The molarity of an acetic acid solution : 0.321 M
Titration is a procedure for determining the concentration of a solution by reacting with another solution that is known to be concentrated (usually a standard solution). Determination of the endpoint/equivalence point of the reaction can use indicators according to the appropriate pH range
Reaction
HC₂H₃O₂(aq) + NaOH(aq) → H₂O(l) + NaC₂H₃O₂(aq)
Molarity NaOh=0.212
volume NaOH=25 ml=0.025 L
mol NaOH =
[tex]\tt mol=M\times V\\\\mol=0.212\times 0.025\\\\mol=0.0053[/tex]
mol ratio NaOH : HC₂H₃O₂ from the equation = 1 : 1, so mol HC₂H₃O₂ :
[tex]\tt \dfrac{1}{1}\times 0.0053=0.0053[/tex]
The molarity of acetic acid HC₂H₃O₂ :
[tex]\tt molarity(M)=\dfrac{n}{V}\\\\M=\dfrac{0.0053}{0.0165}\\\\M=0.321[/tex]
Or you can use titration formula :
[tex]\tt M_1V_1n_1=M_2V_2n_2(n=acid/base~valence, for NaOH~and~Acetic~acid=1)\\\\0.212\times 25\times 1=M_2\times 16.5\times 1\\\\M_2=\dfrac{0.212\times 25\times 1}{16.5\times 1}\\\\M_2=0.321[/tex]
