give the balanced molecular equation: solutions of aluminum acetate and potassium phosphate are mixed

If 26.8 g of KBr (MM = 119.00 g/ mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KBr in the resulting solution?

You mix 500.0 ml of 0.250 M iron(III) chloride solution with 225.0 mL of 0.350 M barium chloride solution. Assuming the volumes are additive, what is the molarity of chloride ion in the mixture.

What mass of copper II hydroxide precipitate is produced by the double displacement reaction in a solution of 2.67 g of potassium hydroxide with excess aqueous copper II nitrate?

Calculate the volume (mL) of 1.0 M metal nitrate solution required to prepare 5.0 g of the COBALT pigment. Again, using the balanced chemical equation you should be able to relate the moles of pigment to the moles of metal nitrate and from that calculate the volume of 1.0 M metal nitrate solution required. Please report your value as XX.X mL (one decimal point and no units).

1) Lead (I) nitrate reacts with sodium chloride. A) Write a balanced chemical equation to describe this reaction B) 100.0 mL of a lead (I) nitrate solution reacts with excess sodium chloride solution and produces 6.95 grams of precipitate. 2) Calculate the moles of the precipitate produced by the reaction. A) Calculate the moles of lead in the original solution. B) Calculate the molarity of the 100.0 mL lead (I) nitrate solution.

What are the spectator ions present when aqueous solutions of ammonium chromate and lead(II) acetate are mixed?

Consider two aqueous solutions: one of lithium hydroxide and one of calcium chloride.  List the ions present in each.  Is a precipitate formed when the two solutions are mixed?  If so, write the molecular, ionic and net ionic equation. Identify the spectator ions.

Write the balanced molecular chemical equation for the reaction in aqueous solution for copper(1) chloride and lithium carbonate. If no reaction occurs, simply write

You wish to make a 0.384 M hydrobromic acid solution from a stock solution of 3.00 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution?