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Weak Bases: Properties, Equilibria, and Calculations, Exercises of Chemistry

An overview of weak bases, their reaction with water, and the production of hydroxide ions. It includes examples of common weak bases, the role of lone pairs on n, the kb expression, and the difference between acids and bases. The document also covers polyprotic bases, amphiprotic molecules, and the relationship between acid strength and base strength. Numerous examples are given for calculating ph and the concentration of ions in solution.

What you will learn

  • How do you calculate the pH of a solution containing a weak base and a weak acid?
  • What is the difference between a weak base and a strong base?
  • How does the strength of an acid relate to the strength of its conjugate base?

Typology: Exercises

2021/2022

Uploaded on 09/12/2022

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Weak Bases
Weak bases (bases without OH) react with water to produce a hydroxide ion. Common examples
of weak bases are ammonia (NH3), methylamine (CH3NH2), and ethylamine (C2H5NH2). The lone
pair on N forms a bond with a H+. Most weak bases involve N.
The equilibrium expression for bases is known as the Kb.
for weak base reactions: B + H2O HB+ + OH
Notice that Ka and Kb expressions look very similar. The difference is that a base produces the
hydroxide ion in solution, while the acid produces the hydronium ion in solution.
Another note on this point: H+ and H3O+ are both equivalent terms here.
Often water is left completely out of the equation since it does not appear in the equilibrium. This
has become an accepted practice. (* However, water is very important in causing the acid to
dissociate.)
polyprotic bases--accept more than one H+; anions with 2 and 3 charges (ex. PO43 ; HPO42)
Amphiprotic or amphoteric --molecules or ions that can behave as EITHER acids or bases; water,
anions of weak acids (look at the examples abovesometimes water was an acid, sometimes it acted
as a base)
pf3

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Weak Bases Weak bases (bases without OH−) react with water to produce a hydroxide ion. Common examples of weak bases are ammonia (NH 3 ), methylamine (CH 3 NH 2 ), and ethylamine (C 2 H 5 NH 2 ). The lone pair on N forms a bond with a H+. Most weak bases involve N. The equilibrium expression for bases is known as the K b. for weak base reactions: B + H 2 O HB+^ + OH−  Notice that K a and K b expressions look very similar. The difference is that a base produces the hydroxide ion in solution, while the acid produces the hydronium ion in solution.  Another note on this point: H+^ and H 3 O+^ are both equivalent terms here. Often water is left completely out of the equation since it does not appear in the equilibrium. This has become an accepted practice. (* However, water is very important in causing the acid to dissociate.)  polyprotic bases --accept more than one H+; anions with −2 and −3 charges (ex. PO 43 −^ ; HPO 42 −)  Amphiprotic or amphoteric --molecules or ions that can behave as EITHER acids or bases; water, anions of weak acids (look at the examples above—sometimes water was an acid, sometimes it acted as a base)

THE STRONGER THE ACID THE WEAKER ITS CB, the converse is also true. Example 1. Using table 14.2, arrange the following species according to their strength as bases: H 2 O, F−, Cl−, NO 2 −, and CN−. Example 2 .The hypochlorite ion (OCl−) is a strong oxidizing agent often found in household bleaches and disinfectants. It is also the active ingredient that forms when swimming pool water is treated with chlorine. In addition to its oxidizing abilities, the hypochlorite ion has a relatively high affinity for protons (it is a much stronger base than Cl-, for example) and forms the weakly acidic hypochlorous acid (HOCl, K a = 3.5 × 10¯^8 ). Calculate the pH of a 0.100 M aqueous solution of hypochlorous acid.