Calculate the volume of a 0.15 mol dm-3 Ba(OH)2 solution required to completely neutralize 45 cm3 of a 0.29 mol dm-3 HNO3 soluti
1 answer:
Answer:
Explanation:
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In this case, given the neutralization chemical reaction of barium sulfate and nitric acid, it is possible to evidence the 1:2 mole ratio between them; thus, at the equivalence point we have:
Which in terms of molarities and volumes is:
In such a way, by solving for the volume of base, we proceed as follows:
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<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
- If the solution has high hydrogen ion concentration, then the pH will be low.
- If the solution has low hydrogen ion concentration, then the pH will be high.
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.