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Chapter 7 – Practice Problems (Concentrations as Conversion Factors)

  1. Using concentration as a conversion factor, how many moles of solute are in 3.44 L of 0.753 M CaCl2?

  2. Using concentration as a conversion factor, how many moles of solute are in 844 mL of 2.09 M MgSO4?

  3. Using concentration as a conversion factor, how many liters are needed to provide 0.822 mol of NaBr from a 0.665 M solution ?

  4. Using concentration as a conversion factor, how many liters are needed to provide 2.500 mol of (NH2)2CO from a 1.087 M solution?

  5. What is the mass of solute in 24.5 mL of 0.755 M CoCl2?

  6. What is the mass of solute in 3.81 L of 0.0232 M Zn(NO3)2?

  7. What volume of solution is needed to provide 9.04 g of NiF2 from a 0.332 M solution?

  8. What volume of solution is needed to provide 0.229 g of CH2O from a 0.00560 M solution?

  9. What volume of 3.44 M HCl will react with 5.33 mol of CaCO3?

    • 2HCl + CaCO3 → CaCl2 + H2O + CO2

  10. What volume of 0.779 M NaCl will react with 40.8 mol of Pb(NO3)2?

    • Pb(NO3)2 + 2NaCl → PbCl2 + 2NaNO3

  11. What volume of 0.905 M H2SO4 will react with 26.7 mL of 0.554 M NaOH?

    • H2SO4 + 2NaOH → Na2SO4 + 2H2O

  12. What volume of 1.000 M Na2CO3 will react with 342 mL of 0.733 M H3PO4?

    • 3Na2CO3 + 2H3PO4 → 2Na3PO4 + 3H2O + 3CO2

  13. It takes 23.77 mL of 0.1505 M HCl to titrate with 15.00 mL of Ca(OH)2. What is the concentration of Ca(OH)2? You will need to write the balanced chemical equation first.
  14. It takes 97.62 mL of 0.0546 M NaOH to titrate a 25.00 mL sample of H2SO4. What is the concentration of H2SO4? You will need to write the balanced chemical equation first.

  15. It takes 4.667 mL of 0.0997 M HNO3 to dissolve some solid Cu. What mass of Cu can be dissolved?

    • Cu + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2 + 2H2O

  16. It takes 49.08 mL of 0.877 M NH3 to dissolve some solid AgCl. What mass of AgCl can be dissolved?

    • AgCl(s) + 4NH3(aq) → Ag(NH3)4Cl(aq)

  17. What mass of 3.00% H2O2 is needed to produce 66.3 g of O2(g)?

    • 2H2O2(aq) → 2H2O(ℓ) + O2(g)

  18.  A 0.75% solution of Na2CO3 is used to precipitate Ca2+ ions from solution. What mass of solution is needed to precipitate 40.7 L of solution with a concentration of 0.0225 M Ca2+(aq)

    • Na2CO3(aq) + Ca2+(aq) → CaCO3(s) + 2Na+(aq)

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