25.00 mL of a solution of phosphoric acid, H3PO4, was titrated with 0.500 M NaOH. a) Write the balanced chemical equation for this reaction. b) If 35.92 mL of NaOH solution were needed to reach the end point in the titration, what is the molarity of the H3PO4 solution? c) How many grams of H3PO4 were present?
25.00 mL of a solution of phosphoric acid, H3PO4, was titrated with 0.500 M NaOH. a) Write the balanced chemical equation for this reaction. b) If 35.92 mL of NaOH solution were needed to reach the end point in the titration, what is the molarity of the H3PO4 solution? c) How many grams of H3PO4 were present?
General Chemistry - Standalone book (MindTap Course List)
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Chapter4: Chemical Reactions
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CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.)
25.00 mL of a solution of phosphoric acid, H3PO4, was titrated with 0.500 M NaOH.
a) Write the balanced chemical equation for this reaction.
b) If 35.92 mL of NaOH solution were needed to reach the end point in the titration, what is the molarity of the H3PO4 solution?
c) How many grams of H3PO4 were present?
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