Understanding Neutralization Reactions
Learn about neutralization reactions, acid-base titrations, pH changes, titration endpoints, and solve titration problems with detailed solutions. Explore the concept of neutralization through practical examples and understand the chemistry behind it.
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Presentation Transcript
Topic: Neutralization Reaction Do Now:
Neutralization Reactions + Base Salt + Water Acid HX(aq) + MOH(aq) MX(aq) +H2O(l) DR rxn
Acid-Base Titration A procedure used in order to determine the unknown molarity of an acid or base MAVA = MBVB (molarity of acid)(volume of acid) = (molarity of base)(volume of base) You will know 3 out of the 4 variable Standard solution slowly added to unknown solution As solutions mix: neutralization reaction occurs Eventually: enough standard solution is added to neutralize the unknown solution
pH changes during neutralization pH < 7 Start with an acid Add a base At neutralization pH pH = 7 When pH = 7 called equivalence point [H+] = [OH-] pH > 7 Start with a base Add an acid At neutralization pH pH = 7 acid-base indicator needed WHY? Usually use phenolphalein WHY?
Titration End-point = point at which indicator changes color if indicator chosen correctly: end-point very close to equivalence point
MH+1 VH+1= MOH-1 VOH-1 If you titrate H2SO4 and NaOH 2H+ 1OH+-
Titration Problem #1 In a titration of 40.0 mL of a nitric acid solution, the end point is reached when 35.0mL of 0.100M NaOH is added Calculate the concentration of the nitric acid solution HNO3 + NaOH H2O + NaNO3
Variables # of H s = 1 Ma = ? Va = 40.0 mL # of OH s = 1 Mb = 0.100 M Vb = 35.0 mL
(1)(X) (40.0 mL) = (0.100 M )(35.0mL)(1) X = 0.875 M HNO3
Titration Problem #2 What is the concentration of a hydrochloric acid solution if 50.0 mL of a 0.250M KOH solution is needed to neutralize 20.0mL of the HCl solution of unknown concentration? KOH + HCl H2O + KCl
(1)(X)(20.0 mL) = (0.250 M) (50.0 mL)(1) X = 0.625 M HCl
Titration Problem #3 What is the concentration of a sulfuric acid solution if 50.0mL of a 0.25 M KOH solution is needed to neutralize 20.0mL of the H2SO4 solution of unknown concentration? H2SO4 + 2 KOH 2 H2O + K2SO4
(2)(X)(20.0ml) = (0.25M)(50.0ml)(1) X = 0.3125 M H2SO4(sulfuric acid)
