1 properties of acids have a sour taste. vinegar owes its taste to acetic acid. citrus fruits...
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Properties of Acids
Have a sour taste. Vinegar owes its taste to acetic acid. Citrusfruits contain citric acid.
React with certain metals to produce hydrogen gas.
React with carbonates and bicarbonatesto produce carbon dioxide gas
Cause color changes in plant dyes.
2HCl (aq) + Mg (s) MgCl2 (aq) + H2 (g)
2HCl (aq) + CaCO3 (s) CaCl2 (aq) + CO2 (g) + H2O (l)
Aqueous acid solutions conduct electricity.
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Have a bitter taste.
Feel slippery. Many soaps contain bases.
Properties of Bases
Cause color changes in plant dyes.
Aqueous base solutions conduct electricity.
Examples:
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Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water
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Hydronium ion, hydrated proton, H3O+
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A Brønsted acid is a proton donorA Brønsted base is a proton acceptor
acidbase acid base
A Brønsted acid must contain at least one ionizable proton!
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Monoprotic acidsHCl H+ + Cl-
HNO3 H+ + NO3-
CH3COOH H+ + CH3COO-
Strong electrolyte, strong acid
Strong electrolyte, strong acid
Weak electrolyte, weak acid
Diprotic acidsH2SO4 H+ + HSO4
-
HSO4- H+ + SO4
2-
Strong electrolyte, strong acid
Weak electrolyte, weak acid
Triprotic acidsH3PO4 H+ + H2PO4
-
H2PO4- H+ + HPO4
2-
HPO42- H+ + PO4
3-
Weak electrolyte, weak acid
Weak electrolyte, weak acid
Weak electrolyte, weak acid
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Identify each of the following species as a Brønsted acid, base, or both. (a) HI, (b) CH3COO-, (c) H2PO4
-
HI (aq) H+ (aq) + I- (aq) Brønsted acid
CH3COO- (aq) + H+ (aq) CH3COOH (aq) Brønsted base
H2PO4- (aq) H+ (aq) + HPO4
2- (aq)
H2PO4- (aq) + H+ (aq) H3PO4 (aq)
Brønsted acid
Brønsted base
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Neutralization Reaction
acid + base salt + water
HCl (aq) + NaOH (aq) NaCl (aq) + H2O
H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O
H+ + OH- H2O
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Neutralization Reaction Involving a Weak Electrolyte
weak acid + base salt + water
HCN (aq) + NaOH (aq) NaCN (aq) + H2O
HCN + Na+ + OH- Na+ + CN- + H2O
HCN + OH- CN- + H2O
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Neutralization Reaction Producing a Gas
acid + base salt + water + CO2
2HCl (aq) + Na2CO3 (aq) 2NaCl (aq) + H2O +CO2
2H+ + 2Cl- + 2Na+ + CO32- 2Na+ + 2Cl- + H2O + CO2
2H+ + CO32- H2O + CO2
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Sr2+(aq) + 2OH-(aq)+ 2H+(aq)+ 2ClO4-(aq)
2H2O(l)+Sr2+(aq)+2ClO4-(aq)
Sr2+(aq) + 2OH-(aq)+ 2H+(aq)+ 2ClO4-(aq)
2H2O(l)+Sr2+(aq)+2ClO4-(aq)
Ba2+(aq) + 2OH-(aq)+ 2H+(aq)+ SO42-(aq)
2H2O(l)+Ba2+(aq)+SO42-(aq)
Sample Problem 4.4 Writing Ionic Equations for Acid-Base Reactions
PROBLEM: Write balanced molecular, total ionic, and net ionic equations for each of the following acid-base reactions and identify the spectator ions.
reactants are strong acids and bases and therefore completely ionized in water
PLAN: SOLUTION:
(a) Sr(OH)2(aq)+2HClO4(aq) 2H2O(l)+Sr(ClO4)2(aq)
2OH-(aq)+ 2H+(aq) 2H2O(l)
(a) strontium hydroxide(aq) + perchloric acid(aq)
(b) barium hydroxide(aq) + sulfuric acid(aq)
(b) Ba(OH)2(aq) + H2SO4(aq) 2H2O(l) + BaSO4(aq)
2OH-(aq)+ 2H+(aq) 2H2O(l)
products are
water
spectator ions
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Figure 4.7 An acid-base titration.
Start of titrationExcess of acid
Point of neutralization
Slight excess of base
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Sample Problem 4.5 Finding the Concentration of Acid from an Acid-Base Titration
PROBLEM: You perform an acid-base titration to standardize an HCl solution by placing 50.00 mL of HCl in a flask with a few drops of indicator solution. You put 0.1524 M NaOH into the buret, and the initial reading is 0.55 mL. At the end point, the buret reading is 33.87 mL. What is the concentration of the HCl solution?
PLAN:SOLUTION:
volume(L) of base
mol of base
mol of acid
M of acid
multiply by M of base
molar ratio
divide by L of acid
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)
(33.87-0.55) mL x 1L
103 mL= 0.03332 L
0.03332 L X 0.1524 M = 5.078x10-3 molNaOH
Molar ratio is 1:1
5.078x10-3 mol HCl
0.05000 L= 0.1016 M HCl
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Figure 4.8
An aqueous strong acid-strong base reaction on the atomic scale.