CHM 104 1st Edition Lecture 20 Outline of Last Lecture I pH of Buffer Outline of Current Lecture II III Acid Base Titrations pH of titrated solutions Current Lecture pH titration A systematic neutralization experiment where a strong base or strong acid solution of known concentration the titrant is incrementally added to a solution containing an acid or base species while the pH of the resulting mixture is measured Example of titration graphs Information that can be obtained from this graph The moles of acid that were present in the solution Equivalence point volume Point in the titration where all of the HA has been neutralized by the NaOH sharp change in pH once all HA reacted At this volume the moles of titrant that has been added is exactly equal to the moles of the species being titrated Strength of the acid in the solution Is it a strong or weak acid What is it s Ka This can be determined by monitored the pH in the region BEFORE the equivalence volume Examples of titrations SA titrated by SB These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute WA SB Mixture of acids SB Diprotic WA SB WB SA Lab Strong Acid titrated by a Strong Base 100 0 mL of 0 20 M HCl titrated by 0 10 M NaOH Titrant NaOH this would be placed in buret What is the neutralization reaction that occurs HCl NaCl NaCl H2O H3O OH H2O H2O How many mL of NaOH need to be added to completely neutralize the HCl Mol NaOH 0 1000 L 0 20 M 0 020 mol Vol NaOH E P 0 020 mol 0 10 M 0 20 L pH of solution after large incremental addition of titrant volume After 0 0 mL of NaOH have been added to the HCl 0 20 M HCl SA so H3O 0 20 M pH 0 70 After 50 0 mL of NaOH have been added to the HCl After 150 0 mL of NaOH have been added to the HCl After 200 0 mL of NaOH have been added to the HCl After 250 0 mL of NaOH have been added to the HCl
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