Mrs. Frankenberg also showed us this chart to help you know what to do next in this type of stoichiometry questions:
A question we practiced with involved an aqueous solution of sodium sulfate and lead nitrate, forming a solid lead sulfate precipitate. It wanted to know the mass of lead sulfate formed when 1.25 liters of 0.0500 M lead nitrate and 2.00 liters of 0.0250 M sodium sulfate are mixed.
To find the mass, we first had to use the molarity formula of moles of solute/ total volume of solution to find the amount of moles in each of the reactants. We then converted the moles of each on two separate equations to grams of lead sulfate formed using a mole to mole ratio. Whichever reactant produced a smaller amount of lead sulfate was the mass of lead sulfate, since it was the limiting reagent.
Here are a couple links with practice problems:
Stoichiometry using molarity ws
Solution stoichiometry
Great post Lilly! I like how you put an example problem into this blog post and included a thorough explanation of how to solve it. I also found your links helpful in practicing stoichiometry problems with molarity!
ReplyDeleteThis is a great post too! I like how you described stoich and molarity and also included the chart that she showed us to be most helpful. The links are interesting too :)
ReplyDeleteThis is a great post too! I like how you described stoich and molarity and also included the chart that she showed us to be most helpful. The links are interesting too :)
ReplyDeleteThanks for this post! I like how you explained everything, and the chart helped me too
ReplyDeleteThanks for this post! I like how you explained everything, and the chart helped me too
ReplyDelete