The solubility of barium hydroxide at 25 °C is $0.24\ g\,dm^{-3}$ . Given that $M_r[Ba(OH)_2] = 171$ , the molar concentration of the saturated solution, in $mol\,dm^{-3}$ , is

1.4 \times 10^{-2}

7.0 \times 10^{-4}

1.4 \times 10^{-3}

2.8 \times 10^{-3}

Explanation

Concentration = mass/

M_r

0.24/171 = 1.4 \times 10^{-3}\ mol\,dm^{-3}

Derived from ZIMSEC Chemistry Paper 2, June 2011, Q1

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