Suppose 20.8g of sodium iodide is dissolved in 250.mL of a 0.70 M aqueous solution of silver nitrate. Calculate the final molarity of ALL IONS in the solution after the reaction. You can assume the volume of the solution doesn't change when the sodium iodide is dissolved in it.
Round your answer to 3 significant digits.
Write the balanced equation
Write the Net Ionic equation
Calculate the final molarity of ALL IONS in the solution after the reaction.
What is the theoretical yield of the product? Identify the product.
If a chemist isolates 25.7 g of product, what is the % yield?
