You have 14.0mL of a 0.12M NaOH solution. How many moles of HCl will it take to neutralize this solution?
same as # mols NaOH
mols NaOH = M x L
To determine the number of moles of HCl required to neutralize the NaOH solution, you need to use the concept of stoichiometry. The balanced chemical equation for the reaction between NaOH (sodium hydroxide) and HCl (hydrochloric acid) is:
NaOH + HCl -> NaCl + H2O
From the balanced equation, you can see that 1 mole of NaOH reacts with 1 mole of HCl to produce 1 mole of NaCl and 1 mole of water.
Given that you have 14.0 mL of a 0.12 M NaOH solution, you first need to convert the volume into moles. To do this, follow these steps:
Step 1: Convert the volume of the solution to liters.
14.0 mL = 14.0 mL * (1 L / 1000 mL) = 0.014 L
Step 2: Calculate the number of moles of NaOH.
moles of NaOH = volume (L) * concentration (M)
moles of NaOH = 0.014 L * 0.12 M = 0.00168 moles
Since the balanced equation shows a 1:1 mole ratio between NaOH and HCl, the number of moles of HCl required to neutralize the solution is also 0.00168 moles.