This graph shows the titration of 25.0 mL of methylamine solution with a 0.0798 M HCl. Determine the molarity of the methylamine solution.
Clearly from the graph it is evident that equivalence happens at Volume of HCl = 21 mL (Steepest Part of Curve)
So, we have the formula,
M1V1 = M2V2
=>M1 * 25.0 = 0.0798 * 21
=> M1 = 0.0670 M
So, molarity of methyl amine is 0.0670 M
Answer:
IF:
CH3NH2 + HCl ------> CH3NH4+Cl-
1moL CH3NH2 + 1moL HCl ------> 1moL CH3NH4+Cl-
1moL x 31 g/moL CH3NH2 + 1moL x 36.45 g/moL HCl ------> 1moL x 67.45 g/moL CH3NH4+Cl-
31 g CH3NH2 + 36.45 g HCl ------> 67.45 g CH3NH4+Cl-
AND IF:
for HClsln:
VHCl= 17 mL = 0.017 L
[M]= 0.0798 M = 0.0798 moL/L
Fw= 36.45 g/moL
MassHCl=0.0798 moL/L x 36.45 g/moL x 0.017 L = 0.04945 g pure HCl
for CH3NH2sln:
VCH3NH2= 25 mL = 0.025 L
[M]= X M = X moL/L
Fw= 31 g/moL
THEN:
0.04945 g pure HCl x (31 g pure CH3NH2 / 36.45 g pure HCl) = 0.04205 g CH3NH2
[M]= MassCH3NH2 / (Vsln x FwCH3NH2)
[M]= 0.04205 g / (0.025 L x 31 g/moL)
[M]= 0.05426 M
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