A solution of 0.300 M NaOH is used to neutralize 25.00 mL H3PO4 solution.
If 37.5 mL NaOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution?
I did the first step by writing the balanced chm eq
Balanced chemical equation:
3NaOH + H3PO4 = 3H20 + Na3PO4
which are the acids, which are the bases? How can I determine if this is a 1:1 mol:mol ratio?
Also, what are the steps to complete this problem?
If 37.5 mL NaOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution?
I did the first step by writing the balanced chm eq
Balanced chemical equation:
3NaOH + H3PO4 = 3H20 + Na3PO4
which are the acids, which are the bases? How can I determine if this is a 1:1 mol:mol ratio?
Also, what are the steps to complete this problem?
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Answer: 0.15
H3PO4 is an acid because it has hydrogen ions at the front of the compound. NaOH is the base because there is no hydrogen ions at the front of the compound.
H3PO4 is an acid because it has hydrogen ions at the front of the compound. NaOH is the base because there is no hydrogen ions at the front of the compound.