The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein 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 don't have enough information posted to work the problem; I assume the picture to which you refer gives the volume of NaOH.
mols NaOH = M x L = ?
mols HCl = mols NaOH
M HCl = mols HCl/L HCl.
Vol NaoH titration Ml Naoh (1L/1000 mL) (.270 M (NAOH)= mol NaOH
Then mol of NaOH mol HCL/.010L
To find the volume of NaOH needed to reach the end point of the titration, we need to determine the stoichiometric ratio between HCl and NaOH.
The balanced chemical equation for the reaction between HCl and NaOH is:
HCl + NaOH -> NaCl + H2O
From the equation, we can see that the stoichiometric ratio between HCl and NaOH is 1:1. This means that for every 1 mole of HCl, we need 1 mole of NaOH.
Given that the concentration of NaOH is 0.270 M and the volume of HCl in the flask is 10.0 mL, we can calculate the moles of HCl using the following equation:
moles of HCl = concentration (in M) * volume (in L)
First, convert the volume of HCl from mL to L:
volume of HCl = 10.0 mL = 10.0 mL / 1000 = 0.010 L
Now, we can calculate the moles of HCl:
moles of HCl = 0.270 M * 0.010 L = 0.0027 moles
Since the stoichiometric ratio between HCl and NaOH is 1:1, we know that we need the same number of moles of NaOH as HCl.
So, the volume of NaOH needed to reach the end point of the titration can be calculated as follows:
volume of NaOH = moles of NaOH / concentration of NaOH
volume of NaOH = 0.0027 moles / 0.270 M = 0.01 L = 10.0 mL
Therefore, 10.0 mL of NaOH is needed to reach the end point of the titration.
Regarding the initial concentration of HCl, it is not mentioned in the provided information. To determine the initial concentration of HCl, we need to know either the concentration of NaOH before titration or the volume of NaOH required to reach the end point, along with the concentration of NaOH. Without this information, we cannot calculate the initial concentration of HCl.