Chapter 17, Problem 17.45QP

Interpretation Introduction

Interpretation:

By mixing $\text{0}\text{.10 M}{\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{and}\text{0}\text{.10 M}{\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ whether ${\text{BaCO}}_{\text{3}}$ precipitate forms or not has to be explained.

Concept introduction:

• The solubility product constant (${\text{K}}_{\text{sp}}$) is defined as the equilibrium between compound and its ions in an aqueous solution.
• Solubility product is the multiplication of concentration of dissolved ion,  raised to the power of coefficients.
• Ionic compound ${\text{A}}_{\text{3}}\text{B}$ ${\text{K}}_{\text{sp}}\text{=}{\left[\text{A}\right]}^{\text{3}}\left[\text{B}\right]$
• Reaction quotient (Q) is the ratio of product of concentration of products  to that of  product of concentration of reactants, raised to the power of coefficients.
• ${\text{Q}}_{\text{c}}\text{=}\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$
• ${\text{Q > K}}_{\text{sp}}$ , precipitation will happen
• ${\text{Q is less than K}}_{\text{sp}}$, more solute can dissolve in solution.
• ${\text{Q is equal to K}}_{\text{sp}}$, no more solute can dissolve or precipitate in solution.

To prove: ${\text{BaCO}}_{\text{3}}$ precipitate formation