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Sandstone
- It depends on the rock formation
- Could be CaCO3, MgFe, SiO2
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Hydrocarbon (Bicarbonate)
HCO3-
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Van't Hoff 10K Rule
Reaction Rate doubles with every 10 degrees K increase in temperture
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Le Chatelier's Principle
- If a chemical system at equilibrium experiences a change in:
- 1. Concentration
- 2. Temperature
- 3. Volume
- 4. Total Pressure
- Then the system will shift in order to counteract the change.
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Exothermic
- deltar H =neg value
- Releases Heat
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Endothermic
- deltar H=positive value
- Absorbs Heat
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Temperature Independant
- deltar H= 0
- Change in temperature has no effect on the system
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Equilibrium Constants (k)
- Temperature Dependent
- Reaction Specific
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How do strong electrolytes dissociate in water?
completely
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How do weak electrolytes dissociate in water?
incompletly
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What is electrical conductivity?
Sum parameter for ions in aqueous solutions.
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Electrical conductivity depends on...
- Concentration (Activity)
- Temperature
- Ion Mobility
- Type of Electrolyte
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What is the dissociation process?
- 1. Breaking of lattice
- 2. Hydration of ions to keep ions apart (shield charges)
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Does each ion have the same number of water molecules in its hydrate shell?
No ions are charged differently depending on density and size
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What is an ideal solution?
Ions are so well shielded by a hydrate shell that there is no electrostatic forces between them.
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What is a non-ideal solution?
Electrostatic forces between ions exist
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What does I>0.01 M mean?
- Concentration of free ions does not equal the total concentration
- Ions interact electrostatically (non-ideal solution)
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What are activity coefficients used for?
Adjusting solutions with I>0.01M (non ideal solutions) molar concentrations to effective concentrations (activity).
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What is Ionic strength?
The measure of ions in a charged solution
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Salts are more soluble in...
hot water
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Alkali Metal Salts are...
very soluble in water
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What are some Alkali Metal Salts???
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Salts containing nitrate ion (NO3-) are...
very soluble in water.
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Most salts containing Cl-, Br-, I- are....
very soluble in water
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Salts containing Ag+ and Pb2+ are
not soluble in water
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Are FeCl2, AlBr3, MgI2 soluble salts?
Yes
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Are AgCl, PbBr2 soluble salts?
No
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Weak electrolytes are...
insoluble in water
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Strong electrolytes are...
soluble in water
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What is the Saturation Index (SI) of a mineral in equilibrium in an aqueous solution?
SI=0
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What is the Saturation Index (SI) of a mineral in an under-saturated aqueous solution?
SI<0
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What is the Saturation Index (SI) of a mineral in a super-saturated aqueous solution?
SI>0
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Is it possible to compare Ksp values?
No, Ksp values must be converted to Solubility (S) and then compared.
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Gases are more soluble in...
cold water
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What is the effect of adding NaF to a CaF2 solution?
- The common ion effect
- Increase in [F-] makes the ion product greater than the solubility product (Ksp)
- Until equilibrium is reestablished CaF2 will precipitate out of the solution
- Over all result of adding a common ion is a decrease in the solubility of the salt in the solution
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What is the Common Ion Effect?
- Le Chatelier Principal
- The increase in common ion makes the ion product larger than the solubility product (Ksp)
- Until equilibrium is reestablished the salt in the solution will precipitate out
- Overall result of adding a foreign ion is the decrease in solubility of the salt in the solution
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What is the effect of adding NaCl to a CaSO4 solution?
- Foreign Ion Effect
- The concentration of Ca2+ and SO4- increases
- The activity coefficient (f) of Ca2+ and SO4- decreases
- This occurs until equilibrium and the solubility product (Ksp) is reestablished again.
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What is the foreign ion effect?
- The addition of a foreign ion causes the system to shift out of equilibrium
- Ionic strength (I) increases
- Concentration (C) of the products in solution to increase and the activity coefficient (f) decreases
- This process occurs until equilibrium is reestablished
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Enthalpy (delta H) depends on...
Temperature
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What are some ions who's concentration is controlled by other ions?
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For Endothermic Processes (+ delta H) solubility....
increases with increasing temperature
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For Exothermic Processes (-delta H) solubility....
decreases with increasing temperature.
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For Endothermic reactions the Lattice Enthalpy is....
> Hydration Enthalpy
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For Exothermic reactions the Lattice Enthalpy is....
<Hydration Enthalpy
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What is lattice enthalpy?
Strength of forces between ions in an ionic solid
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What is Hydration Energy?
- Energy released upon attachment of water molecules to ions.
- Special case of dissolution energy
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What is an Example of Hydration Energy?
- Dissolving a salt in water
- Outermost ions (those at the edge of the lattice) move away from the lattice and become covered with the neighboring water molecule
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If Hydration Energy >= Lattice Energy then
the salt soluble in water
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For Ionic Strength (I) do not multiply by....
charge and consider all of the molecules present in the water sample
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When claculating Ionic Balance mulitply mol/L of substance by....
- charge
- only consider major and minor ions in the water sample
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