1.

KF combines with HF to form KHF₂. This compound contains the species

• K⁺, F^- and H⁺

• K⁺, F^- and HF

• K⁺ and [HF₂]^-

• [KHF]⁺ and F₂

pH of a 0.01 M solution (K_a = 6.6 $\times$ 10^-4)

• 7.6

• 8

• 2.6

• 5

A vessel of one litre capacity containing 1 mole of SO₃ is heated till a state of equilibrium is attained.

2SO_{3 (g)} $\rightleftharpoons$ 2SO_{2 (g)} + O_{2 (g)}

At equilibrium, 0.6 moles of SO₂ had formed. The value of equilibrium constant is

• 0.18

• 0.36

• 0.45

• 0.68

Mercurous chloride exists in the form of

• Hg⁺

• Hg₂²⁺

• Hg²⁺

• Hg₃²⁺

What is the molarity of H₂SO₄ solution that has a density of 1.84 g/cc at 35$°$C and contains 98% by weight?

• 4.18 M

• 8.14 M

• 18.4 M

• 18 M

The variation of volume V, with temperature T, keeping pressure constant is called the coefficient of thermal expansion ($\mathrm{\alpha }$) of a gas, i.e., $\mathrm{\alpha }$ = $\frac{1}{\mathrm{V}}{\left(\frac{\mathrm{dV}}{\mathrm{dT}}\right)}_{\mathrm{P}}$. For an ideal gas $\mathrm{\alpha }$ is equal to

• T

• $\frac{1}{\mathrm{T}}$

• P

• $\frac{1}{\mathrm{P}}$

The molecules having the same hybridization, shape and number of lone pairs of electrons are

• SeF₄, XeO₂F₂

• SF₄, XeF₂

• XeOF₄, TeF₄

• SeCl₄, XeF₄

2.5 g of the carbonate of a metal was treated with 100 mL of 1N H₂SO₄. After the completion of the reaction, the solution was boiled off to expel CO₂ and was then titrated against 1N NaOH solution. The volume of alkali that would be consumed, if the equivalent weight of the metal is 20

• 50

• 25

• 75

• 100

The equilibrium constant for mutarotation $\mathrm{\alpha }$-D Glucose $\rightleftharpoons$ $\mathrm{\beta }$-D Glucose is 1.8. What percentage of $\mathrm{\alpha }$ form remains at equilibrium?

• 35.7

• 64.3

• 55.6

• 44.4

The M - O- M bond angles in MO (where M is halogen) is in the order

• Br₂O > Cl₂O > F₂O

• F₂O > Br₂O > Cl₂O

• F₂O > Cl₂O > Br₂O

• Cl₂O > F₂O > Br₂O