Question

a. How many equivalents of NaOH are needed to titrate an inorganic phosphate solution (H3PO4 <-->...

a. How many equivalents of NaOH are needed to titrate an inorganic phosphate solution (H3PO4 <--> H2PO4^- <--> HPO4^2- <-->PO4^3-) from pH2.15 to pH9.60? (assume pk1=2.15; pk2 6.82; pk3=12.38)

b. If in "a" above you would have 100 mL of 50.0mM inorganic phosphate solution at pH 2.15, how many mL of 0.500M NaOH would you have to add to get to pH 9.6?

c. Suppose, by accident, you added 1.00 mL extra 0.500M NaOH than you needed in "b" above. What would be the pH of the final solution?

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