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30 Cards in this Set
- Front
- Back
What will anions of strong acids do to the pH?
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No change
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What will cations of strong bases do to the pH?
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No change
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What will anions of weak acids do to the pH?
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Higher the pH
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What will cations of weak acids do to the pH?
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Lower the pH
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What will polyatomic cations with >1+ protons do to the pH? (NH_4^+ and H_3O^+)
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Lower the pH
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What will metal ions do to the pH?
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Lower the pH
Hydration-positive charge interact with the oxygen electrons Increasing metal charge=more acidic |
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What are binary acids?
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Binary acids are compounds containing H and one other element
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What are the acidity trends of binary acids?
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1. Bond strength increases with decreasing size=less acidic
2. Larger differences of electronegativity=more acidic 3. Acidity increases down a particular group |
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What is the Oxy-acids rule #1?
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For two acids with equal number of OH and O: the acid with the most electronegative central atom is more acidic
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What is the Oxy-acids rule #2?
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The OH bond becomes more polar as electron density is pulled away. Larger size conjugate bases can "spread out" the extra charge more easily
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What is the common-ion effect?
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Weak electrolyte ionization is decreased by adding a strong electrolyte that has an ion in common with the weak electrolyte
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What is the characteristic of buffered solutions?
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Because buffer solutions contain both acidic and basic species they are resistive to pH changes
-assuming the amounts of HX and X- in the buffer are large in comparison to the amount of OH- and H+ added. -And the weak acid/base was not used up |
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What do you use to find the initial pH of a titration?
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Normal ICE table
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What do you use to find the pH before the equivalence point?
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BCA table, the used henderson-hasselbalch equation
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What do you use to find the pH at the equivalence point?
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BCA table, the ICE table with the conjugate reacting with water
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What do you use to find the pH after the equivalence point?
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BCA table, the find the pH based on just the strong acid or base
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Solubility?
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how much solid will dissolve before a solution becomes saturated....g/L
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Molar solubility?
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how many moles dissolve to make the saturated solution....mol/L
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Solubility-The Common-ion effect?
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In general, the solubility of a slightly soluble salt is decreased by the presence of a second solute that furnishes a common ion
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Complex ions?
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Metal complexes are formed as Lewis bases share non-bonding electrons with vacant orbitals on the metal
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Amphoteric substances?
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Amphoteric substances are soluble in strong acid or strong base, but insoluble at neutral pH
Examples: Al^3+, Cr^3+, Zn^2+, Sn^2+ |
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K_sp < Q
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Then precipitation until Q=K_sp
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K_sp=Q
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Saturated solution
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K_sp>Q
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Then all of solid dissolves
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What are the three factors that affect solubility?
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1. The presence of common ions
2. The pH of a solution will affect the solubility of any substance where the anion is basic 3. Formation of complex ions |
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What is the first law of thermodynamics?
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Energy is conserved(not created or destroyed)
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What is the second law of thermodynamics?
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In any irreversible(spontaneous) process the entropy of the universe increases
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What is the third law of thermodynamics?
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Entropy of a pure crystalline substance at absolute zero is zero
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Entropy increases with???
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1. increased temperature of atoms/molecules
2. increased volume for atoms/molecules to move in 3. increased number of independently moving objects |
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What are the factors that effect spontaneity?
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1. Enthalpy
2. Temperature 3. Entropy |