. Calculate the initial concentrations of acetic acid, HC 2 H 3 O 2 , and acetat
ID: 1018233 • Letter: #
Question
. Calculate the initial concentrations of acetic acid, HC2H3O2, and acetate ion, C2H3O2– , in the buffer (see step #2 of the procedure).
Procedure Obtain three clean 250-mL Erlenmeyer flasks. Label one 'Buffer'. Label the second flask '0.100 M HCI. Label the third flask '0.100 M NaOH 2. To prepare 200.0 mL of buffer solution, add 20.0 mL of 1.00 M acetic acid solution to a 100-mL graduated cylinder and add enough distilled water to bring the volume to the 100.0 mL mark. Add to the 'Buffer flask. Add 20.0 mL of 1.00 M sodium acetate solution to the 100-mL graduated cylinder, add enough distilled water to bring the volume to the 100.0 mL mark. Add to the 'Buffer flask. Mix by swirling.Explanation / Answer
CH3COOH
Intial final
M1 = 1M M2
V1 = 20ml V2 = 100ml
M1V1 = M2V2
M2 = M1V1/V2
= 1*20/100 = 0.2M
CH3COOH initial concentration is 1M final concentration is 0.2M
CH3COONa
Intial Final
M1 = 1M M2 =
V1 = 20ml V2 = 100ml
M1V1 = M2V2
M2 = M1V1/V2
= 1*20/100 = 0.2M
intial concentration of CH3COONa is 1M final concentration is 0.2M
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