The compound you will be investigating in this experiment is the ionic salt barium nitrate, Ba(NO3)2. (a)  Write the balanced equilibrium reaction for the dissolution of barium nitrate in a satu- rated solution and the expression for the solubility product, Ksp. (b)  Write the mathematical relationship between the molar solubility of barium nitrate and the concentrations of the barium ions in the saturated solution [Ba2+]eq and nitrate ions in the saturated solution [NO3–]eq. (c)  Write an equation that relates the molar solubility of barium nitrate and the solubility product Ksp, similar to how Equation 3 in the Background was written for sodium chloride. (d)  Consider dissolving the barium nitrate in nitric acid HNO3, a strong acid (it reacts completely with water to form hydronium and nitrate ions), instead of water. Does the nitric acid influence the barium nitrate’s solubility equilibrium? If so, how, and will this cause more or less barium nitrate to dissolve in

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.