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Chapter 15 Acids bases
acids• Sour• Turns litmus red• Reacts with some metals to
• Ka is large-lots of ions• Weak acid• partially dissociates• Ka is small, not many
ions• Ka =ionization constant
Strong Acids [H3O+]
• HCl• HNO3
• H2SO4
• HBr• HI
• What is the hydronium ion [H3O+] concentration in a .10 M HCl solution?
• HCl(g) + H2O(l) -----> H3O+(aq) + Cl-(aq)
Weak Acids [H3O+]
• What is the hydronium ion concentration in a .10 M HF solution? (Ka =6.8 x 10-4)
• HF(g) + H2O(l) <-----> H3O+(aq) + F -(aq)
Find Ka for weak acid• A .10 M weak acid has a hydronium ion concentration of 3.0 x 10 -4 M? What is the Ka? (ionization constant)
Arrhenius Base• produces hydroxide (OH-) ion in water• NaOH(s) -----> Na+(aq) + OH-(aq)
• Strong base-completely dissociates Kb is large-favors products• Weak base-partially dissociates Kb is small-favors reactants
Strong Bases
• NaOH• LiOH• KOH• RbOH• CsOH• Ca(OH)2
• Sr(OH)2
• Ba(OH)2
• What is the hydroxide ion concentration in a .10 M NaOH solution?
Weak Base
• NH3 is a weak base
• NH3(g) + H2O(l) <-----> NH4+(aq) + OH-(aq)
• What is the hydroxide ion concentration in a 0.10 M NH3 solution? (Kb for NH3 is 1.8 x 10 -5)
Neutralization• HCl(aq) + NaOH(aq) -------> H2O(l) + NaCl (aq)• Acid + Base water + a salt• H+ (aq) + OH- (aq)-------> H2O (l) • H3O+ (aq) + OH- (aq)------->2 H2O (l) • Titration process of adding an acid to a base or base to an acid• Equivalence point -moles of H3O+ (H+) = moles of OH-
• Indicator changes color at a certain [H3O+]• End point when color changes• When titrating to neutrality End point and equivalence point
should be very close (Choose an indicator that changes color when moles of H+ = moles of OH-)
• When neutralizing a strong acid with strong base the indicator phenolphthalein is usually used
Titration molarity of an acid or base
orvolume of an acid or base
• What volume of .10 M HCl is needed to neutralize 10. mL of .20 M NaOH?
• One to one ratio use MaVa=MbVb• Not one to one ratio use stoichiometry
• What volume of .10 M HCl is needed to neutralize 10. mL of .30 M Ca(OH)2?
• What is the molarity of an HCl solution if it takes 5.0 mL of .20 M NaOH solution to neutralize 8.0 mL of the HCl?
• What is the molarity of an H2SO4 solution if it takes 5.0 mL of .20 M NaOH solution to neutralize 4.0 mL of the HCl?
Bronsted-Lowry acids and basesdoes not need to be in water
• What is the hydronium ion concentration if the hydroxide ion concentration of a solution is 1.0 x 10 -2?
• What is the hydroxide ion concentration if the hydronium ion concentration of a solution is 2.0 x 10 -4?
• Acid - more hydronium ions than hydroxide ions
• Base - more –hydroxide ions than hydronium ions
pH = –log[H3O+]
• Log in base 10 • number to which 10 must
be raised to equal that number
• Log of .10 = ?• .10 = 10 -1
• log = -1
• Log of .010 = ?• .010 = 10 -2
• log = -2
• What is the pH of a solution that has a hydronium in concentration of .10 M?
• pH =1• What is the pH of a solution
that has a hydronium in concentration of .010 M?
• pH =2
hydronium hydroxide pH Acid/base 0.100 0.01 1.0 X 10 -7
1.0 x 10 -12
1.0 x 10 -9
What is the pH of a solution if the hydronium ion concentration is 2.5 x 10 -3 M ?
• Estimate
• On calculator enter -log[H3O+] =
Given pH find hydronium ion concentration
• pH = 1 hydronium ion concentration = .10 M or 10-1 M• pH = 2 = = .010 M or 10-2 M• pH = 9 = 10-9 M• pH = 12 10-12 M• What is the hydronium ion concentration of a solution that
has a pH of 4.8?• On calculator enter 10 x (2nd log button) - pH
pH scale• 0_________________________________ 7_____________________________________14• acid neutral base (alkaline)
• H3O+ > OH- OH- > H3O+
• The lower the pH the more acidic The higher the pH the more basic