if i have a 1:1 mole ratio as with this reaction:
NaOH + HCl --> NaCl + H20
and i use same volumes (50mL) and same Molaritys (1.00M) then there is no limiting reactant correct??
That is correct.
thank you :)
To determine if there is a limiting reactant in a reaction, you need to compare the number of moles of each reactant involved. In this case, since the reaction has a 1:1 mole ratio, it means that for every 1 mole of NaOH, you need exactly 1 mole of HCl.
To find the number of moles of a substance, you can use the formula:
moles = volume (in liters) x molarity
Given that the volume is the same (50 mL) and the molarity is the same (1.00M) for both NaOH and HCl, the number of moles of each substance would be:
moles of NaOH = (50 mL) / 1000 mL/L x (1.00 mol/L) = 0.050 mol
moles of HCl = (50 mL) / 1000 mL/L x (1.00 mol/L) = 0.050 mol
Since the number of moles of both NaOH and HCl is the same, there is no limiting reactant in this case. This means that both reactants are in excess, and they will react completely based on the 1:1 mole ratio.