what is the equilibrium constant? what is the concentration if the lead cation a

Question

what is the equilibrium constant?

what is the concentration if the lead cation at the equilibrium if the chloride concentration is 2.0X10^-3?

CHEM 183 LAB-Pre-Lab Exercise for Lab #4: Qualitative Analysis Name: TA: This exercise is due at 12:00 when you come to lab next week 1) The solubility product constant, Ksp, for lead (I) chloride has a value of 1.17x10s at 25 °C Write the chemical equation and equilibrium constant expression for the reaction that matches this value. Pb,(S 2) For the reaction you determined above, what is the concentration of the lead cation at equilibrium if the chloride concentration is 2.0x10-3 M? 3) Which of the four cations that you will be searching for in your unknown would form a precipitate in the presence of dissolved chloride ion? 4) Predict the products, if any, that might form upon mixing a solution of barium nitrate with a solution of sulfuric acid. And write (1) the full balanced equation, (2) the full ionic equation, and (3) the net ionic equation. Circle/list the spectator ions.

Explanation / Answer

Q1

PbCl2(s) <-> Pb+2 + 2Cl-

Ksp = [Pb+2][Cl-]^2

Q2-.

find [Pb+2] present in

[Cl-]= 2*10^-3

1.17*10^-5 = [Pb+2] ( 2*10^-3)

[Pb+2] = (1.17*10^-5) / ( 2*10^-3) = 0.00585 M

Q3

Precipitate is likely to be formed by

PB2+ + Cl- = PbCl2(s)

Q4

Ba(NO3)2 + H2SO4 = BaSO4(s) + 2HNO3(aq)

barium sulfat is not soluble

spectator ions --> NO3- and H+

net ionic

Ba2+ + SO4-2 = BaSO4(s)

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.