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Concentrations of solutions
- 1. Solutions Molarity •Two solutions can contain the same compounds but be quite different because the proportions of those compounds are different. • Molarity is one way to measure the concentration of a solution. moles of solute volume of solution in liters Molarity (M) =
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- 4. Solutions Mixing aSolution
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- 8. Solutions Using Molaritiesin Stoichiometric Calculations
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- 10. Solutions Titration Theanalytical technique in which one can calculate the concentration of a solute in a solution.
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- 14. Solutions Ways of Expressing Concentrations of Solutions
- 15. Solutions Mass Percentage Mass % of A = mass of A in solution total mass of solution × 100
- 16. Solutions Parts perMillion and Parts per Billion Parts per Million (ppm) ppm = mass of A in solution total mass of solution × 106 Parts per Billion (ppb) ppb = mass of A in solution total mass of solution × 109
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- 18. Solutions Mole Fraction(X) moles of A total XA = moles in solution • In some applications, one needs the mole fraction of solvent, not solute— make sure you find the quantity you need!
- 19. Solutions Molarity (M) mol of solute M = L of solution • You will recall this concentration measure from Chapter 4. • Because volume is temperature dependent, molarity can change with temperature.
- 20. Solutions Molality (m) mol of solute m = kg of solvent Because both moles and mass do not change with temperature, molality (unlike molarity) is not temperature dependent.
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- 22. Solutions Conversion ofconcetration units
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- 24. Changing Molarity toMolality Solutions If we know the density of the solution, we can calculate the molality from the molarity, and vice versa.