Question

1. are the following ionic compounds soluble or insoluble in water? based on their solubility, are the following compounds strong electrolytes? a. licl b. agbr c. pb(no₃)₂ d. baso₄ e. ca(oh)₂ f. alpo₄

Explanation:

Step1: Recall solubility rules

Salts of alkali - metal ions (like Li⁺) are soluble. LiCl is a salt of lithium (an alkali - metal). So LiCl is soluble in water and a strong electrolyte as it dissociates completely in water.

Step2: Consider silver halides

Silver bromide (AgBr) is an insoluble salt according to solubility rules. Insoluble salts are weak electrolytes as they have very low dissociation in water.

Step3: Analyze lead(II) chromate

Lead(II) chromate ($PbCrO_{4}$) is insoluble in water. It is a weak electrolyte due to its low solubility and limited dissociation.

Step4: Recall sulfate solubility

Barium sulfate ($BaSO_{4}$) is insoluble in water. It is a weak electrolyte because of its low solubility and minimal dissociation.

Step5: Consider calcium hydroxide

Calcium hydroxide ($Ca(OH)_{2}$) is slightly soluble in water. But the dissolved part dissociates completely, so it is a strong electrolyte.

Step6: Analyze aluminum phosphate

Aluminum phosphate ($AlPO_{4}$) is insoluble in water. It is a weak electrolyte as it has low solubility and little dissociation.

Answer:

a. Soluble, strong electrolyte
b. Insoluble, weak electrolyte
c. Insoluble, weak electrolyte
d. Insoluble, weak electrolyte
e. Slightly soluble, strong electrolyte
f. Insoluble, weak electrolyte