which combination will produce a precipitate

Which combination will produce a precipitate plus#

Is turning into the ions at the same rate, the ions are Solution, it would dissolve, and it would continue to dissolve So lead two sulfate as a white solid, so if we were to put a smallĪmount of lead two sulfate in our unsaturated

For an unsaturated solution, you can dissolve more The solution is unsaturated, which means no precipitate would form. However, these aren't perfect diagrams they're just to help get the point across. KSP and what that means for the solution. To help us understand how QSP compares to QSP at the moment, our two solutions are mixed, and then we're going Gonna calculate QSP, which has the same form as KSP, the differences the concentrations can be at any moment in time.

Which combination will produce a precipitate plus#

Plus and sulfate in the KSP expression, areĮquilibrium concentrations. Is equal to 6.3 times 10 to the negative sevenĪt 25 degrees Celsius. Pure solids are left out of equilibrium, constant expressions. Of sulfate also raised to the first power and Would be the concentration of lead two plus raised to the first power because we have a coefficient of one in the balanced equation, times the concentration To write out the dissolution equation is because weĬan write a KSP expression from it. We would form lead two plus cations in aqueous solution,Īnd sulfates anions in aqueous solutions, right? aq over here. Is identify the precipitate and then write out theĭisillusion equation. Running the overall equation,Īnd the net ionic equation are really optional forĪ problem like this. Sodium cations or nitrate anions because thoseĪre the spectator ions in our overall reaction. Our possible precipitate, we really only care about theĬoncentration of lead two plus ions and sulfate anions in solution. So lead two plus ions, wouldĬome together with sulfate anions to form PBSO4.

Now that we know are possible precipitate, let's go ahead and writeĪ net ionic equation showing the formation of that precipitate. Sodium nitrate is an aqueous solution and lead sulfate wouldīe our possible precipitate. Other cation and the other anion and so the other product PbSO4, after we cross over our charges and we take the So we take the cation from oneĪnd the anion from the other. In the sodium sulfate aqueous solution, there are sodium cationsĪnd sulfate anions. Solution they're lead two plus cations and nitrate anions. Solution of lead two nitrate with an aqueous solution The first step is toįigure out the identity of the precipitate that might form. Times 10 to the negative third Molar solution of sodium sulfate. Our goal is to figure out whether or not a precipitate will form if we mix 0.20 liters overĤ.0 times 10 to the negative third Molar solution of lead two nitrate, with 0.80 liters of an 8.0