Equilibrium Tes...

When strong base $$(NaOH)$$ is added to the weak acid (acetic acid, $${ CH }_{ 3 }COOH$$), then dissociation of acetic acid increases; this effect is known as:

For the equilibrium, $$ H_2 + I_2 \leftrightharpoons 2HI , $$ which of the following will effect the equilibrium constant?

Which of the following acid / base pairs act as natural buffers in living systems?

$${ H }_{ 2 }(g)+{ I }_{ 2 }(g)\rightleftharpoons 2HI(g)$$ 

The degree of dissociation of water at $${ 25 }^{ o }C$$ is $$1.8\times { 10 }^{ -7 }$$% and density is $$1.0g{ cm }^{ -3 }$$. The ionic constant for water is:

Which of the following is not a buffer solution ?

What do you mean by buffer solution?

The pH of a $$0.1M$$ aqueous solution of a weak acid ($$HA$$) is $$3$$. Its degree of dissociation is

To prepare a buffer solution of $$pH = 4.04$$, amount of Barium acetate to be added to $$100 mL$$ of $$0.1$$ M acetic acid solution [ $$pK_0(CH_3COO^-) =9.26$$] is:

If some $$He$$ gas is introduced into the equilibrium $${ PCl }_{ 5(g) }\rightleftharpoons { PCl }_{ 5(g) }+{ Cl }_{ 2(g) }$$ at constant pressure and temperature then equilibrium constant of reaction: