Acid-Base Titration Process
Learn about acid-base titration, a method to determine the concentration of acids and bases. Explore the procedure, equivalence point, end-point, and solve titration problems with this informative guide.
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Presentation Transcript
Topic: Titration Do Now:
Acid-Base Titration A procedure used in order to determine the molarity of an acid or base Known volume of a solution with a known concentration (standard solution) and known volume of unknown concentration and a MAVA = MBVB acid-base indicator needed
Titration Standard solution slowly added to unknown solution As solutions mix: neutralization reaction occurs Eventually: enough standard solution is added to neutralize the unknown solution Equivalence point
Equivalence point total # moles H+1 ions donated by acid equals total # moles H+1 accepted by base total moles H+1 = total moles OH-1
Titration End-point = point at which indicator changes color if indicator chosen correctly: end-point very close to equivalence point
Titration of a strong acid with a strong base 14- Phenolphthalein Color change: 8.2 to 10 pH Equivalence Pt 7- 0- Volume of 0.100 M NaOH added (ml) 20 ml 0 ml 40m l
MH+1 VH+1= MOH-1 VOH-1 MH+1= molarity of H+1 MOH-1= molarity of OH-1 VH+1= volume of H+1 VOH-1= volume of OH-1
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
Variables # of H s = 1 Ma = X Va = 20.0 mL # of OH s = 1 Mb = 0.250 M Vb = 50.0 mL
(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
Variables # of H s = 2 Ma = X Va = 20.0mL # of OH s = 1 Mb = 0.25M Vb = 50.0mL
(2)(X)(20.0ml) = (0.25M)(50.0ml)(1) X = 0.3125 M H2SO4(sulfuric acid)
