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# Topic: Titration Do Now: - PowerPoint PPT Presentation

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.

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Do Now:

• 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

• 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

• End-point = point at which indicator changes color

• if indicator chosen correctly:

• end-point very close to equivalence point

Equivalence Pt 

0 ml

20 ml

Titration of a strong acid with a strong base

Phenolphthalein

Color change:

8.2 to 10 

pH

7-

0-

Volume of 0.100 M NaOH added (ml)

40ml

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

• 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

• # of H’s = 1

• Ma= ?

• Va = 40.0 mL

• # of OH’s = 1

• Mb = 0.100 M

• Vb = 35.0 mL

X = 0.875 M HNO3

• 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

• # of H’s = 1

• Ma= X

• Va = 20.0 mL

• # of OH’s = 1

• Mb = 0.250 M

• Vb = 50.0 mL

X = 0.625 M HCl

• 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

• # 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)