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$${ A }_{ 2 }B(s)\rightleftharpoons 2{ A }^{ + }(aq)+{ B }^{ 2– }(aq)$$

A soluble weak electrolyte, ${A}_{2}B$, dissociates in water according to the equation that is shown above. At a particular temperature, the compound is known to be 40.% dissociated.

Suppose you have a solution that has an initial concentration of 0.050 M (0.050 molar) in ${A}_{2}B$.

Which of the following CORRECTLY gives the total number of moles of ions per 1.0 L of solution?

A

0.060

B

0.070

C

0.090

D

0.110

Accuracy 0%
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