\right)$ on ignition produced 5 gm residue of Pt,will be -

1.  52

2.  58

3.  88

4.  None of these

What volume of HCl solution of density 1.2 g/cm³ and containing 36.5% by weight HCl, must be allowed to react with zinc(Zn) in order to liberate 4.0 g of hydrogen?

1.  333.33 mL

2.  500 mL

3.  614.66 mL

4.  None of these

100 mL of ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution having molarity of 1M and density 1.5 g/mL is mixed with 400 mL of water. The molarity of the ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution will be: (final density is 1.25 g/mL )

Phosphoric acid $\left({\mathrm{H}}_3{\mathrm{PO}}_4\right)$ prepared in a two step process.

(1) ${\mathrm{P}}_4+5{\mathrm{O}}_2 \stackrel{}{\to } {\mathrm{P}}_4{\mathrm{O}}_{10}$
(2) ${\mathrm{P}}_4{\mathrm{O}}_{10}+6{\mathrm{H}}_2\mathrm{O} \stackrel{}{\to } 4{\mathrm{H}}_3{\mathrm{PO}}_4$

We allow 62g of phosphorus to react with react with excess oxygen which form ${\mathrm{P}}_4{\mathrm{O}}_{10}$ in 85% yield. In the step (2) reaction 90% yield of ${\mathrm{H}}_3{\mathrm{PO}}_4$ is obtained. Produced mass of ${\mathrm{H}}_3{\mathrm{PO}}_4$ is:

1.  37.485 g

2.  149.949 g

3.  125.47 g

4.  564.48 g