Answer:
NET equation: 2Br^- (aq) + Cr2+ (aq) → CrBr2 (aq)
The solubility signs for each compound are:
Barium bromide (BaBr2): (aq) - aqueous (soluble)
Chromium (II) sulfate (CrSO4): (aq) - aqueous (slightly soluble)
Barium sulfate (BaSO4): (s) - solid (insoluble)
Chromium (II) bromide (CrBr2): (aq) - aqueous (soluble)
Step-by-step explanation:
Barium bromide and chromium (II) sulfate are both ionic compounds that can dissociate into their constituent ions in aqueous solutions. To write the net ionic equation for the reaction between barium bromide and chromium (II) sulfate, we first need to determine the state of the reactants and products (whether they are soluble or insoluble in water) using solubility rules.
Barium bromide (BaBr2) is soluble in water, while chromium (II) sulfate (CrSO4) is slightly soluble. When the two are mixed in water, a double displacement reaction takes place, producing barium sulfate (BaSO4) and chromium (II) bromide (CrBr2) as the products:
BaBr2 (aq) + CrSO4 (aq) → BaSO4 (s) + CrBr2 (aq)
To write the net ionic equation, we need to eliminate any spectator ions that do not participate in the reaction. In this case, the barium and sulfate ions are spectator ions, as they appear unchanged on both sides of the equation. The net ionic equation is therefore:
2Br^- (aq) + Cr2+ (aq) → CrBr2 (aq)
where Br^- and Cr2+ are the ions that actually participate in the reaction.
The solubility signs for each compound are:
Barium bromide (BaBr2): (aq) - aqueous (soluble)
Chromium (II) sulfate (CrSO4): (aq) - aqueous (slightly soluble)
Barium sulfate (BaSO4): (s) - solid (insoluble)
Chromium (II) bromide (CrBr2): (aq) - aqueous (soluble)