A solution contains 0.050 M Br⁻ and 0.050 M CrO₄²⁻. Solid Pb(NO₃)₂ is added slowly. (K_sp) PbBr₂ = (6.6 \times 10^-6) (K_sp) PbCrO₄ = (2.8 \times 10^-13) Which precipitates first? At what [Pb²⁺] does the second begin to precipitate? What is [Br⁻] at that moment?
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Suppose a solution contains 0.1 M AgNO3, 0.1 M NaCl, and 0.1 M NaNO3. If HCl is added to the solution, what will happen? A solution contains 0
The [CO₃²⁻] to begin precipitating BaCO₃ is 2.6 × 10⁻⁷ M . 0.1 M NaCl
Calculate the concentration of the first ion remaining in solution when the second ion begins to precipitate. ⚠️ Why You Should Use Keys Carefully