$100 mL$ of $0.500 M$ acetic acid is shaken with $2.5 g$ of charcoal. At equilibrium the concentration is $0.436 M$ . Taking the molar mass of acetic acid as $60 g mo l^{- 1}$ , find the mass of acid adsorbed per gram of charcoal in $mg g^{- 1}$ (nearest integer).

Numerical answer type, answer in mg/g, tolerance 1.

Answer: 153.6 mg/g

Amount removed

= (0.500 - 0.436) \times 100 = 6.4 mmol

. Per gram:

6.4/2.5 = 2.56 mmol g^{- 1}

. Mass

= 2.56 \times 60 = 153.6 \approx 154 mg g^{- 1}