Which of the following aqueous solutions has a molarity of $0.50 M$ ? (Molar masses in $g/mol$ : $NaOH$ 40, $H X_{2} SO X_{4}$ 98, $Na X_{2} CO X_{3}$ 106, $NaCl$ 58.5.)

A $4 g$ of $NaOH$ in $200 mL$ solution
B $9.8 g$ of $H X_{2} SO X_{4}$ in $400 mL$ solution
C $5.3 g$ of $Na X_{2} CO X_{3}$ in $200 mL$ solution
D $5.85 g$ of $NaCl$ in $200 mL$ solution

Answer: A, D

Molarity = (mass/molar mass)/volume in L: A: 4/40 = 0.1 mol in 0.2 L gives 0.5 M; B: 9.8/98 = 0.1 mol in 0.4 L gives 0.25 M; C: 5.3/106 = 0.05 mol in 0.2 L gives 0.25 M; D: 5.85/58.5 = 0.1 mol in 0.2 L gives 0.5 M. So A and D are 0.50 M.

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Which of the following aqueous solutions has a molarity of 0.50 M? (Molar masses in g/mol: NaOH 40, HX2​SOX4​ 98, NaX2​COX3​ 106, NaCl 58.5.)

Answer: A, D

More questions on Concentration terms (molarity, molality, mole fraction, ppm) and dilution

Which of the following aqueous solutions has a molarity of $0.50 M$ ? (Molar masses in $g/mol$ : $NaOH$ 40, $H X_{2} SO X_{4}$ 98, $Na X_{2} CO X_{3}$ 106, $NaCl$ 58.5.)