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Chem 116 - General Chemistry II

Titrations

pH During a Titration 1

In a titration, 15 mL of 0.30 M HBr is titrated with 0.25 M KOH. What is the pH of the solution after the addition of a total of 17. mL of 0.25 M KOH?

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pH During a Titration 2

In a titration, 15 mL of 0.30 M HBr is titrated with 0.25 M KOH. What is the pH of the solution after the addition of a total of 19. mL of 0.25 M KOH?

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pH During a Titration 3

Consider the titration of 10.0 mL of 0.120 M of HA (KA = 8.0×10-3) with 0.30 M NaOH. What is the pH after the addition of a total of 1.0 mL of 0.30 M NaOH?

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Neutralization of a Diprotic Acid

Consider the titration of 20.0 mL of 0.20 M H2SO3 with 0.62 M NaOH. What volume of NaOH solution is needed to reach the second equivalence point (i.e., to completely neutralize both protons)?

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Relative pH Values at the Equivalence Point

Relative pH values (i.e., acidic, basic, or neutral) at the equivalence point in titrations of HNO3 by Ca(OH)2 and CH3NH2 by HBr are expected to be __________ and __________, respectively.

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pH at the Equivalence Point

Consider the titration of 10.0 mL of 0.120 M of HA (KA = 8.0×10-3) with 0.30 M NaOH. What is the pH at the equivalence point?

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Volume of Base Needed to Reach the Equivalene Point

Consider the titration of 20.0 mL of 0.012 M HNO3 with 0.010 M Ca(OH)2. What volume of Ca(OH)2 solution is needed to reach the equivalence point and what is the pH at the equivalence point?

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Acid/Base Titration

Consider a 40.00 mL volume of 0.10 M HCl that is titrated with 0.10 M NaOH.

 

Write the neutralization reaction and classify the resulting salt as acidic, neutral, or basic.

 

Calculate the pH of the solution after the addition of 0.00 mL of 0.10 M NaOH (start of titration).

 

Calculate the pH of the solution after the addition of 20.00 mL of 0.10 M NaOH.

 

Calculate the pH of the solution after the addition of 40.00 mL of 0.10 M NaOH.



Video Solution

Acid/Base Titration

Consider the titration of 40.00 mL of 0.10 M propanoic acid (Ka = 1.3 X 10-5) that is titrated with 0.10 M NaOH. Represent propanoic acid as HA and its conjugate base as A-.

 

Calculate the pH of the solution after the addition of 0.00 mL of 0.10 M NaOH (start of titration).

 

Calculate the pH of the solution after the addition of 20.00 mL of 0.10 M NaOH.

 

Calculate the pH of the solution after the addition of 30.00 mL of 0.10 M NaOH.

 

Calculate the pH of the solution after the addition of 40.00 mL of 0.10 M NaOH.



Video Solution

Acid/Base Titration

In titration of HCN by KOH:

What type of salt is present at the equivalence point?

 

What is the pH half-way to the equivalence point?

Video Solution

Titration of a Weak Base

Consider the titration of 40.00 mL of 0.10 M piperidine (Kb= 1.3 X 10-5) that is titrated with 0.10 M HCl. Represent piperidine as B and its conjugate acid as BH+.

Calculate the pH of the solution after the addition of 0.00 mL of 0.10 M HCl (start of titration).

 

Calculate the pH of the solution after the addition of 20.00 mL of 0.10 M HCl.

Calculate the pH of the solution after the addition of 40.00 mL of 0.10 M HCl.

Video Solution