'Buffered solution' diaporamas de présentation

Acid-Base Equilibria

Acid-Base Equilibria. AP Chem Unit 15. Unit 15 Content . Solutions of Acids or Bases Containing a Common Ion Buffered Solutions Buffering Capacity Titrations and pH Curves Acid-Base Indicators. Introduction.

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Chapter 15 Applications of Aqueous Equilibria

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Chapter 15 Applications of Aqueous Equilibria

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Fractions of H 2 CO 3 , HCO 3 - , and CO 3 2- as a Function of pH

Fractions of H 2 CO 3 , HCO 3 - , and CO 3 2- as a Function of pH. Fractions of H 3 PO 4 , H 2 PO 4 2- , and PO 4 3- as a Function of pH. Solving a Buffering Problem. Hydroxide Ions Added to a Solution. Resulting Buffered Solution. Buffered Solution. Buffered Solution.

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Chapter 15

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Applications of Aqueous Equilibria

Applications of Aqueous Equilibria. Strong Acid/Strong Base Titration. Endpoint is at pH 7. A solution that is 0.10 M HCl is titrated with 0.10 M NaOH. Strong Acid/Strong Base Titration. A solution that is 0.10 M NaOH is titrated with 0.10 M HCl. Endpoint is at pH 7.

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Additional Aspects of Aqueous Equilibria

Additional Aspects of Aqueous Equilibria. Reaction of Weak Bases with Water. The base reacts with water, producing its conjugate acid and hydroxide ion:. CH 3 NH 2 + H 2 O ? CH 3 NH 3 + + OH - K b = 4.38 x 10 -4. K b for Some Common Weak Bases.

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Additional Aspects of Aqueous Equilibria

Additional Aspects of Aqueous Equilibria. Reaction of Weak Bases with Water. The base reacts with water, producing its conjugate acid and hydroxide ion:. CH 3 NH 2 + H 2 O ? CH 3 NH 3 + + OH - K b = 4.38 x 10 -4. K b for Some Common Weak Bases.

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Chapter 15 Applications of Aqueous Equilibria

Chapter 15 Applications of Aqueous Equilibria. REACTIONS AND EQUILIBRIA INVOLVING ACIDS, BASES, AND SALTS. Common Ions. Common ion effect - The addition of an ion already present (common) in a system causes equilibrium to shift away from the common ion. Example 1.

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ELECTROCHEMICAL DETECTION OF BIOFILMS

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Buffers and Acid/Base Titration

Buffers and Acid/Base Titration. Reaction of Weak Bases with Water. The base reacts with water, producing its conjugate acid and hydroxide ion:. CH 3 NH 2 + H 2 O ? CH 3 NH 3 + + OH - K b = 4.38 x 10 -4. K b for Some Common Weak Bases.

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Buffers

Buffers. Buffered Solutions. A buffered solution is one that resists a change in its pH when either hydroxide ions or protons (H 3 O + ) are added. Very little change in pH is witnessed even when a strong acid or base is added. The components of a buffer are a conjugate acid-base pair.

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Buffered Solutions

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