I need help. please show step by step?
How many milliliters of 1.0 M NaOH would be required to completely neutralize 40.0 mL of 0.60 M
HCl?
mols HCl - M x L = ?
Equn is HCl + NaOH ==>NaOH + H2O so the ratio is 1 mol HCl to 1 mol NaOH. That means mols NaOH = mols HCl and you have that from above.
Then M NaOH = mols NaOH/L NaOH. you have M and mols, solve for L and convert to mL.
To find the volume of NaOH required to completely neutralize HCl, we can use the concept of stoichiometry. The balanced chemical equation for the reaction between NaOH and HCl is as follows:
NaOH + HCl -> NaCl + H2O
Here's how you can calculate the volume of 1.0 M NaOH needed to neutralize 40.0 mL of 0.60 M HCl step by step:
Step 1: Determine the balanced equation
The balanced equation shows that the stoichiometric ratio between NaOH and HCl is 1:1. This means that one mole of NaOH reacts with one mole of HCl.
Step 2: Calculate the number of moles of HCl
Use the molarity (0.60 M) and volume (40.0 mL) of HCl to find the number of moles. Remember that the volume needs to be converted from milliliters to liters:
Number of moles of HCl = (0.60 M) x (40.0 mL / 1000 mL/1 L) = 0.024 moles
Step 3: Determine the volume of NaOH required
Since the stoichiometric ratio between NaOH and HCl is 1:1, the number of moles of NaOH required to neutralize HCl is also 0.024 moles.
Now, we can use the molarity of NaOH (1.0 M) to calculate the volume of NaOH needed. Rearrange the equation:
Molarity = Moles / Volume
Volume of NaOH = Moles / Molarity = 0.024 moles / 1.0 M = 0.024 L
Finally, convert the volume from liters to milliliters:
Volume of NaOH = 0.024 L x (1000 mL/1 L) = 24.0 mL
Therefore, 24.0 mL of 1.0 M NaOH would be required to completely neutralize 40.0 mL of 0.60 M HCl.