If 5.00 mL of 1.456 M aqueous NaOH and 5.00 mL of 1.456 M aqueous HF were each pipetted into a simple calorimeter, how many moles of HF would we expect to react?

Question

If 5.00 mL of 1.456 M aqueous NaOH and 5.00 mL of 1.456 M aqueous HF were each pipetted into a simple calorimeter, how many moles of HF would we expect to react?

Answer 1

www2.ucdsb.on.ca/tiss/stretton/CHEM2/enthal06.htm

Answer 2

This is not a calorimeter question. All of the HF would react.

mols = M x L = 1.456 M x 0.005 L = ?
Also, all of the NaOH would react. mols = M x L = 1.456 M x .005 L = ?

Answer 3

To determine the number of moles of HF that would react, we first need to calculate the number of moles of NaOH used in the reaction, which will then be used to find the number of moles of HF.

1. Calculate moles of NaOH:
- Given that we have 5.00 mL of 1.456 M NaOH solution, we can use the equation:
moles = concentration (M) x volume (L)
- Convert the given volume to liters:
volume (L) = 5.00 mL / 1000 (conversion factor from mL to L)
- Calculate the moles of NaOH:
moles of NaOH = 1.456 M x 0.00500 L

2. Determine the stoichiometric relationship between NaOH and HF:
- The balanced equation for the reaction between NaOH and HF is:
NaOH + HF → NaF + H2O
- From the equation, we can see that each mole of NaOH reacts with one mole of HF. Therefore, the moles of HF that would react would be equal to the moles of NaOH.

Thus, the number of moles of HF that would be expected to react is the same as the moles of NaOH, which can be calculated using the information provided.