So I am a little confused on I may need help finding the mole ratio and possibly the empirical formula? The following data were collected from an experiment to synthesize lead iodide.  A 0.150 g sample of lead, was dissolved in 10.0 mL of 3 M nitric acid. An excess of a sodium iodide solution was added to the dissolved lead ions. A yellow precipitate lead iodide was was formed in this reaction. See the table below for the data collected and the calculations in determining the empirical formula of lead iodide from this experiment. A Mass of empty beaker 26.975 g B Mass of lead + beaker 27.125 g C Mass of lead iodide formed + beaker 27.492 g D Mass of lead (B-A) 0.150 g E Mass of lead iodide (C-A)       0.517g  F Mass of iodine (E-D)       0.367g   G Moles of Pb element        0.000724g H Moles of I element       0.00289g  J Mole ratio of I to Pb            K Empirical formula for PbxIy

A sample of an unknown sulfate compound has a mass of 0.100 g. Addition of excess barium chlo- ride solution to the sample forms a barium sulfate precipitate of mass 0.0676 g. What is the mass % of sulfate ion in the unknown sample?

A precipitation reaction involves the formation of a precipitate when aqueous solutions are mixed. Not all combinations of aqueous solutions produce precipitates, and it is important to be able to predict the ones that do. A) Complete and balance the molecular equation for the reaction between aqueous solutions of lithium fluoride and potassium chloride, and use the states of matter to show if a precipitate forms. B) Write the complete ionic equation for the reaction that takes place when aqueous solutions of lithium fluoride and potassium chloride are mixed.   C) Write the net ionic equation for the precipitation reaction, if any, that may occur when aqueous solutions of lithium fluoride and potassium chloride are mixed. If there is no net ionic equation, simply write "none."

Consider the reaction when aqueous solutions of barium hydroxide and iron(III) acetate are combined. The net ionic equation for this reaction is:

10. You mix 93.3 mL of 0.811 M silver acetate with 21.8 mL of 0.703 M sodium chloride. How many grams of precipitate would be formed? A) 2.20 g B) 0.0153 g C) 10.8 g D) 0.0757 g E) no precipitate would be formed

Consider the reaction when aqueous solutions of calcium acetate and cobalt(II) sulfate are combined. The net ionic equation for this reaction is:

2. Calculate the mass of the precipitate formed when 2.00 g of Barium Nitrate is mixed with an excess of Sodium Phosphatein water. Write out the balanced Molecular Equation .

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?

25.00 mL of 0.125 M aluminum chloride solution is mixed with 25.00 mL of 0.100 M sodium hydroxide solution. What mass of aluminum hydroxide will be formed?

What compound will react with aqueous potassium carbonate to form a precipitate? Iron (iii) chloride, ammonium acetate or Lithium phosphate.