50 cm³ of 0.2 N HCl is titrated against 0.1 N NaOH solution. The titration was discontinued after adding 50 cm³ of NaOH. The remaining titration is completed by adding 0.5 N KOH. The volume of KOH required for completing the titration is 

• 12 cm³

• 10 cm³

• 21.0 cm³

• 16.2 cm³

182.

The rms velocity of hydrogen is $\sqrt{7}$ times the rms velocity of nitrogen. If T is the temperature of the gas, which of the following is true?

• ${\mathrm{T}}_{{\mathrm{H}}_2} = \sqrt{7 } {\mathrm{T}}_{{\mathrm{N}}_2}$

• ${\mathrm{T}}_{{\mathrm{N}}_2} = {\mathrm{T}}_{{\mathrm{H}}_2}$

• ${\mathrm{T}}_{{\mathrm{N}}_2} = \sqrt{7} {\mathrm{T}}_{{\mathrm{H}}_2}$

• ${\mathrm{T}}_{{\mathrm{N}}_2} = 2{\mathrm{T}}_{{\mathrm{H}}_2}$

50 cm³ of 0.2 NHCl is titrated against 0.1 N NaOH solution. The titration is discontinued after adding 50 cm³ of NaOH.The remaining titration is completed by adding 0.5 N KOH. The volume of KOH required for completing the titration is

• 12 cm³

• 10 cm³

• 25 cm³

• 10.5 cm³

1 g of silver gets distributed between 10 cm³ of molten zinc and 100 cm³ of molten lead at 800°C. The percentage of silver in the zinc layer is approximately

• 89

• 91

• 97

• 94

Excess of silver nitrate solution is added to 100 mL of 0.01 M pentaaqua chloro chromium (III) chloride solution. The mass of silver chloride obtained in grams is [Atomic mass of silver is 108].

• 287 × 10^-3

• 143.5 × 10^-3

• 143.5 × 10^-2

• 287 × 10^-2

The empirical formula of a non-electrolyte is CH₂O. A solution containing 3 g of the compound exerts the same osmotic pressure as that of 0.05 M glucose solution. The
molecular formula of the compound is 

• CH₂O

• C₂H₄O₂

• C₄H₈O₄

• C₃H₆O₃

The empirical formula of a non-electrolyte is CH₂O. A solution containing 6g of the compound exerts the same osmotic pressure as that of 0.05 M glucose solution at the same temperature. The molecular formula of

• C₂H₄O₂

• C₃H₆O₃

• C₅H₁₀O₅

• C₄H₈O₄

The total number of electrons in 18 mL of water (density = 1 g mL^-1) is

• 6.02 × 10²⁵

• 6.02 × 10²⁴

• 6.02 ×  18 × 10²³

• 6.02 × 10²³

The number of water molecules present in a drop of water weighing 0.018 g is

• 6.022 × 10²⁶

• 6.022 × 10²³

• 6.022 × 10¹⁹

• 6.022 × 10²⁰

Empirical formula of a compound is CH₂O and its molecular mass is 90, the molecular formula of the compound is

• C₃H₆O₃

• C₂H₄O₂

• C₆H₁₂O₆

• CH₂O