Calculate the ph of the solution at that point

Reference no: EM13707833

Problem- For a 25.0 ml of solution containing 0.100 M H3PO4 titrated by 0.200 M NaOH (Ka1= 7.11x10^-3 Ka2=6.32x10^-8 Ka3= 4.5x10^-13 for H3PO4: (a) calculate the pH of the solution when 0ml of NaOH is added. (b) Calculate the pH of the solution after 10.0ml of NaOH are added. (c) How many milliliters of NaOH are needed to reach the first equivalence point? Calculate the pH of the solution at that point. (d) Calculate the pH of the solution after 20.0 ml of NaOH are added. (e) How many milliliters of NaOH are needed to reach the second equivalence point? Calculate the pH of the solution at that point.

Give a step by step rationalization so I can understand how to work the question myself. Thank you!

Reference no: EM13707833

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