1. Applying Neutralization Titrations

9. Preparing standard acid solution Solution of HCl, HClO 4, and H 2 SO 4 are stable indefinitely, Restandardization is never required. Standard acid solutions are ordinarily prepared by diluting an approximate volume of the concentrated and subsequently standardizing the diluted solution against a primary-standard base.

10. Standardizing Acids using Sodium Carbonate Dealing the reagent The reaction equation Which equivalence point used as end point Why are the solution heated near the end point What indicators are selected How to calculate the results

11. Preparing standard base solution The effect of carbon dioxide: carbonate error, indicator The amount of hydronium ion consumed is identical to the amount of hydroxide lost during formation of carbonate ion, no error is incurred. Carbonate ion decrease the sharpness of end points. Boiled to eliminate the gas, Deionized water, Sparging the solution. Stored in polyethylene bottles rather than glass.

12. Standardizing solutions of base Standard solution of strong bases cannot be prepared directly by mass and must always be saandardized against a primary standard with acidic properties Potassium hydrogen phthalate

18. Table 14-2 Volume of relationships in the analysis of mixtures containing hydroxide, carbonate, and hydrogen carbonate ions

21. The hydrogen carbonate equivalence point is not sufficient to give a sharp color change with a chemical indicator, what is the method to improve the accuracy? 1. Carbonate/hydroxide mixtures 2.Carbonate/ hydrogen carbonate

22. How could you analyze a mixture of HCl and H 3 PO 4 ? A mixture of Na 3 PO 4 and Na 2 HPO 4 ? How could you determine the saponification number or ester value? Could you design the experiments of analyzing N, S, C, Cl, F, P etc based on neutralization titrations? Group Discussion