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Solution Chemistry

Solution Chemistry. Solutions, Problems, Solutions, Problems. Does it ever end?. How can you express concentration?. How can you express concentration?. Mass % composition Molarity Molality Mole fraction Density. Mass % problems:. Find mass % Find amount of solute

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Solution Chemistry

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  1. Solution Chemistry Solutions, Problems, Solutions, Problems. Does it ever end?

  2. How can you express concentration?

  3. How can you express concentration? • Mass % composition • Molarity • Molality • Mole fraction • Density

  4. Mass % problems: • Find mass % • Find amount of solute • Find total mass of solution

  5. Mass % problems: • Find mass % • Mass % = mass of solute x 100 % total mass of solution Don’t forget to add the masses of the solute and solvent for the total mass

  6. Mass % problems: • Find amount of solute • Mass % = mass of solute x 100 % total mass of solution • Multiply by total mass and divide by 100% to solve for mass of solute

  7. Mass % problems: • Find total mass of solution • Mass % = mass of solute x 100 % total mass of solution • Multiply both sides by the mass of solution first to get it out of the denominator.

  8. Molarity problems: • Find molarity • Find amount of solute • Find volume of solution

  9. Molarity problems: • Find molarity • M= moles solute Volume of solution (L)

  10. Molarity problems: • Find amount of solute • M= moles solute Volume of solution (L) • Molarity x volume= moles!

  11. Molarity problems: • Find volume of solution • M= moles solute Volume of solution (L) • Multiply both sides by the volume of solution first to get it out of the denominator. OR!

  12. Molarity problems: • Find volume of solution • Use the molarity as a conversion factor! • moles solute x 1 L = Volume of solution! M

  13. Dilution problems M x V = Moles • Moles of solute in new solution = moles in the stock solution. Molarity goes down, volume goes up

  14. Dilution problems Example: What is the concentration of a solution made by diluting 25 ml of a .50 M HCl solution to a new volume of 150 ml?

  15. Dilution problems Example: What is the concentration of a solution made by diluting 25 ml of a .50 M HCl solution to a new volume of 150 ml? M x V = moles. .50 M x .025 L= .0125 moles HCl M = mol/vol= .0125 mol / .150 L = .083 M

  16. Dilution Problems • What is the concentration of a solution made by diluting 125 ml of a 2.5 M NH3solution to a new volume of 350 ml? • What is the concentration of a solution made by diluting 2.5 ml of a 6.0 M NaClsolution to a new volume of 80. ml? • What is the concentration of a solution made by diluting 30. ml of a 1.0 M Fe(NO3)3solution with 20. ml of water? (The final volume should be 20. + 30. = 50. ml)

  17. Dilution problems Example: What volume of a 2.0 M NaOH stock solution is required to mix 1.50 L of a .150 M NaOH solution?

  18. Dilution problems Example: What volume of a 2.0 M NaOH stock solution is required to mix 1.50 L of a .150 M NaOH solution? M x V = moles. .150 M x 1.50 L = .225 moles NaOH .225 moles NaOH x 1 L/ 2.0 moles= .113 L

  19. Dilution problems • What volume of a 6.0 M NaOH stock solution is required to mix 1.50 L of a .150 M NaOH solution? • What volume of a 2.0 M MgCl2stock solution is required to mix .750 L of a .10 M MgCl2solution? • What volume of a 1.0 M HClstock solution is required to mix 100. ml of a .10 M HCl solution?

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