Understanding Titrations: Key Concepts and Equations
Explore the concept of titrations where a solution of known concentration is gradually added to another solution until a chemical reaction is complete. Learn about strong acid-strong base titrations and how to calculate molarity based on titration results.
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Presentation Transcript
Topic 1.5 Titrations
Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical reaction between the two solutions is complete. Equivalence point the point at which the reaction is complete Indicator substance that changes color at the endpoint (hopefully close to the equivalence point) Slowly add base to unknown acid UNTIL The indicator changes color (pink) 4.7
Strong Acid-Strong Base Titrations 100% ionization! NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq) OH- (aq) + H+(aq) H2O (l) No equilibrium 16.4
Titration equation The titration equation can be used for neutralization reactions (strong acid-strong base). NaOH (aq)+ HCl (aq) H2O(l) + NaCl (aq) Bb x Ca x Va = Ba x Cb x Vb Volume of base Balanced base coefficeint Concentration of base Concentratio n of acid Balanced acid coefficeint Volume of acid
A titration of a 25.00 mL sample of a hydrochloric acid solution of unknown molarity reaches the equivalence point when 38.28 mL of 0.4370 M NaOH solution has been added. What is the molarity of the HCl solution? NaOH(aq) + HCl(aq) NaCl(aq) +H2O(l) 0.6691 M HCl
A 50.00 mL sample of a sodium hydroxide solution is titrated with a 1.605 M solution of sulfuric acid. The titration requires 24.09 mL of the acid solution to reach the equivalence point. What is the molarity of the base solution? H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l) 1.547 M NaOH
