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Normality

Normality. Dr. Steve Badger. Number of moles of solute. Molarity =. Liter of solution. Number of moles of solute. Molality =. Kg of solvent. Concentrations of Solutions. A brief review of molarity & molality. Preparing a Solution of Known Molarity.

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Normality

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  1. Normality Dr. Steve Badger

  2. Number of moles of solute Molarity = Liter of solution Number of moles of solute Molality = Kg of solvent Concentrations of Solutions A brief review of molarity & molality

  3. Preparing a Solution of Known Molarity

  4. Would you use a volumetric flask to prepare a solution of known molality? How would you prepare a solution of known molality?

  5. Number of moles of solute Molarity = Liter of solution Number of equivalents of solute Normality = Liter of solution Another way to express solution concentration • Now that you understand molarity… …let’s consider normality!

  6. What’s an equivalent ? • An equivalent of a substance is the mass (grams) of that substance that will combine with one mole of another reactant. • In an acid-base reaction, an equivalent is that amount of a substance that reacts with or liberates 1.0 mole of H+.

  7. What’s an equivalent ? • An equivalent of a substance is the mass (grams) of that substance that will combine with one mole of another reactant. • In a redox reaction, an equivalent is that amount of a substance that gains or loses 1.0 mole of e–s.

  8. Making a 1.00N Solution • Calculate the mass of one equivalent of the substance, then measure that number of grams of the substance. • Put that substance in…. ?? • Add how much solvent?

  9. Preparing a Solution of Known Normality

  10. AbNormality? • Why don’t many modern chemistry textbooks cover normality? • If we take a dimensional analysis approach to problems solving, normality is a superfluous concept. • Consider the following problem:

  11. H2SO4 + KOH H2O + K2SO4 What volume of a 0.500 M KOH solution is required to titrate 10.0 mL of a 0.20 M H2SO4 solution? Could we just use this equation? MaVa = MbVb

  12. Here’s what we’d get if we used MaVa = MbVb 0.20 M H2SO4X 10.0 mL = 0.500 M KOH X ? mL Solving this, we get 4.0 mL of0.500 M KOH. But is this correct? No, it’s wrong! Why? So let’s see how we solve this correctly.

  13. H2SO4 + KOH H2O + K2SO4 M M rx volume acid moles acid moles base volume base base acid coef. What volume of a 0.500 M KOH solution is required to titrate 10.0 mL of a 0.20 M H2SO4 solution? BALANCE THE CHEMICAL EQUATION!

  14. H2SO4 + 2KOH 2H2O + K2SO4 M M rx volume acid moles acid moles base volume base base acid coef. ___ mol H2SO4 __ mol KOH ____ ml soln x x x ____ mL soln __ mol H2SO4 ____ mol KOH What volume of a 0.500 M KOH solution is required to titrate 10.0 mL of a 0.20 M H2SO4 solution? 10.0 mL = ___ mL

  15. M M rx volume acid moles acid moles base volume base base acid coef. 0.20 mol H2SO4 2 mol KOH 1000 ml soln x x x 1000 mL soln 1 mol H2SO4 0.500 mol KOH What volume of a 0.500 M KOH solution is required to titrate 10.00 mL of a 0.20 M H2SO4 solution? H2SO4 + 2KOH 2H2O + K2SO4 10.0 mL = 8.0 mL

  16. M M rx volume acid moles acid moles base volume base base acid coef. 0.20 mol H2SO4 2 mol KOH 1000 ml soln x x x 1000 mL soln 1 mol H2SO4 0.500 mol KOH Notice this! 10.0 mL = 8.0 mL Notice this! This is what makes normality superfluous!

  17. Is the following statement true or false? • Any volume of a base will completely react with (neutralize) that same volume of acid if the two solutions have the same normality (vice versa too). • In other words, is this true: NaVa = NbVb

  18. Is the following statement true or false? • Any volume of a reducing agent will completely react with that same volume of an oxidizing agent if the two solutions have the same normality. • In other words, is this true: NoxVox = NredVred

  19. Let’s solve a few problems using normality • Look at the handout that has sample problems and work the first one.

  20. And another thing… • We also use equivalents and milliequivalents as an amount of a substance • The same way that we use moles (mol) and millimoles (mmol) as an amount of a substance

  21. If you need more help: Come by my office and I can give you a few pages of worked examples from a Schaum’s Solved Problems Series. You can download this PowerPoint file at my EU web site: www.evangel.edu/Personal/badgers/Web/

  22. The End Now wasn’t that fascinating?

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