calculate how much 0.100 M NaOH is needed to react completely in 45 mL of 0.0500 M HCl
mL HCl x M HCl = mL NaOH x M NaOH
To calculate how much 0.100 M NaOH is needed to react completely with 45 mL of 0.0500 M HCl, we need to first determine the balanced chemical equation for the reaction between NaOH and HCl:
NaOH + HCl -> NaCl + H2O
From the balanced equation, we can see that one mole of NaOH reacts with one mole of HCl to produce one mole of NaCl and one mole of water.
Next, we need to determine the number of moles of HCl present in 45 mL of the 0.0500 M HCl solution. To do this, we use the formula:
moles = (concentration in M) x (volume in liters)
First, we convert the volume of the HCl solution from milliliters to liters:
45 mL = 45/1000 = 0.045 L
Now we can calculate the number of moles of HCl:
moles of HCl = (0.0500 M) x (0.045 L) = 0.00225 moles
Since the reaction is stoichiometric, it means that 1 mole of HCl reacts with 1 mole of NaOH. Therefore, in order to completely react with 0.00225 moles of HCl, we will need 0.00225 moles of NaOH.
Lastly, we can calculate the volume of 0.100 M NaOH solution needed to obtain 0.00225 moles of NaOH:
volume of NaOH solution = (moles of NaOH) / (concentration in M)
volume of NaOH solution = 0.00225 moles / 0.100 M = 0.0225 L
Since the volume is given in liters, we can convert it to milliliters by multiplying by 1000:
volume of NaOH solution = 0.0225 L x 1000 = 22.5 mL
Therefore, to completely react with 45 mL of 0.0500 M HCl, you would need 22.5 mL of 0.100 M NaOH solution.