Which of the following alkali metal carbonates is/are water soluble?

L i_{2} C O_{3}

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N a_{2} C O_{3}

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K_{2} C O_{3}

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R b_{2} C O_{3}

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Solution

The correct options are
B $K_{2} C O_{3}$
C $N a_{2} C O_{3}$
The polarity of water molecules enables water to dissolve many ionically bonded substances.
Water can dissolve Sodium carbonate and Potassium carbonate because the positive part of water molecules attracts the negative carbonate ions and the negative part of water molecules attracts the positive sodium ions.

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Similar questions

R b_{2} C O_{3}, C s_{2} C O_{3}, L i_{2} C O_{3}, N a_{2} C O_{3}, K_{2} C O_{3}

L i_{2} C O_{3}, R b_{2} C O_{3}, C s_{2} C O_{3}, N a_{2} C O_{3}, K_{2} C O_{3}

H_{2} O ?

(1) B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}

(2) B e (O H)_{2} > M g (O H)_{2} > C a (O H)_{2} > B a (O H)_{2}

(3) L i O H < N a O H < K O H < R b O H

(4) L i_{2} C O_{3} < N a_{2} C O_{3} < K_{2} C O_{3} < R b_{2} C O_{3}

L i_{2} C O_{3}, N a_{2} C O_{3}, K_{2} C O_{3}

H_{2} O

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

B e (O H)_{2} > M g (O H)_{2} > C a (O H)_{2} > B a (O H)_{2}

L i O H < N a O H < K O H < R b O H

L i_{2} C O_{3} < N a_{2} C O_{3} < K_{2} C O_{3} < R b_{2} C O_{3}

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