Answer :
The volume of base required to reach the equivalence point is 81.4 ml. After adding 98.5 ml of KOH, the pH of the solution is 7, indicating a neutral solution.
To calculate the volume of base required to reach the equivalence point, we need to use the concept of stoichiometry. In this case, the balanced chemical equation is:
HNO3 + KOH → KNO3 + H2O
From the equation, we can see that one mole of HNO3 reacts with one mole of KOH. Therefore, the number of moles of HNO3 can be calculated using the formula:
moles of HNO3 = concentration of HNO3 * volume of HNO3 (in L)
Given that the concentration of HNO3 is 0.225 M and the volume is 56.3 ml, we can convert the volume to liters:
Volume of HNO3 = 56.3 ml * (1 L / 1000 ml) = 0.0563 L
Now, we can calculate the moles of HNO3:
moles of HNO3 = 0.225 M * 0.0563 L = 0.0127 moles
Since the stoichiometry is 1:1, we need the same number of moles of KOH as HNO3. So, the volume of KOH required can be calculated using the formula:
volume of KOH = moles of KOH / concentration of KOH
Given that the concentration of KOH is 0.156 M, we can calculate the volume of KOH:
volume of KOH = 0.0127 moles / 0.156 M = 0.0814 L
Finally, we convert the volume from liters to milliliters:
volume of KOH = 0.0814 L * (1000 ml / 1 L) = 81.4 ml
Therefore, the volume of base required to reach the equivalence point is 81.4 ml.
For the second part of the question, calculating the pH after adding 98.5 ml of KOH, we need to consider the reaction between HNO3 and KOH. The balanced chemical equation is the same as before:
HNO3 + KOH → KNO3 + H2O
Since we are adding an excess amount of KOH (98.5 ml), it will react completely with the remaining HNO3. Therefore, the moles of HNO3 remaining after the reaction can be calculated by subtracting the moles of KOH used from the initial moles of HNO3:
moles of HNO3 remaining = initial moles of HNO3 - moles of KOH used
Given that the initial moles of HNO3 is 0.0127 moles (as calculated earlier) and the moles of KOH used is the same as the initial moles of HNO3 (since the stoichiometry is 1:1), we can calculate the moles of HNO3 remaining:
moles of HNO3 remaining = 0.0127 moles - 0.0127 moles = 0 moles
Since there are no moles of HNO3 remaining, the solution is completely neutralized. Therefore, the pH after adding 98.5 ml of KOH is 7, indicating a neutral solution.
Therefore, the volume of base required to reach the equivalence point is 81.4 ml. After adding 98.5 ml of KOH, the pH of the solution is 7, indicating a neutral solution.
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To calculate the volume of base required to reach the equivalence point, we can use the concept of stoichiometry. The balanced chemical equation for the reaction between HNO3 and KOH is:
(HNO3 + KOH → KNO3 + H2O), From the equation, we can see that the stoichiometric ratio between HNO3 and KOH is 1:1. This means that for every 1 mole of HNO3, we need 1 mole of KOH to reach the equivalence point.Given that the concentration of HNO3 is 0.225 M, and the volume is 56.3 ml (which can be converted to liters by dividing by 1000, we can calculate the number of moles of HNO3.
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