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Assignment #64 Concentration

Assignment #64 Concentration. Percent Mass. Percent Mass. Percent Mass. 15.0 grams of sodium chloride is dissolved in 100. grams of water. What is the percent mass of NaCl in this solution? 13.0%. Molarity. Symbol  M Volumetric Flasks Come in Handy. Molarity.

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Assignment #64 Concentration

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  1. Assignment #64Concentration Regular Chemistry

  2. Percent Mass Regular Chemistry

  3. Percent Mass Regular Chemistry

  4. Percent Mass • 15.0 grams of sodium chloride is dissolved in 100. grams of water. What is the percent mass of NaCl in this solution? • 13.0% Regular Chemistry

  5. Molarity • Symbol  M • Volumetric Flasks Come in Handy Regular Chemistry

  6. Molarity • 13.8 grams of potassium hydroxide are added to water. If the volume of the resulting solution is 688mL, what is the molarity? • 0.357M Regular Chemistry

  7. Molarity • What mass of solute is present in 52.4mL of 2.50M nitric acid? • 8.25g Regular Chemistry

  8. Molality • Symbol  m • Kilograms Instead of Liters • Just Solvent Instead of Total Solution • Graduated Cylinders Come in Handy Regular Chemistry

  9. Mole Fraction • 12.7 grams of sodium chloride and 21.9 grams of lithium fluoride are dissolved in 260. grams of water. What is the mole fraction of lithium fluoride in this solution? • χLiF = 0.0545 • Chi • No Units Regular Chemistry

  10. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • Balanced Equation Regular Chemistry

  11. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • Al(s.) + HBr(aq.) Regular Chemistry

  12. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • Al(s.) + HBr(aq.) AlBr3(aq.) + H2(g.) Regular Chemistry

  13. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • 2 Al(s.) + 6 HBr(aq.) 2 AlBr3(aq.) + 3 H2(g.) • Convert to Moles Regular Chemistry

  14. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • 2 Al(s.) + 6 HBr(aq.) 2 AlBr3(aq.) + 3 H2(g.) • 0.0324mol Al; 0.0888mol HBr • Limiting Reactant Regular Chemistry

  15. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • 2 Al(s.) + 6 HBr(aq.) 2 AlBr3(aq.) + 3 H2(g.) • 0.0324mol Al; 0.0888mol HBr • HBr is Limiting Reactant • Moles of AlBr3 Regular Chemistry

  16. Stoichiometry • 0.875 grams of aluminum is added to 14.8mL of 6.00M hydrobromic acid. What mass of aluminum bromide will be produced? • 2 Al(s.) + 6 HBr(aq.) 2 AlBr3(aq.) + 3 H2(g.) • 0.0324mol Al; 0.0888mol HBr • HBr is Limiting Reactant • 0.0296mol AlBr3 • 7.89g Regular Chemistry

  17. Summary • Percent Mass • Molarity (M) • Moles of Solute / Liters of Solution • Stoichiometry • Molality (m) • Moles of Solute / Kg of Solvent • Mole Fraction (χ) • Mole Fraction = Moles of Solute / Total Moles of Solution Regular Chemistry

  18. Tonight's Assignment Regular Chemistry

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