The Henry's law constant of CH₃Br in water at 25 °C is 0.159 mol L⁻¹ bar⁻¹. The solubility of CH₃Br at 25 °C and a partial pressure of 130 mm Hg is approximately:
A2.7 M
B0.27 M
C0.027 M
D20.7 M
Answer & Solution
Correct answer: B. 0.27 M
Convert: $P = 130/760$ atm $= 0.171$ atm $\times 1.013$ bar/atm $= 0.173$ bar. $S = K_H P = 0.159 \times 0.173 \approx 0.275$ M $\approx 0.27$ M.
Related questions
The mass of NaOH (M = 40 g/mol) required to prepare 500 mL of a 0.20 M NaOH solution isWhich of these solutions will boil at the highest temperature at 1 atm?The molality of a 1 M aqueous NaCl solution (density = 1.04 g/mL, NaCl M = 58.5 g/mol) is Osmotic pressure π of a dilute solution obeys π = C R T. Here C representsVan't Hoff factor i > 1 for a solute indicatesA negative deviation from Raoult law is expected whenIf a solute dimerises in solution, its observed molar mass compared with the calculated vaWhich of the following is NOT a colligative property?