In part B of this experiment 2.0 g of NaOH (molar mass = 40.0 g/mol) is mixed with 100 mL of 1.0 M HCl. Which one of these statements is true?Question 6Select one:This is a stoichiometric mixture, there is no limiting reagent. The limiting reagent is HCl. There is excess NaOH. The limiting reagent is NaOH.
Question
In part B of this experiment 2.0 g of NaOH (molar mass = 40.0 g/mol) is mixed with 100 mL of 1.0 M HCl. Which one of these statements is true?Question 6Select one:This is a stoichiometric mixture, there is no limiting reagent. The limiting reagent is HCl. There is excess NaOH. The limiting reagent is NaOH.
Solution
First, let's calculate the number of moles for each reactant.
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For NaOH: The number of moles = mass / molar mass = 2.0 g / 40.0 g/mol = 0.05 mol
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For HCl: The number of moles = concentration * volume = 1.0 M * 0.1 L = 0.1 mol
The balanced chemical equation for the reaction between NaOH and HCl is:
NaOH + HCl -> NaCl + H2O
From the balanced equation, we can see that the stoichiometric ratio between NaOH and HCl is 1:1. This means that 1 mole of NaOH reacts with 1 mole of HCl.
Comparing the number of moles of NaOH and HCl, we have 0.05 mol of NaOH and 0.1 mol of HCl. Since the stoichiometric ratio is 1:1, we need the same amount of NaOH and HCl for the reaction to occur completely.
Therefore, since we have less NaOH than HCl, NaOH is the limiting reagent. So, the correct statement is "The limiting reagent is NaOH."
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