50.00 mL of 0.567 M aqueous NaOH solution and 75.00 mL of 0.348 M aqueous HCl solution were combined in a simple (coffee cup) calorimeter. Determine how many moles of NaOH will actually react in this calorimeter.
This is another problem that is not a calorimeter problem. It is a simple stoichiometry problem.
NaOH + HCl ==> NaCl + H2O
mols NaOH = mols x L = 0.567 M x 0.0500 L = 0.0283
mols HCl = 0.348 x 0.075 = 0.0261
Since this is a 1:1 reaction (1 mol NaOH to 1 mol HCl), then 0.0261 mols NaOH will react. mols NaOH unreacted will be 0.0283 - 0.0261 = ?
A 50 ml of 10 Molar aqueous sodium hydroxide solutions from solid NaOH.
To determine the number of moles of NaOH that will react in the calorimeter, we need to first identify the limiting reagent, i.e., the reactant that will be completely consumed in the reaction.
To do this, we can use the stoichiometry of the balanced chemical equation for the reaction between NaOH and HCl. The balanced equation is:
NaOH + HCl → NaCl + H2O
From the balanced equation, we can see that the ratio of moles of NaOH to moles of HCl is 1:1. This means that for every 1 mole of NaOH, 1 mole of HCl is required for complete reaction.
Let's calculate the number of moles of HCl present in the solution using the given concentration and volume:
moles of HCl = concentration of HCl × volume of HCl solution
= 0.348 M × 0.07500 L
= 0.0261 moles
Now, since the stoichiometry of the reaction is 1:1, the number of moles of NaOH that will react is also 0.0261 moles.
Therefore, 0.0261 moles of NaOH will react in the calorimeter.