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22 Cards in this Set
- Front
- Back
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A Generalized Arrhenius Acid
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HA(aq) <--> H+(aq) + A-(aq)
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A Generalized Arrhenius Base
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MOH(aq) <--> M+(aq) + OH-(aq)
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Bronsted-Lowry Acid
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A substance that can transfer H+
(a proton donor) When HA is placed in water, it reacts reversibly in an acid-dissociation equilibrium. |
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Bronsted-Lowry Base
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A substance that can accept H+
(a proton acceptor) |
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Name Seven Strong Acids
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Hydroiodic Acid HI
Hydrobromic Acid HBr Hydrochloric Acid HCl Nitric Acid HNO3 HClO3 Perchloric Acid HClO4 Sulfuric Acid H2SO4 |
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What is The Effect of Acid on Solubility for Salts that contain the conjugate of a weak acid?
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Salts that contain the conjugate of a weak acid become more soluble as the acidity of the solution increases
Examples MgCO₃, Ba(OH)₂, CuS |
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What is The Effect of Acid on Solubility for Salts that contain the conjugate of a strong acid?
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Salts that contain the conjugate of a strong acid will not affect solubility because strong acids dissociate 100%
Examples AgI, PbBr₂ |
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The Effect of Acid on Solubility
How to approach the problem of Identify the effect of increasing acidity on the solubility of the given compounds. |
Look at the anion of each salt. If the anion is the conjugate base of a weak acid, then the solubility increases with acidity.
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Why does the addition of acid increase the solubility of calcium phosphate?
Ca3(PO4)2(s) ⇆ 3Ca(2+)(aq)+ 2PO4^(3-)(aq) |
It decreases the phosphate ion concentration, forcing the equilibrium to the right.
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How is an ionic compound called SALT formed?
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It occurs when an acid neutralizes a base
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Which ions do not react appreciably with water to produce either H3O+ or OH- ions?
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Cations from Strong Bases: Li+, Na+, K+, CA+2, Sr+2, BA+2
Anions from strong monoprotic acids: Cl-, Br-, I-, NO3- and ClO4- Salts that contain only the above ions give neutral solutions in pure water (pH=7) |
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In which of the following would silver chloride be most soluble?
1M K2CO3 1M HCl 1M AgNO3 1M CaCl2 |
1M K2CO3
silver chloride will be most soluble in a solution that does not contain any silver ions or chloride ions. |
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pKa = -log Ka
Ka = Acid Dissociation Constant pKa = 14 - pKb |
pKa = -log Ka
Ka = Acid Dissociation Constant pKa = 14 - pKb |
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Kw = Ka x Kb
Kw = [H+][OH-] |
Kw = 1 x 10^14
[H+] = Kw / [OH-] |
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pH = -log[H+]
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pOH = -log[OH-]
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monoprotic acids
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acids capable of donating ONE H+ only
Examples Hcl, HNO3, CH3CO2H (weak acid) |
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polyprotic acids
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acids capable of donating > 1 H+
Examples, H2SO4, H3PO4, H2CO3 (sulfuric acid, phosphoric acid and carbonic acid, respectively) |
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polyprotic base
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can accept >1 H+ ion
CO3(-2), SO4(-2), PO4(-3), C2O4(-2) |
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What does amphiprotic mean?
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can accept or donate H+ ions
Example, HPO4(-2) a compound that can combine with water to make either H+ or OH- ions |
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STRONG Bases
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NaOH, LiOH, KOH,
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Dissociation of H20 is known as what?
H20(l) + H2O(l) ⇆ H3O+(aq) + OH-(aq) |
Auto Ionization
H20(l) + H2O(l) ⇆ H3O+(aq) + OH-(aq) |
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Ion-Product Constant for Water
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Kw = [H3O+] [OH-] = 10^-7 x 10^-7 = 10^-14
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