5. 14.0 g of cobalt(III) chloride are mixed with water to give 250.0 mL of solution. 15.00 mL of this solution is diluted with water to a total volume of 100.0 mL. Determine the molarity of chloride ion in the ending solution. Your answer

The three drawings below represent aqueous ionic solutions. Solution A has a total volume of 25 mL, solution B has a total volume of 50. mL, and solution C has a total volume of 100. mL. If each sphere represents 0.011 mol of ions, calculate the total molarity of solute.

19.3 mL of a 2.8 M solution of lithium hydroxide is used to prepare a solution with a concentration of 0.088 M. What volume of the new solution was made (in mL)?

If 30.0 g of NaI (MM = 149.89 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of NaI in the resulting solution?

Solid sodium sulfide is slowly added to 150 mL of a 0.454 M manganese(II) nitrate solution until the concentration of sulfide ion is 0.0268 M. The mass of manganese(II) ion remaining in solution is  grams.

What is the concentration (in molarity) of a solution of HCI of unknown concentration when 24.88 mL of acid is titrated to the end point with 21.19 mL of a 0.189 M NAOH solution.

Calculate the molar concentration (molarity) of a dilute barium hydroxide solution if a 50.00 mL sample yields 0.1791 g of barium sulfate when titrated with sulfuric acid.  Round to three significant figures.

An aqueous solution of sodium hydroxide is standardized by titration with a 0.123 M solution of hydrobromic acid. If 24.6 mL of base are required to neutralize 10.8 mL of the acid, what is the molarity of the sodium hydroxide solution? M sodium hydroxide

A sample is a mixture of the salts and silver nitrate, copper (II) chloride, and iron (III) chloride. When a 1.000 g sample of the mixture is dissolved in water and reacted with excess silver nitrate, 1.7809 g of precipitate forms. When a separate 1.000g sample of the mixture is treated with a reducing agent, all the metal ions in the sample are reduced to pure metals. The total mass of the metals produced is 0.4684g. Calculate the percent of each salt in the original mixture.

0.8888 g a mixture contains calcium chloride and potassium nitrate. To determine the % of each compound, silver nitrate was added to these solutions to precipitate all the chlorine in a form of silver chloride. 1.885 grams of silver chloride was precipitated, washed and dried. Calculate the % of calcium chloride in the sample.