7.2: Mole Ratios and Reaction Stoichiometry Pre-lab Assignment
- Page ID
- 306775
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\[ \text{Sodium bicarbonate + hydrochloric acid} \ce{->} \text{sodium chloride + carbon dioxide + water} \label{1}\]
\[ \text{Sodium carbonate + hydrochloric acid} \ce{->} \text{sodium chloride + carbon dioxide + water} \label{2}\]
\[ \ce{1 NaHCO3(s) + 1HCl(aq) -> 1 NaCl(aq) + 1 H2O(g) + 1 CO2(g)} \label{3}\]
\[ \ce{1 Na2CO3(s) + 2 HCl (aq) -> 2 NaCl(aq) + 1CO2(g) + 1 H2O(l)} \label{4}\]
Questions
-
Calculate the molar mass for the following compounds:
- NaHCO3:
- Na2CO3:
- Your goal in this lab is to experimentally verify the mole-to-mole ratios between a certain reactant and a certain product in both reactions. Identify the two substances in Reaction \ref{4}.
- In Reaction \ref{3}, you will react a pre-weighed sample of sodium bicarbonate with acid. In Reaction \ref{4}, you will use sodium carbonate instead of the bicarbonate. Name the "container" that you will perform both reactions in.
- What is the purpose of the watch glass?
- How will you know when enough acid has been added to the sodium bicarbonate (in Reaction \ref{3}) or sodium carbonate (in Reaction \ref{4}), and that the reactions are complete?
- After mixing the reactants together, you will then use a Bunsen burner to heat the contents of the reaction "container". When should you stop heating?
- Once heating is complete, you will then weigh the substance that remains in the reaction "container". What is the name of this substance?
- The mass of this substance could be described as your (circle one): theoretical yield/experimental yield/percent yield