Adapted by Nelson Nuñez-Rodriguez
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By David W. Ball
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| QUESTION | ANSWER |
|
1. Using concentration as a conversion factor, how many moles of solute are in 3.44 L of 0.753 M CaCl2? |
1. 2.59 mol |
|
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? |
3. 1.24 L |
|
5. What is the mass of solute in 24.5 mL of 0.755 M CoCl2? |
5. 2.40 g |
|
7. What volume of solution is needed to provide 9.04 g of NiF2 from a 0.332 M solution? |
7. 0.282 L |
|
9. What volume of 3.44 M HCl will react with 5.33 mol of CaCO3? 2HCl + CaCO3 → CaCl2 + H2O + CO2 |
9. 3.10 L |
|
11. What volume of 0.905 M H2SO4 will react with 26.7 mL of 0.554 M NaOH? H2SO4 + 2NaOH → Na2SO4 + 2H2O |
11. 8.17 mL |
|
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. |
13. 0.1192 M |
|
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 |
15. 7.39 mg |
|
17. What mass of 3.00% H2O2 is needed to produce 66.3 g of O2(g)? 2H2O2(aq) → 2H2O(ℓ) + O2(g) |
17. 4.70 kg |