Volume of Fe(NO₃)₃ = 5.00 ml
Total voluem of the solution = 20.0 ml
Concentration of Fe(NO₃)₃ = 0.002 M
Assuming complete dissociation of Fe(NO₃)₃ concentration of Fe³⁺ = 0.200 M
Using the dilution equation, M₁V₁ = M₂V₂
where M₁ and M₂ are the initial and final concentration of Fe³⁺ respectively and V₁ and V₂ are the initial and final volume of Fe³⁺ respectively
Plugging the data we get,
M₂ = = 5 x 10⁻⁴
Therefore, the concentration of Fe³⁺ once diluted in the mixture is 5 x 10⁻⁴M
<u>Answer:</u> The correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.
<u>Explanation:</u>
Common ion effect is defined as the effect which occurs on equilibrium when a common ion (an ion which is already present in the solution) is added to a solution. This effect generally decreases the solubility of a solute.
Equilibrium reaction of HA and KA follows the equation:
According to Le-Chateliers principle, if there is any change in the variables of the reaction, the equilibrium will shift in the direction in order to minimize the effect.
In the equilibrium reactions, ion is getting increased on the product side, so the equilibrium will shift in the direction to minimize this effect, which is in the direction of HA.
Thus, the addition of KA will shift the equilibrium in the left direction.
Equilibrium constant depends on the temperature of the system. It does not have any effect on any change of pH.
pH is defined as the negative logarithm of hydrogen ions present in the solution
As, the equilibrium is shifting in the left direction, that means concentration of ions are getting decreases. This will increase the pH of the solution.
Hence, the correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.