Describe how you would prepare 100mL of 0.02 M NaCl solution from a stock of 4.0 M NaCl.  Make sure to include the units with your final answer.

A 0.249 M sodium hydroxide solution required 25.00 mL to titrate 10.0 mL of an unknown concentration of sulfuric acid.  Calculate the molarity of the sulfuric acid solution.

It takes 23.98mLs of 0.05M HCl to react completely with 30.00mLs of a barium hydroxide solution. What is the molarity of the barium hydroxide solution?

A chemistry student needs 10.0 ml of 0.350M NaOH. The only NaOH solution in the lab has a concentration of 5.00M. What volume of 5.0M solution must be used to prepare the needed solution?     1.43 mL     0.700 mL     0.175 mL     143 mL

What mass (in grams) of sodium chloride do you need in order to make 250.0 mL of a 0.44 M sodium chloride solution?

A 21.25 g of a mixture of the solid salts, sodium chloride and lead II nitrate, is added to distilled water and stirred. The precipitate that is formed is filtered and dried. Its mass was determined to be 11.06 g. Analysis of the remaining solution shoed that the following ions were present: Pb2+, Na+ and NO3". Determine the percent (by mass) of lead (II) nitrate in the mixture. Assume 100 % yield.

1. What is the mass of the solution when 50.0 mL of 1.0 M HCI solution is mixed with 50.0 mL of 1.0 M NaOH solution? (d = 1.02 g/mL )

A student wants to prepare exactly 350. ml of a 0.2750 M aqueous potassium nitrate solution. What mass of potassium nitrate (molar mass = 101.11 g/mol) must the student dissolve in the 350. mL of solution? 7.01 128 O 9.73 28.1

10) A solution is made by diluting 348 mL of a 3.42M KCl stock solution with water to a final volume of 1.98L. What is the molar concentration of the diluted solution

You have been asked to make 250.0 mL of a 0.100 M solution of calcium nitrate. A. Calculate the mass (in g) of solid calcium nitrate needed to make the solution.