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# Titrations: Weak Acid-Strong Base

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Sections
Intro to Buffers
Henderson-Hasselbalch Equation
Intro to Acid-Base Titration Curves
Strong Titrate-Strong Titrant Curves
Weak Titrate-Strong Titrant Curves
Acid-Base Indicators
Titrations: Weak Acid-Strong Base
Titrations: Weak Base-Strong Acid
Titrations: Strong Acid-Strong Base
Titrations: Diprotic & Polyprotic Buffers
Solubility Product Constant: Ksp
Ksp: Common Ion Effect
Precipitation: Ksp vs Q
Selective Precipitation
Complex Ions: Formation Constant

Titration where weak acid is the titrate and strong base is titrant.

Concept #1: Before the Equivalence Point

Before the Equivalence Point is where the moles of weak acid is greater than moles of strong base. Some conjugate base is formed.

Example #1: Consider the titration of 75.0 mL of 0.0300 M HC3H3O3 (Ka = 4.1 X 10-3) with 12.0 mL of 0.0450 M KOH. Calculate the pH.

Practice: In order to create a buffer 7.510 g of sodium cyanide is mixed with 100.0 mL of 0.250 M hydrocyanic acid, HCN. What is the pH of the buffer solution after the addition of 12.0 mL of 0.300 M NaH? Ka = 4.9 × 1010.

Concept #2: At the Equivalence Point

At the Equivalence Point is where the moles of weak acid is equal to moles of strong base. Only conjugate base remains.

Example #2: Consider the titration of 75.0 mL of 0.0300 M HC3H3O3 (Ka = 4.1 X 10-3) with 50.0 mL of 0.0450 M KOH. Calculate the pH.

Practice: Consider the titration of 75.0 mL of 0.60 M HNO2 with 0.100 M NaOH at the equivalence point. What would be the pH of the solution at the equivalence point? The Ka of HNO2 is 4.6 × 104.

Concept #3: After the Equivalence Point

After the Equivalence Point is where moles of weak acid is less than the moles of strong base. Excess strong base remains.

Example #3: Consider the titration of 75.0 mL of 0.0300 M HC3H3O3 (Ka = 4.1 X 10-3) with 75.0 mL of 0.0450 M KOH. Calculate the pH.

Practice: Calculate the pH of the solution resulting from the mixing of 55.0 mL of 0.100 M NaCN and 75.0 mL of 0.100 M HCN with 0.0090 moles of NaOH.