topic: titration do now:
DESCRIPTION
Topic: Titration Do Now: . Acid-Base Titration. A procedure used in order to determine the molarity of an acid or base K nown volume of a solution with a known concentration (standard solution) and k nown volume of unknown concentration and a M A V A = M B V B acid-base indicator needed. - PowerPoint PPT PresentationTRANSCRIPT
Topic: TitrationDo 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
Volume of 0.100 M NaOH added (ml)
pH
0-
14-
7- Equivalence Pt
Phenolphthalein Color change: 8.2 to 10
0 ml
40ml
20 ml
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)