When will a precipitate form? a. when the concentration of the cation is greater than the concentration of the anion. b. when the concentration of the anion is greater than the concentration of the cation. c. when the reaction quotient is greater than the solubility-product constant. d. when the solubility-product constant is greater than the reaction quotient. e. none of these.

c. when the raction quotient is greater than the Ksp

Explanation:

∴ Ksp = [ A+ ]∧x  *  [ B- ]∧ysolubility product constant

∴ I.P = xA+ * yB-ionic product

⇒ the relationship between Ksp and I.P, will give us the precipitation conditions.

∴ I.P > Ksp ⇒ precipitation

∴ I.P < Ksp ⇒ no precipitation (disolution)

∴ I.P = Ksp ⇒ equilibrium

⇒ the ionic product is directly related to the reaction quotient Q, where Q = [A+] * [B-] / [AxBy] = PI / [AB], then the higher this product the higher the reaction quotient will be and therefore will be greater than the value of the constant and will have precipitated, the correct answer is the c

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: