A solution contains I-, Br- and OH- ions. If Ag+ is added, what will the precipitate(s) be?
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
To determine the precipitates that will form when Ag+ is added to a solution containing I-, Br-, and OH- ions, we need to consider the solubility rules for common salts.
1. Start by writing down the formula for the possible precipitates by combining the cation (Ag+) with each of the anions (I-, Br-, and OH-).
- AgI (silver iodide)
- AgBr (silver bromide)
- AgOH (silver hydroxide)
2. Next, consult the solubility rules to determine the solubility of each compound. Here are the relevant rules:
- Most iodides (I-) are insoluble, except when paired with alkali metal cations (e.g., Na+, K+).
- Most bromides (Br-) are insoluble, except when paired with alkali metal cations (e.g., Na+, K+).
- Most hydroxides (OH-) are insoluble, except when paired with alkali metal cations (e.g., Na+, K+).
Based on these rules, we can conclude the following:
- AgI is insoluble and will form a precipitate.
- AgBr is insoluble and will form a precipitate.
- AgOH is insoluble and will form a precipitate.
Therefore, when Ag+ is added to the solution containing I-, Br-, and OH- ions, the precipitates formed will be AgI, AgBr, and AgOH.