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Precipitation and Net Ionic Reactions

Precipitation and Net Ionic Reactions. Definitions. Solute: the substance that dissolves Solvent: the substance in which the solute is dissolved. Solution (soln.): solute dissolved in a solvent. Precipitation Reactions. Write a double replacement reaction.

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Precipitation and Net Ionic Reactions

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  1. Precipitation and Net Ionic Reactions

  2. Definitions Solute: the substance that dissolves Solvent: the substance in which the solute is dissolved. Solution (soln.): solute dissolved in a solvent.

  3. Precipitation Reactions Write a double replacement reaction. Identify the product that will precipitate. (Na+, K+, NH4+, NO3- NEVER precipitate)

  4. Complete Ionic Reactions Multiply the coefficient (big number out in front) by the subscript (little number behind) for each element (or polyatomic ion. This will be the coefficient for each ion.

  5. Net Ionic Reactions Write a net ionic reaction by writing down the ions (with appropriate coefficients and charges) that produce the precipitate on the left (reactant side) and the precipitate on the right (product side).

  6. Example #1 1. NaOH + FeCl3  2. Pb(NO3)2 + NaI  3. Cu(NO3)2 + NaOH  4. BaCl2 + Na2SO4

  7. Solubility (ability to dissolve) Solubility: mass of a solute that will dissolve in a given quantity of solvent (normally 100mL) at a particular temperature. Molarity (M): number of moles of solute that will dissolve in one liter of solvent (1L) at a particular temperature.

  8. Molarity Formula Or Molarity (Liters) = moles

  9. Solving Molarity Problems If it asks for molarity or volume: Convert grams to moles, convert milliliters to liters. Plug in to the molarity formula. If it asks for mass: Plug into the molarity formula first and solve for moles. Then do a gram-mole conversion to find grams.

  10. Example #2 A. What is the molarity of 500mL of solution that contains 40g of sodium hydroxide? B. How many grams of potassium nitrate will be needed to make 750mL of a 0.25M potassium nitrate solution?

  11. What if you are diluting a concentrated solution? Find the portion of the problem that gives you both milliliters and molarity. Plug into the molarity formula and find moles. Plug the moles you found into the molarity formula with the other molarity or volume given in the problem.

  12. Example #3 A. How many milliliters of 18M H2SO4 will be needed to make 375mL of 1.75M? B. When 35mL of 12M HCl are placed into beaker and diluted to 400mL. What is the molarity of the dilute solution? C. What volume of 15M ammonia, NH3, will be needed to make 1750mL of 6.7M NH3?

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