Determine the MAX amount of titrant you will possibly need for your titration.
Your unknown solution has been prepared by dissolving btw 0.05-0.09mol of zwitterion form of the amino acid in 1L of ~ 0.1M HCl solution.
you will titrate 50mL of that amino acid with 0.5M NaOH.
Assume that the amino acid concentration of 0.0900mol per L of 0.1 M HCl
Please help me...I don't uderstand what to do. Explanation will help greatly.
To determine the maximum amount of titrant (in this case, NaOH) needed for the titration, you need to consider the stoichiometry of the reaction between the amino acid and NaOH.
First, let's determine the maximum moles of the amino acid present in the 50 mL of the solution.
Given that the amino acid concentration is 0.0900 mol/L in the 1L solution, we can calculate the moles of amino acid in the 50 mL solution:
(0.0900 mol/L) x (0.050 L) = 0.0045 mol of amino acid
Now, let's determine the stoichiometry of the reaction between the amino acid and NaOH. Since the amino acid is a zwitterion, we can assume it will react with one mole of NaOH per mole of amino acid.
Therefore, the maximum amount of NaOH required for the titration will be:
0.0045 mol NaOH
Now, let's calculate the volume of 0.5 M NaOH needed to provide 0.0045 mol NaOH:
(0.0045 mol NaOH) / (0.5 mol/L) = 0.009 L or 9 mL of 0.5 M NaOH
So, the maximum amount of NaOH you will possibly need for the titration is 9 mL of 0.5 M NaOH.
Note: This calculation assumes complete reaction and disregard any additional factors such as side reactions or pH dependent changes in the amino acid's protonation state.
To determine the maximum amount of titrant you will possibly need for your titration, you need to identify the limiting reactant in the titration reaction.
In this case, you are titrating 50mL of an unknown amino acid solution with 0.5M NaOH. The information given states that the amino acid concentration is between 0.05 and 0.09 mol per L of 0.1M HCl solution.
To find the limiting reactant, you need to compare the number of moles of amino acid present in the titration volume (50mL) with the number of moles of NaOH required to neutralize it.
First, let's calculate the number of moles of amino acid present in 50mL of the solution:
Moles of amino acid = Volume (L) x Concentration (mol/L)
Moles of amino acid = 0.050L x (0.05-0.09 mol/L) = 0.0025 - 0.0045 mol
Since we are given a range for the concentration (0.05-0.09 mol/L), we calculate the minimum and maximum number of moles of amino acid present in 50mL.
Next, we need to determine the stoichiometry of the titration reaction. The balanced equation for the reaction between amino acid and NaOH is:
Amino acid + NaOH → Sodium salt of amino acid + H2O
Assuming a 1:1 stoichiometry, it means one mole of amino acid reacts with one mole of NaOH.
Therefore, the maximum amount of NaOH required to neutralize the amino acid is equal to the maximum number of moles of amino acid present in the 50mL solution (0.0045 mol).
Finally, let's calculate the maximum volume of 0.5M NaOH needed:
Volume (L) = Moles / Concentration
Volume (L) = 0.0045 mol / 0.5 mol/L = 0.009 L or 9 mL
So, the maximum amount of titrant (0.5M NaOH) you will possibly need for your titration is 9 mL.
Remember that this calculation assumes that the concentration is at its maximum value (0.09 mol/L) and the amino acid is fully consumed by the NaOH. In reality, the actual amount of titrant needed may be less.