To receive the full credit, you must
[a] list the known quantities, the constants and equations used;
[b] write chemical equations where applicable;
[c] use tables to list initial, change and final quantities/concentrations of the reactants and products where applicable;
[d] show your calculations Neatly in Details and in a Logical order.
[e] carry an additional significant figure of values for your intermediate steps;
[f] include correct units and significant figures in the intermediate steps and final results.

1. A sample of 25.00 mL of 0.100 M HNO2 (in a flask) is tirated with 0.150 M of NaOH solution (in a buret) at 25ºC. (Hint: Find the constants in your textbook)

(1) Calculate the volume (Ve) of the NaOH solution needed to completely neutralize the acid in the flask. (0.5 pt)

(2) Calculate the pH for (a) the initial acid solution in the flask, (b) the point at which 8.00 mL of the base has been added, (c) the equivalence point, and (d) the point at which 20.00 mL of the base has been added. Box the pH values calculated (Hint: An approximation may not be applicable to all of your calculations). (10 pts)

(3) Based on the pH values you have calculated, sketch the titration curve of this acid-base reaction using either the Excel Program or a graphing paper.