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Answer :
Explanation:
Sulfuric acid ([tex]H_{2}SO_{4}[/tex]) is a diprotic acid. So, it means that we need twice as much NaOH.
As we known that an equivalence point is reached when moles of an acid equals the moles of a base.
As moles of [tex]H_{2}SO_{4}[/tex] is calculated as follows.
[tex]36.3 mL \times \frac{1 L}{1000 mL} \times 0.0529 M H_{2}SO_{4}[/tex] = 0.00192 moles of [tex]H_{2}SO_{4}[/tex]
Therefore, moles of NaOH needed will be as follows.
[tex]2 \times 0.00192 moles[/tex]
= 0.00384 mol
Hence, volume of NaOH is calculated as follows.
[tex]\frac{1000 mL}{1 L} \times \frac{0.00384 moles}{0.0411 M NaOH}[/tex]
= 93.43 mL
Thus, we can conclude that the volume of base required to reach the equivalence point is 93.43 mL.
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Answer: 934.4 ml
Explanation:
According to the neutralization law,
[tex]n_1M_1V_1=n_2M_2V_2[/tex]
where,
[tex]M_1[/tex] = molarity of [tex]H_2SO_4[/tex] solution = 0.529 M
[tex]V_1[/tex] = volume of [tex]H_2SO_4[/tex] solution = 36.3 ml
[tex]M_2[/tex] = molarity of [tex]NaOH[/tex] solution = 0.0411 M
[tex]V_2[/tex] = volume of [tex]NaOH[/tex] solution = ?
[tex]n_1[/tex] = valency of [tex]H_2SO_4[/tex] = 2
[tex]n_2[/tex] = valency of [tex]NaOH[/tex] = 1
[tex]2\times 0.529M\times 36.3=1\times 0.0411\times V_2[/tex]
[tex]V_2=934.4ml[/tex]
Therefore, the volume of the base required to reach the equivalence point is 934.4 ml
