acids and bases suroviec spring 2014 chapter 15. i. definitions of acids/bases a. arrhenius acid:...
TRANSCRIPT
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Acids and BasesSuroviec
Spring 2014
Chapter 15
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I. Definitions of Acids/Bases
A. Arrhenius Acid: something that
releases H+ in water Base: something that
releases OH- in water
B. Brønsted-Lowry Acid: substance that
donates a proton Base: substance that
accepts a proton
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C. Monoprotic vs. Polyprotic
Monoprotic acid – only has 1
proton to donate base – only can
accept 1 proton
Polyprotic acid – can donate
several protons Base – can accept
several protons
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D. Conjugate Acid-Base Pairs
A pair of compounds that differ by the presence of one H+ is called a conjugate acid-base pair
Every reaction between a Brønsted acid and Brønsted base involves H+ transfer and has 2 conjugate acid-base pairs
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II. Water Ionization
A. Water equilibriumWater ionization constant
Kw = 1.00 X 10-14 at 25.0oC
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II. Water Ionization
C. pH scale• One way to describe the concentration of H+ in solution
or the acidity of the solution
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D. Determining [H3O+] and [OH-]
pH = 1.00 pH = 10.50
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IV. Equilibrium constants
A. Acid Acids and bases are either: strong electrolytes:
completely dissociates weak electrolytes:
ionizes very little in water
Ionization constants measure extent of ionization: K>1: ionize extensively,
strong acid/base K<1: does not ionize
extensively, weak acid/base
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B. Bases
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C. Compare Acid/Base strength
Look at the pKa value and compare to the acid strength
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D. Relationship between Ka, Kb and Kw
As acid strength increases Ka increasesAs base strength increases Kb increasesConsider the relation between a conjugate
acid-base pair HB (aq) ⇌ H+ (aq) + B- (aq) KI= Ka of HB
B- (aq) + H2O ⇌ HB (aq) + OH- (aq) KII = Kb of B-
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III. Acid/Base reactions
A. Strong Acid/Strong Base
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B. Strong – Weak
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V. Equilibrium Calculations
A. Determining K from pH
0.015 M HOCN has a pH of 2.67, what is the [H3O+]? What is the Ka of HOCN?
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B. Determining the Equilibrium Concentrations and pH from Ka
A. Weak acid ionization
Given a weak acid (HA) concentration of 0.040M with a Ka of 4.0 x 10-9 what are the equilibrium concentrations of HA, A-, H3O+
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C. 5% rule
Codeine (Cod) is a powerful and addictive painkiller. It is also a weak base. Write the reaction of weak base Cod with H2O If the Ka of Hcod (the weak conjugate acid) is 1.2×10-
8, what is the Kb of Cod? Find the pH of a 2.0×10-3M solution of Cod in water.
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VI. Polyprotic Acids
Acids capable of donating more than 1 proton