Which of the following compounds is more soluble in acidic solution than in pure neutral water?

a. baco3
b. cui
c. pbcl2
d. agbr
e. nh4no3

The compound A (BaCO₃) is the most soluble in acidic solution.

Explanation:

We analyze the dissociation of the compounds:

A) BaCO₃ ⇒ Ba⁺² + CO₃⁻²

CO₃⁻² is the conjugated base of HCO₃ acid, which is a weak acid, therefore its conjugate base is strong.

B) CuI ⇒ Cu⁺ + I⁻

I⁻ is the conjugated base of HI acid, which is a strong acid, therefore its conjugate base is weak.

C) PbCl₂ ⇒ Pb⁺² + 2 Cl⁻

Cl⁻ is the conjugated base of HCl acid, which is a strong acid, therefore its conjugate base is weak.

D) AgBr ⇒ Ag⁺ + Br⁻

Br⁻ is the conjugated base of HBr acid, which is a strong acid, therefore its conjugate base is weak.

E) NH₄NO₃ ⇒ NH₄⁺ + NO₃⁻

NO₃⁻ is the conjugated base of HNO₃ acid, which is a strong acid, therefore its conjugate base is weak.

As the medium is acidic, there is a high concentration of H₃O⁺ and the CO₃⁻² is a strong base, the concentration of CO₃⁻² decreases to form H₂CO₃ and by the Le Chatelier's principle the equilibrium of the dissociation reaction shifts to the right and increases the solubility of the salt.

i need mutiple choices

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.