Which of the following represents a correct water solubility order?

B e C l_{2} < M g C l_{2} < C a C l_{2} < S r C l_{2} < B a C l_{2}

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B e S O_{4} < M g S O_{4} < C a S O_{4} < S r S O_{4} < B a S O_{4}

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B e C l_{2} > M g C l_{2} > C a C l_{2} > S r C l_{2} > B a C l_{2}

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B e S O_{4} > M g S O_{4} > C a S O_{4} > S r S O_{4} > B a S O_{4}

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Solution

The correct options are
C $B e C l_{2} > M g C l_{2} > C a C l_{2} > S r C l_{2} > B a C l_{2}$
D $B e S O_{4} > M g S O_{4} > C a S O_{4} > S r S O_{4} > B a S O_{4}$
As the atomic number of the alkaline earth metal increases, the solubility of alkaline earth halides decreases. Thus, the correct order of the solubilities of alkaline earth chlorides is $B e C l_{2} > M g C l_{2} > C a C l_{2} > S r C l_{2} > B a C l_{2}$ .
This is also true with alkaline earth metal sulphates.
The correct order is $B e S O_{4} > M g S O_{4} > C a S O_{4} > S r S O_{4} > B a S O_{4}$ .
As the size of the metal increases, the hydration energy decreases.
Hence, the solubility decreases.

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Similar questions

R a C l_{2} < B a C l_{2} < S r C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}

B e C l_{2} < M g C l_{2} < C a C l_{2} < S r C l_{2} < B a C l_{2} < R a C l_{2}

R a C l_{2} < B a C l_{2} < S r C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}

R a C l_{2} < B a C l_{2} < S r C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}

B e S O_{4}, M g S O_{4}, C a S O_{4}, S r S O_{4}, B a S O_{4}

Why are $B e S O_{4} a n d M g S O_{4}$ readily solubel in water whle $C a S O_{4}, S r S O_{4}$ are insoluble?

B e C l_{2}, M g C l_{2}, C a C l_{2}, S r C l_{2}

B a C l_{2}

B e S O_{4}, M g S O_{4}, C a S O_{4}, S r S O_{4}

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