Write the dissolution equation for the slightly soluble salt Mg3PO42{“version”:”1.1″,”math”:”Mg3PO42″} and the solubility product constant, Ksp{“version”:”1.1″,”math”:”Ksp”}                            

Calculate the standard entropy for the following process: H2(g) +C2H4(g) →C2H6(g){“version”:”1.1″,”math”:”H2(g) +C2H4(g) →C2H6(g)”} Standard entropies for the substance are: Substance                                 S°(Jmol-1K-1){“version”:”1.1″,”math”:”S°(Jmol-1K-1)”} H2(g){“version”:”1.1″,”math”:”H2(g)”}                                             130.57 C2H4(g){“version”:”1.1″,”math”:”C2H4(g)”}                                         219.5 C2H6(g){“version”:”1.1″,”math”:”C2H6(g)”}                                         229.5  

What is the effect on the amount of solid Mg(OH)2{“version”:”1.1″,”math”:”Mg(OH)2″} and the concentrations of Mg2+ and OH-{“version”:”1.1″,”math”:”Mg2+ and OH-“}when MgCl2{“version”:”1.1″,”math”:”Cl2″} is added to a saturated solution of Mg(OH)2 {“version”:”1.1″,”math”:”Mg(OH)2 ”}?

Use the ionic equation for the dissolution of the slightly soluble salt Sr3PO42{“version”:”1.1″,”math”:”Sr3PO42″}to write the solubility product Ksp{“version”:”1.1″,”math”:”Ksp”} Sr3PO42(s) ⇌3Sr2+(aq) +2PO43-(aq){“version”:”1.1″,”math”:”Sr3PO42(s) ⇌3Sr2+(aq) +2PO43-(aq)”}

Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of Hg2I2 if Ksp = 4.5 x 10 -29{“version”:”1.1″,”math”:”Hg2I2 if Ksp = 4.5 x 10 -29″}

Predict whether CaHPO4{“version”:”1.1″,”math”:”PO4″} will precipitate from a solution with Ca2+ =0.0001 M{“version”:”1.1″,”math”:”Ca2+ =0.0001 M”} and HPO42-=0.001 M{“version”:”1.1″,”math”:”HPO42-=0.001 M”}  Ksp = 7 x 10-7 {“version”:”1.1″,”math”:”Ksp = 7 x 10-7 ”}

Calculate the solubility product constant of  0.026 g/100 mL solution of BaSiF6{“version”:”1.1″,”math”:”BaSiF6″},  contains SiF62-{“version”:”1.1″,”math”:”SiF62-“} ions)

 Use the Henderson-Hasselbalch equation to predict the perceived color of the methyl orange solution where pH >pKa{“version”:”1.1″,”math”:”>pKa”}. Note: HIn color is red and In-{“version”:”1.1″,”math”:”In-“} color is yellow. pH = pKa+logIn-HIn{“version”:”1.1″,”math”:”Ka+logIn-HIn”}

In the balanced redox equation for the formation of rust on iron metal, identify the correct oxidizing and reducing agents.  4Fe(s) + 3O2(g) → 2Fe2O3(s){“version”:”1.1″,”math”:”4Fe(s) + 3O2(g) → 2Fe2O3(s)”}

Write the solubility product, Ksp{“version”:”1.1″,”math”:”Ksp”} expression for the slightly soluble ionic compound: Ag2S(s){“version”:”1.1″,”math”:”Ag2S(s)”}