if 50 mL of .012M barium chloride are mixed with 25 mL of 1.0 x 10^-6M sulfuric acid, will a precipitate form?

Calculate Qsp. Compare with Ksp.

I never learned what Qsp is, what do I do?

Qsp = (Ba^+2)(SO4^-2)
[That's Ksp, also; however, Ksp is at equilibrium and has a constant attached to it while Qsp is just the concentrations multiplied.
Calculate Ba ion and sulfate ion from the BaCl2 mixed with H2SO4. Multily them together to obtain Qsp. Remember that Ksp CAN'T be exceeded. Therefore, if Qsp is > than Ksp, a ppt forms. If Qsp is < Ksp, no ppt forms. Simple, huh?

To calculate Qsp, you need to determine the concentrations of Ba^+2 and SO4^-2 ions in the solution after mixing BaCl2 and H2SO4.

First, calculate the number of moles of BaCl2 in 50 mL of a 0.012M solution:
moles of BaCl2 = volume (L) x concentration (mol/L)
moles of BaCl2 = 50 mL / 1000 mL/L x 0.012 mol/L = 0.0006 mol

Since BaCl2 dissociates into one Ba^+2 ion and two Cl^- ions, we have 0.0006 mol of Ba^+2 ions in the solution.

Next, calculate the number of moles of H2SO4 in 25 mL of a 1.0 x 10^-6 M solution:
moles of H2SO4 = volume (L) x concentration (mol/L)
moles of H2SO4 = 25 mL / 1000 mL/L x 1.0 x 10^-6 mol/L = 2.5 x 10^-8 mol

Since H2SO4 dissociates into two H^+ ions and one SO4^-2 ion, we have 2.5 x 10^-8 mol of SO4^-2 ions in the solution.

Now, calculate Qsp by multiplying the concentrations of Ba^+2 and SO4^-2 ions:
Qsp = (Ba^+2) x (SO4^-2)
Qsp = 0.0006 mol/L x 2.5 x 10^-8 mol/L = 1.5 x 10^-11

To compare Qsp with Ksp, you need to know the value of Ksp for barium sulfate (BaSO4). If Qsp is greater than Ksp, which means the concentrations of the ions exceed the equilibrium constant, a precipitate will form. If Qsp is less than Ksp, no precipitate will form.

If you provide the Ksp value for BaSO4, I can help you determine if a precipitate will form in this specific case.