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White Board Review

Practicing with Concentration Expressions. Molarity Percent ppm. White Board Review. Practicing with Concentrations. Molarity. Determine the molarity of 250 mL of solution containing 35 g of NaOH. What you must remember: molarity = moles of solute per liter of solution.

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White Board Review

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  1. Practicing with Concentration Expressions • Molarity • Percent • ppm White Board Review

  2. Practicing with Concentrations Molarity Determine the molarity of 250 mL of solution containing 35 g of NaOH. What you must remember: molarity = moles of solute per liter of solution 35 g NaOH = 0.250 Liters = 3.5 M NaOH

  3. Practicing with Concentrations Molarity What volume of a 2.0 M solution will provide 18 g of NaOH? What you must remember: moles solute ÷ molarity = L volume First find moles: 18 g NaOH = 0.45 mol NaOH Next, divide moles by molarity: 0.45 mol NaOH = 0.23 L or 230 mL of solution

  4. Practicing with Concentrations Molarity What mass of NaOH is needed to make 4.0 liters of a 0.75 M solution? What you must remember: L volume X molarity = moles solute First find moles solute: = 4.0 L solution 3.0 mol NaOH Next, multiply moles by molar mass: 3.0 mol NaOH = 120 g NaOH

  5. Practicing with Concentrations Molarity Determine the molarity of 850 mL of solution containing 95 g of KCl. What you must remember: molarity = moles of solute per liter of solution 95 g KCl = 0.850 Liters = 1.5 M KCl

  6. Practicing with Concentrations Molarity What volume of a 3.8 M solution will provide 120 g of LiF? What you must remember: moles solute ÷ molarity = L volume First find moles: 120 g LiF = 4.63 mol LiF Next, divide moles by molarity: 4.63 mol LiF = 1.2 L

  7. What mass of NaSCN is needed to make 550 mL of a 2.4 M solution? Practicing with Concentrations What you must remember: L volume X molarity = moles solute First find moles solute: Molarity = 0.55L solution 1.32 mol NaSCN Next, multiply moles by molar mass: 1.32 mol NaSCN = 110 g NaSCN

  8. Practicing with Concentrations Percent Determine the % w/v of 25 mL of solution containing 3.0 g of CsOH. What you must remember: % w/v = g of solute per mL of solution X 100 3.0 g CsOH = x 102 25 mL = 12 % w/v CsOH

  9. Practicing with Concentrations Percent What volume of a 6.2 % w/v solution will provide 32 g of KMnO4? What you must remember: g solute ÷ % w/v = mL volume First interpret % w/v: Next, divide the g solute by the %: 32 g = 520 mL KMnO4 solution

  10. Percent What mass of NaClO is needed to make 150 mL of a 4.9 % w/v solution? Practicing with Concentrations What you must remember: % w/v = g/100mL and mL volume X % = g solute First interpret % w/v: Next, multiply by mL volume: = X 150 mL 7.4 g NaClO

  11. Practicing with Concentrations Percent Determine the % w/v of 960 mL of solution containing 37 g of KClO3. What you must remember: % w/v = g of solute per mL of solution X 100 37 g KClO3 = x 102 960 mL = 3.9 % w/v KClO3

  12. Practicing with Concentrations Percent What volume of a 0.55 % w/v solution will provide 2.5 g of KNO2? What you must remember: g solute ÷ % w/v = mL volume First interpret % w/v: Next, divide the g solute by the %: 2.5 g = 450 mL KNO2 solution

  13. Percent What mass of NaSO4 is needed to make 500. mL of a 1.0 % w/v solution? Practicing with Concentrations What you must remember: % w/v = g/100mL and mL volume X % = g solute First interpret % w/v: Next, multiply by mL volume: = X 500. mL 5.0 g NaSO4

  14. Practicing with Concentrations ppm Calculate the concentration in ppm of 3250mL of solution containing 0.25 g of NiSeO3. What you must remember: ppm = g of solute per mL of solution X 106 0.25 g NiSeO3 = x 106 3250 mL = 77 ppm NiSeO3

  15. Practicing with Concentrations ppm What volume of a 320 ppm solution will provide 0.75 g of K2Cr2O7? What you must remember: ppm = mg/L and mg solute ÷ ppm = L volume First interpret ppm: Next, convert g to mg: = 0.75 g 750 mg Finally, divide mg solute by ppm: 750 mg = 2.3 L

  16. ppm What mass of MgSO3 is needed to make 100. mL of a 38 ppm solution? Practicing with Concentrations What you must remember: ppm = mg/L and L volume X ppm = mg solute First interpret ppm: Next, multiply by L volume: = X 0.100 L 3.8 mg MgSO3

  17. Practicing with Concentrations ppm Calculate the concentration in ppm of 25,000mL of solution containing 1.0 g of KF. What you must remember: ppm = g of solute per mL of solution X 106 1.0 g KF = x 106 25,000 mL = 40. ppm KF

  18. Practicing with Concentrations ppm What volume of a 5.0 ppm solution will provide 1.0 g of NaCN? What you must remember: ppm = mg/L and mg solute ÷ ppm = L volume First interpret ppm: Next, convert g to mg: = 1.0 g 1000 mg Finally, divide mg solute by ppm: 1000 mg = 2.0 x 102L

  19. ppm What mass of FePO4 is needed to make 500. mL of a 120 ppm solution? Practicing with Concentrations What you must remember: ppm = mg/L and L volume X ppm = mg solute First interpret ppm: Next, multiply by L volume: = X 0.500 L 60. mg FePO4

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