Question

Consider these compounds: A. Ca(OH)2 B. BaSO4 C. Mg(OH)2 D. AgBr

Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that lead bromide is more soluble than___ , and lead bromide is less soluble than__ . It is not possible to determine whether lead bromide is more or less soluble than___ by simply comparing Ksp values.

Answer 1

Without doing any calculations it is possible to determine that

lead bromide is more soluble than (B) BaSO₄ (C)Mg(OH)₂ and (D) AgBr

and lead bromide is less soluble than NA. (not applied)

It is not possible to determine whether lead bromide is more or less soluble than (A) Ca(OH)₂ by simply comparing Ksp values.

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​​​​​since,

Higher the K_sp value of compound, the more soluble the compound is.

from K_sp values of these compounds it is observed that, the solubility constant (K_sp) of PbBr₂ (lead bromide) is higher than that of BaSO₄ , Mg(OH)₂ and AgBr. Hence, PbBr₂ is more soluble than BaSO₄ , Mg(OH)₂ and AgBr.

While K_sp values of PbBr₂ () and Ca(OH)₂() are very close to each other and hence, It is not possible to determine whether PbBr₂ (lead bromide) is more or less soluble than Ca(OH)₂ by simply comparing K_sp values.