6M HCl + 1M NaOH => NaCl + H2O
If I'm understanding this correctly, all of the NaOH is used up because the molarity is 1 where the HCl's is 6 this leaves excess HCl correct?
if there are equal volumes of each fluid, yes.
Yes, you are correct. In the given chemical equation:
6M HCl + 1M NaOH → NaCl + H2O
The molarity of HCl is 6M (6 moles per liter) while the molarity of NaOH is 1M (1 mole per liter). The stoichiometric ratio between HCl and NaOH is 1:1, which means that for every 1 mole of NaOH, 1 mole of HCl is required to react completely.
Since the molarity of HCl is higher (6M) compared to NaOH (1M), it means that there is an excess of HCl present. This excess HCl does not have enough NaOH to react with, so it will remain unreacted after the completion of the reaction.
To confirm this, you can calculate the moles of HCl and NaOH present based on the given molarities and compare their ratios:
- Moles of HCl = 6M × Volume of HCl solution in liters
- Moles of NaOH = 1M × Volume of NaOH solution in liters
If the moles of HCl are greater than the moles of NaOH, it indicates that HCl is in excess.