The flask shown contains 10.0 mL of HCl and a few drops of phenolphthaein indicator. The buret contains 0.270 M NaOH.
What volume of NaOH is needed to reach the end point of the titration?
What was the initial concentration of HCl?
You have a volume of HCl and no M. You have a M of NaOH and no volume. Something is missing, probably because you can't post the picture.
To find the volume of NaOH needed to reach the endpoint of the titration, we need to use the concept of stoichiometry and the balanced chemical equation for the reaction.
Step 1: Write the balanced chemical equation for the reaction.
HCl + NaOH -> NaCl + H2O
Step 2: Determine the mole ratio between HCl and NaOH.
From the balanced equation, we can see that the mole ratio between HCl and NaOH is 1:1. This means that 1 mole of HCl reacts with 1 mole of NaOH.
Step 3: Convert the volume of HCl to moles.
We are given that the flask contains 10.0 mL of HCl. Since we are going to convert to moles, we need to convert mL to L by dividing by 1000.
10.0 mL / 1000 = 0.010 L
The concentration of HCl is not given, so we'll need additional information or an assumption to determine the initial concentration of HCl.
Assuming the initial concentration of HCl is the same as the concentration of NaOH (0.270 M), we can proceed with the calculations.
Step 4: Calculate the number of moles of HCl.
Number of moles = concentration x volume
Number of moles of HCl = 0.270 M x 0.010 L
Step 5: Determine the volume of NaOH needed to react completely with the HCl.
Since the mole ratio between HCl and NaOH is 1:1, the moles of NaOH needed is the same as the moles of HCl.
Step 6: Convert the moles of NaOH to volume.
Number of moles = concentration x volume
Volume of NaOH = Number of moles / concentration
So, the volume of NaOH needed to reach the endpoint of the titration is equal to the number of moles of HCl, which can be calculated using the formula:
Volume of NaOH = (0.270 M x 0.010 L) / 0.270 M
Now, let's calculate the volume of NaOH needed:
Volume of NaOH = (0.270 M x 0.010 L) / 0.270 M
Volume of NaOH = 0.010 L
Therefore, the volume of NaOH needed to reach the endpoint of the titration is 0.010 L.
To find the initial concentration of HCl, we would need additional information. If the assumption that the initial concentration of HCl is the same as the concentration of NaOH is not valid, we would need the volume of NaOH used to reach the endpoint in order to calculate the initial concentration of HCl.