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The first step in the preparation of magnesium metal is the precipitation of  MgOH2{“version”:”1.1″,”math”:”MgOH2″} from sea water by the addition of CaOH2{“version”:”1.1″,”math”:”CaOH2″}. The concentration of Mg2+(aq){“version”:”1.1″,”math”:”Mg2+(aq)”} in sea water is 5.37 x 10-2 M.{“version”:”1.1″,”math”:”5.37 x 10-2 M.”} Calculate the pH and OH-{“version”:”1.1″,”math”:”OH-“} at which Mg2+ is decreased to 1.0 x 10 -5 M{“version”:”1.1″,”math”:”Mg2+ is decreased to 1.0 x 10 -5 M”}. Ksp MgOH2 = 8.9 x 10-12{“version”:”1.1″,”math”:”Ksp MgOH2 = 8.9 x 10-12″}

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)”}

AgCl(s), {“version”:”1.1″,”math”:”AgCl(s), ”} silver chloride , has a very low solubility : AgCl(s) ⇌Ag+(aq) + Cl- (aq){“version”:”1.1″,”math”:”AgCl(s) ⇌Ag+(aq) + Cl- (aq)”}, Ksp =1.6 x 10-10{“version”:”1.1″,”math”:”Ksp =1.6 x 10-10″} . Adding ammonia significantly increases the solubility of AgCl because———–

How do the concentrations of Ag+{“version”:”1.1″,”math”:”Ag+”} and  CrO42-{“version”:”1.1″,”math”:”CrO42-“} in a saturated solution above 1.0 g of solid Ag2CrO4{“version”:”1.1″,”math”:”Ag2CrO4″}, change when 100 g of solid AgCrO4 {“version”:”1.1″,”math”:”AgCrO4 ”} is added to the system?

What is ∆G°{“version”:”1.1″,”math”:”∆G°”} if ∆H° is +58.7 kJ and ∆S° is +129 J/K{“version”:”1.1″,”math”:”∆H° is +58.7 kJ and ∆S° is +129 J/K”}, at 25°C{“version”:”1.1″,”math”:”25°C”}. Recall: ∆G° = ∆H° – T∆S°{“version”:”1.1″,”math”:”∆G° = ∆H° - T∆S°”}

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  

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)

If the reaction quotient is less than the equilibrium constant, which statement would be correct ?

Use the following schematic for this galvanic cell reaction to determine the oxidizing agent: Zn(s){“version”:”1.1″,”math”:”Zn(s)”}|Zn2+(aq) {“version”:”1.1″,”math”:”Zn2+(aq) ”}|| Sn+4(aq), Sn2+(aq){“version”:”1.1″,”math”:”Sn+4(aq), Sn2+(aq)”}|Pt(s){“version”:”1.1″,”math”:”Pt(s)”}

A patient is admitted to the hospital for a coronary artery bypass surgery.  Postoperatively, he develops a pulmonary embolism.  The present on admission (POA) indicator is