1. A bright yellow precipitate is produced in a laboratory reaction, when lead(II) nitrate solution is reacted with potassium iodide solution. How many moles of a precipitate are produced when 256 mL of a 1.5 mol/L potassium iodide solution is reacted with excess lead(II) nitrate solution? Hint: Write a balanced chemical reaction equation first. (Record only your final answer with the correct number of significant digits and the proper units.)

In a double replacement reaction, 1.214 g of tin(ii) fluoride react with sodium phosphate to form a precipitate. If the tin (ii) phosphate precipitate weighs 1.078 g, what is the percent yield?

Converting Concentrations to Different Units   Introduction:   Depending on how the concentration unit is defined, concentration can serve as a conversion between the amount of a solute and the amount of a solution or solvent. Concentrations can therefore be helpful in a number of stoichiometry issues. The original definition of the concentration unit is frequently preferred because it contains the conversion factor.  Today, for chemists, it is suitable to make a solution in the lab using a specific concentration unit like molarity, and then convert the concentration to another unit. Today in the lab, I will prepare a sodium bicarbonate (baking soda) solution with a specific molarity. I will then translate the concentration into molality, mass percent, and mole fraction.   Procedure   The first step of this lab was to make sure I had everything I needed and that my surroundings were safe. I then looked at an empty beaker weighing paper and a balance. I first took a piece of weighing…

If 18.00 mL of 0.1000 M magnesium hydroxide reacts with 10.00 mL of hydrochloric acid, what is the molarity of the acid solution? (consider significant figures; enter the number only)