Equilibrium Tes...

The pH of a solution which is 0.1 M in HA and 0.5 M in NaA. $${K_a}$$ for HA is $$1.8 \times {10^{ - 6}}$$ 

Ionic product of $$H_2O$$ is $$10^{-14}$$. The $$H^+$$ ion concentration in $$0.1\ M$$ $$NaOH$$ solution is:

The mass of acetic acid present in 500 ml of solution in which it is 1% ionised ($$Ka$$ of $$CH_{3}COOH=1.8\times 10^{-5}$$) 

The value of observed and calculate molecular weights of silver nitrate are $$92.64$$ and $$170$$ respectively. 

$$A+B\rightleftharpoons C+D$$.If initially the concentration of A and B both equal but at equilibrium,concentration of D will be twice of that of A,then what will be the equilibrium constant of the reaction?

If 0.1 M of a weak acid is taken and its percentage of the degree of ionization is $$1.34\%$$, then its ionization constant will be:

What is $$[{ NH }_{ 4 }^{ + }]$$ in a solution containing 0.02M $${ NH }_{ 3 }$$ ($${ K }_{ b }={ 1.8\times 10 }^{ -5 }$$) and 0.01M KOH?

Four grams of $$NaOH$$ solid are dissolved in just enough water to make $$1$$ litre of solution. What is the$$[H^+]$$ of the solution?

$$K_a$$ for $$HF$$ is $$3.5\times 10^{-4}$$. Calculate $$K_b$$ for the fluoride ion.

$$C(s)+H_2O(g) \rightleftharpoons CO(g)+H_2(g)$$;   $$ \Delta H < 0$$.