A flask contains 50.0 mL of 1.00 M sodium hydroxide. Its contents are fully transferred to a larger flask, and enough water is added to prepare 1.00 L of solution. What is the concentration of sodium hydroxide in the diluted solution?

A solution of 49.0% H2SO4 by mass has a density of 1.39 g/cm³ at 293 K. A 25.0-cm³ sample of this solution is mixed with enough water to increase the volume of the solution to 99.8 cm³. Find the molarity of sulfuric acid in this solution.

A 100.0 mL sample is prepared from a 250.0 mL stock solution by pipetting 5.00 mL of the stock solution and diluting it until it had a molarity of 2.5 * 10^-4 M. What is the molarity of the original stock solution?

A student prepared a stock solution by dissolving 15.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of a final solution. What is the concentration of the final solution in mol/L?

A student prepared a stock solution by dissolving 20.0 g of KOH in enough water to make 150.0 mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make a final solution of 65.0 mL. What is the concentration of the final solution in mol/L?

Calculate the concentration (M) of sodium ions in a solution made by diluting 25.0 mL of a 0.765 M solution of sodium sulfide (Na2S) to a total volume of 225 mL.

Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide (Na2S) to a total volume of 300 mL.