Multiple Choice QuestionsIf the value of an equilibrium constant ofr particular reaction is 1.6 x1012 then at equilibrium the system will contains
all reactants
mostly reactants
mostly products
mostly products
The Ksp of Ag2CrO4, AgCl, AgBr and AgI are respectively, 1.1 x 10-12, 1.8 x 10-11, 8.3 x 10-17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, NaI and Na2CrO4?
AgI
AgCl
AgBr
AgBr
For the reversible reaction,
the equilibrium shifts in the forward direction
by increasing the concentration of NH3 (g)
by decreasing the pressure
by decreasing the concentrations of N2 (g) and H2(g)
by decreasing the concentrations of N2 (g) and H2(g)
For a given exothermic reaction Kp and Kp' are the equilibrium constant at temperatures T1 and T2 respectively. Assuming that heat of reaction si constant in temperature range between T1 and T2 it is readily observed that
Kp> Kp'
Kp< Kp'
Kp = Kp'
Kp = Kp'
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product Ksp of Ba(OH)2 is
3.3 x 10-7
5.0 x 10-7
4.0 x 10-6
4.0 x 10-6
Equimolar solutions of the following substances were prepared separately, which one of these will record the highest pH value?
BaCl2
AlCl3
LiCl
LiCl
Buffer solutions have constant acidity and alkalinity because
these give unionised acid or base on reaction with added acid or alkali
acids and alkalies in these solutions are shielded from attack by other ions.
they have a large excess of H+ or OH- ions
they have a large excess of H+ or OH- ions
A.
these give unionised acid or base on reaction with added acid or alkali
If a small amount of an acid or alkali is added to a buffer solution, it converts them into unionised acid or base. Thus, remains unaffected or in other words its acidity/alkalinity remains constant. e.g.,
H3O+ + A- ⇌ H2O +HA
-OH +HA → H2O +A-
If acid is added, it reacts with A- to form undissociated HA. Similarly, if base/alkali is added, O H- combines with HA to give H2O and A- and thus, maintains the acidity/alkalinity of buffer solution.
Give that the equilibrium constant for the reaction,
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction t the same temperature?
SO3 (g) ⇌ SO2 (g) +1/2 O2 (g)
1.8 x 10-3
3.6 x 10-3
6.0 x 10-2
6.0 x 10-2
Switch
