N3 Solution Stoichiometry And Molar Dilution Problems
1. What is the molarity of a solution of ammonium chloride prepared by diluting 50.00 mL of a 3.79 M NH4Cl solution to 2.00 L?
2. A student takes a sample of KOH stock solution and dilutes it with 100.0 mLof water. The student determines that the diluted solution is 0.046 M KOH, but has forgotten to record the volume of the original stock solution sample. The concentration of the stock solution is 2.09 M. What was the volume of the original sample of stock solution?
3. A chemist wants to prepare a stock solution of H2SO4 (sulfuric acid), so that a sample of 20.00 mL will produce a solution with a concentration of 0.50 M when added to 100.0 mL of water.
A) What should the molarity of the stock solution be?
B) If the chemist wants to prepare 5.00 L of the stock solution from concentrated H2SO4, which is 18.0 M, what volume of concentrated acid should be used?
4. To what volume should 1.19 mL of an 8.00 M acetic acid solution be diluted in order to obtain a final solution that is 1.50 M
5. What volume of a 5.75 M solution be used to prepare 2.00 L of a 1.00 M solution?
6. A 25.00 mL of ammonium nitrate solution produces a 0.186 M solution when diluted with 50.00 mL of water. What is the molarity of the stock solution?
7. What mass of NaCl is required to precipitate all the Ag1+ ions from 20.0 mL of 0.100 M AgNO3 solution?
8. What mass of NaOH is required to precipitate all the Fe2+ ions from 50.0 mL of 0.200 M Fe(NO3)2 solution?
9. If 25.8 mL of AgNO3 solution is required to precipitate all of the Cl ions in a 0.785-g sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution?
10. If 55.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 0.544-g sample of Na2SO4 (forming BaSO4), what is the molarity of the BaCl2 solution?
11. In the laboratory, 6.67 g of Sr(NO3)2 is dissolved in enough water to form a volume of 0.750 L. A 0.100-L sample of this stock solution is mixed with a 0.0460 M solution of Na2CrO4. What volume of Na2CrO4
2. A student takes a sample of KOH stock solution and dilutes it with 100.0 mLof water. The student determines that the diluted solution is 0.046 M KOH, but has forgotten to record the volume of the original stock solution sample. The concentration of the stock solution is 2.09 M. What was the volume of the original sample of stock solution?
3. A chemist wants to prepare a stock solution of H2SO4 (sulfuric acid), so that a sample of 20.00 mL will produce a solution with a concentration of 0.50 M when added to 100.0 mL of water.
A) What should the molarity of the stock solution be?
B) If the chemist wants to prepare 5.00 L of the stock solution from concentrated H2SO4, which is 18.0 M, what volume of concentrated acid should be used?
4. To what volume should 1.19 mL of an 8.00 M acetic acid solution be diluted in order to obtain a final solution that is 1.50 M
5. What volume of a 5.75 M solution be used to prepare 2.00 L of a 1.00 M solution?
6. A 25.00 mL of ammonium nitrate solution produces a 0.186 M solution when diluted with 50.00 mL of water. What is the molarity of the stock solution?
7. What mass of NaCl is required to precipitate all the Ag1+ ions from 20.0 mL of 0.100 M AgNO3 solution?
8. What mass of NaOH is required to precipitate all the Fe2+ ions from 50.0 mL of 0.200 M Fe(NO3)2 solution?
9. If 25.8 mL of AgNO3 solution is required to precipitate all of the Cl ions in a 0.785-g sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution?
10. If 55.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 0.544-g sample of Na2SO4 (forming BaSO4), what is the molarity of the BaCl2 solution?
11. In the laboratory, 6.67 g of Sr(NO3)2 is dissolved in enough water to form a volume of 0.750 L. A 0.100-L sample of this stock solution is mixed with a 0.0460 M solution of Na2CrO4. What volume of Na2CrO4