Equilibrium Tes...

Which of the following mixture is not a buffer solution?

1M NaCl and 1M HCl are present in an aqueous solution . The solution is:

The $$pH$$ of a solution obtained by mixing $$50\: ml$$ of $$0.4N$$ $$NH_{4}Cl$$ and $$50\: ml$$ of $$0.2 N$$ $$NaOH$$ is:

Assertion: A buffer solution has a capacity to resist the change in pH value on an addition of a small amount of acid or base to it.
Reason: An aqueous solution of ammonium acetate can act as buffer.

$$C_{2}H_{4}(g) + H_{2}(g)\leftrightharpoons  C_{2}H_{6}(g);\ \Delta H = - 31.7 \ kcal$$.
The equilibrium concentration of $$C_{2}H_{4}$$ in the following reaction can be increased by:

The equilibrium constant of a reaction at $$298 \:K$$ and $$1000\: K$$ is $$5 \times 10^{-3}$$ and $$2\times 10^{-3}$$ respectively. The $$\Delta  H$$ for the reaction is:

The reaction $$A + B \leftrightharpoons C + D + heat$$, has reached equilibrium. It is possible to make the reaction to proceed forward:

Assertion: pH of blood does not change in spite of taking acidic foods.
Reason: Blood behaves as a buffer solution.

In the system $$CaF_{2} (s) \rightleftharpoons Ca^{2+}(aq) + 2F^{-}(aq)$$, if the concentration of $$Ca^{2+}$$ is increased by four times, then the equilibrium concentration of $$F^{-}$$ will be changed to: