On the basis of the general solubility rules given in the table, predict which of the following substances are likely to be soluble in water. Simple Rules for the Solubility of Salts in Water

On the basis of the general solubility rules given in 7.1 write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. Underline the formula of the precipitate (solid) that forms. If no precipitation reaction is likely for the reactants given, explain why. ammonium chloride, ‍, and sulfuric acid, ‍ potassium carbonate, ‍, and tin(IV) chloride,  ammonium chloride, ‍, and lead(II) nitrate, ‍ copper(II) sulfate, , and potassium hydroxide,  sodium phosphate, ‍, and chromium(III) chloride,  ammonium sulfide, ‍, and iron(III) chloride,

When you reacted the 'black solid' with hydrochloric acid a metal chloride salt was formed and water. Based on the experiment performed, suggest a way of obtaining the solid metal chloride salt from this solution. What color do you think the solid metal chloride salt will be? And why?

Enter the net ionic equation, including phases, for the reaction of AgNO, (aq) and KCI(aq). Refer to the solubility rules as needed. net ionic equation:

A student adds silver nitrate solution to hydrochloric acid solution and obtains a white precipitate. The student then adds a clear, colorless solution of an unknown metal ion to a solution of hydrochloric acid, and the result is clear and colorless. What can the student conclude about the unknown?

Solubility Rules for Some Ionic Compounds in Water Soluble Ionic Compounds 1. All sodium (Na*), potassium (K*), and ammonium (NH,) salts are SOLUBLE. 2. All nitrate (NO;), acetate (CH;CO,), chlorate (CIO3), and perchlorate (Cl0,) salts are SOLUBLE. All chloride (CI"), bromide (Br"), and iodide (I') salts are SOLUBLE – EXCEPT those containing: lead, silver, or mercury (I) (Pb2+, 3. Ag*, Hg,2") which are NOT soluble. All sulfate (SO,2) salts are SOLUBLE – EXCEPT those containing: calcium, silver, mercury (I), strontium, barium, or lead (Ca2", 4. Ag", Hg,2", Sr*, Ba2“, Pb²*) which are NOT soluble. Not Soluble Ionic Compounds Hydroxide (OH") and oxide (02) compounds are NOT SOLUBLE- - EXCEPT those containing: sodium, potassium, or barium 5. (Na", K*, Ba2") which are soluble. Sulfide (S2) salts are NOT SOLUBLE – EXCEPT those containing: sodium, potassium, ammonium, or barium (Na", K*, NH,", 6. Ba2") which are soluble. Carbonate (CO,2) and phosphate (PO,') salts are NOT SOLUBLE – EXCEPT…

ences to access important values if needed for this question. Does a reaction occur when aqueous solutions of copper(II) bromide and zinc acetate are combined? Oyes Ono If a reaction does occur, write the net ionic equation. Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank.