Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solution of salt in contact with a solution containing a common ion. Show that changes in the initial concentrations: PbCl2(s) in 0.631 M MgCl2 (MgCl2 is strong electrolyte)
Ksp PbCl2 = 1.6 × 10−5

The concentration of all solute species in the solution are:

MgCl₂ (0.631 M) is a strong electrolyte that dissociates according to the following equation.

MgCl₂(aq) ⇒ Mg²⁺(aq) + 2 Cl⁻(aq)

Considering the molar ratios, the initial concentrations of Mg²⁺ and Cl⁻ are:

Cl⁻ is a common ion between MgCl₂ and PbCl₂. To consider the solution equilibrium for PbCl₂ (a sparingly soluble salt), we will make an ICE chart.

        PbCl₂(s) ⇄ Pb²⁺(aq) + 2 Cl⁻(aq)

I                            0               1.26

C                          +x              +2x

E                            x             1.26+x

The solubility product constant, Ksp, is:

Since 1.26 >>> x, 1.26 + x ≈ 1.26.

The concentration of all solute species in the solution are:

You can learn more about solubility product here:

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.