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# Weak Titrate-Strong Titrant Curves

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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

Concept #1: Key Features of Weak Titrate-Strong Titrant Curve

Buffer Region exists between a weak titrate and strong titrant. This is a region where pH gradually changes.

Example #1: Consider the titration of 55.0 mL of 0.120 M HCN with 0.160 M LiOH. Calculate the volume needed to reach the half equivalence point.

Practice: Consider the titration of 30.0 mL of 0.100 M HC2H3O2 with 0.100 M NaNH2. Which volume of NaNH2 would take place within the buffer region?

a) 30.0 mL                    b) 50.0 mL                    c) 10.0 mL                     d) 100.0 mL                   e) 1.5 L

Concept #2: Buffer Region

In this titration curve, weak acid was titrated with a strong base, creating a buffer region.

Concept #3: Buffer Region

In this titration curve, weak base was titrated with a strong acid, creating a buffer region.

Example #2: At the half equivalence point the [WA] = [CB]. Consider the titration of 100.0 mL of 0.200 M of a weak monoprotic acid with 50.0 mL of 0.200 M NaOH. Determine Ka value of the weak acid if the pH is 4.18.

Practice: In titration of NH3 and HCl, what is the predominant species beyond the equivalence point?

a) NH3                                      b) HCl                                       c) CH3NH­2                                d) Cl