What volume of titrant would be required to reach the equivalence point in the titration of 25.0 mL and 0.825M CH3NH2 with 1.00 M HCL?
mL x M = mL x M since this is a 1:1 molar titration.
To calculate the volume of titrant required to reach the equivalence point, you need to determine the stoichiometry of the reaction and use it to calculate the amount of titrant required.
The balanced chemical equation for the reaction is as follows:
CH3NH2 + HCl -> CH3NH3+ + Cl-
From the equation, you can see that the reaction ratio between CH3NH2 and HCl is 1:1. This means that 1 mole of CH3NH2 reacts with 1 mole of HCl.
To determine the amount of CH3NH2 in moles,
moles CH3NH2 = volume (in L) x concentration (in mol/L)
moles CH3NH2 = 0.025 L x 0.825 mol/L
moles CH3NH2 = 0.020625 mol
Since the stoichiometry of the reaction is 1:1, you will need 0.020625 moles of HCl to reach the equivalence point.
Now, to calculate the volume of HCl required,
volume HCl = moles HCl / concentration HCl
volume HCl = 0.020625 mol / 1.00 mol/L
volume HCl = 0.020625 L or 20.625 mL
Thus, approximately 20.625 mL of 1.00 M HCl would be required to reach the equivalence point in the titration.
To determine the volume of the titrant (in this case, 1.00 M HCl) required to reach the equivalence point in the titration, we need to use the concept of stoichiometry.
First, let's write a balanced chemical equation for the reaction between CH3NH2 and HCl:
CH3NH2 + HCl → CH3NH3+ + Cl-
From the balanced equation, we can see that the stoichiometry of the reaction is 1:1. This means that for every one mole of CH3NH2, we need one mole of HCl to react completely.
Next, we calculate the number of moles of CH3NH2 in 25.0 mL of 0.825 M CH3NH2 solution:
Moles of CH3NH2 = Volume (in liters) × Concentration
= 25.0 mL × (1 L / 1000 mL) × 0.825 M
= 0.020625 moles
Since the stoichiometry of the reaction is 1:1, we know that we need 0.020625 moles of HCl to react completely with the CH3NH2.
Finally, we use the concentration of HCl (1.00 M) to calculate the volume of HCl solution needed to reach the equivalence point. The equation we use is:
Volume (in liters) = Moles / Concentration
= 0.020625 moles / 1.00 M
= 0.020625 L
To convert the volume to milliliters (mL), we multiply by 1000:
Volume (in mL) = 0.020625 L × 1000
= 20.625 mL
Therefore, the volume of 1.00 M HCl required to reach the equivalence point in the titration is 20.625 mL.