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75.00 mL of a H3PO4(aq) solution was titrated with a 0.2556 M Mg(OH)2 (aq) and the end point of this titration was 63.65 mL.  Please answer the following questions.

1. What is the name of H3PO4(aq)?

2. What is the name of Mg(OH)2?

3. What is the pH at the endpoint of this titration?

4. Write out the balance equation for this titrations include the phases.

5. What is the molarity of the hydronium ion at the endpoint?

6. What is the molarity of the hydroxide ion at the endpoint?

7. What is the molarity of the H3PO4(aq) solution when no Mg(OH)2(aq) has been added?

8. What is the pH of the H3PO4(aq)solution when no Mg(OH)2(aq) has been added?

9. When 50.00 mL of Mg(OH)2 solution is added to the H3PO4(aq) solution, what is the pH of the combined solutions.

10. When 70.00 mL of Mg(OH)2(aq) solution is added to the H3PO4(aq) solution, what is the pH of the combined solutions.

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