1. A 4.24 g sample of a laboratory solution contains 1.42 g of acid. What is the concentration of the solution as a mass percentage? 2. Isopropyl alcohol is mixed with water to produce a solution that is 35.0% alcohol by volume. How many milliliters of each component are present in 645 mL of this solution?

1.) What mass of NaCl (in g) is necessary for 5.25 L of a 1.25 M solution? 2.) You have measured out 75.00 g of MgCl2 (formula weight: 58.33 g/mol) to make a solution.  What must your final volume be (in L) if you want a solution made from this mass of MgCl2 to have concentration of 0.175 M? 3.) You have a concentrated solution  of 5.00 M NaOH.  If you dilute 365.2 mL of this solution with water to a final volume of 2.00 L, what is the molarity of the diluted solution? 4.) What volume (in mL) of 5.00 M HCl must diluted to a final volume of 1.50 L to make a solution with a final concentration of 0.470 M?

In the laboratory, a student dilutes 13.5 mL of a 8.75 M hydrochloric acid solution to a total volume of 150.0 mL. What is the concentration of the diluted solution? Concentration =  M

A sample of 8.51 g of solid calcium hydroxide is added to 35.0 mL of 0.480 M aqueous hydrochloric acid. Write the balanced chemical equation for the reaction. Physical states are optional. chemical equation: What is the limiting reactant? hydrochloric acid calcium hydroxide How many grams of salt are formed after the reaction is complete? mass of salt: How many grams of the excess reactant remain after the reaction is complete? excess reactant remaining: g

A student in a lab takes 16.0 M aqueous stock solutions and dilutes it in a 500 mL volumetric flask with deionized water. After that the student takes 10 mL of the resulting diluted solution, and further dilutes it to 25.0 mL in a test tube. The student did so with the intention of making 25.0 mL of a 0.750 solution. In order to make the final 25.0 mL solution, how much stock solution did the student need to add to the 500 mL volumetric flask?

In the laboratory you dilute 2.56 mL of a concentrated 12.0 M hydrochloric acid solution to a total volume of 100 mL. What is the concentration of the dilute solution? M

A stock solution of KNO2 is available to prepare solutions that are more dilute. Calculate the volume, in mL, of a 2.0-M solution of KNO2 required to prepare exactly 100 mL of a 0.790-M solution of KNO2. mL

Consider a solution prepared by combining 45.0 g of BaCl2 with enough water to prepare a 750.0 mL of solution.  Assume that the volume of water added was 748 mL.  Density of water is 1.00 g/mL.  1)  What volume of this solution would be required to prepare 500.0 mL of a solution that is 0.0034 M in BaCl2?

What volume (mL) of a concentrated solution of calcium chloride (9.00 M) must be diluted to 350. mL to make a 2.75 M solution of calcium chloride?

Suppose 9.67g of sodium chloride is dissolved in 100.mL of a 0.50M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the sodium chloride is dissolved in it. Round your answer to 3 significant digits.