On the basis of the general solubility rules, choose a balanced molecular equation for the precipitation reactions that

[answerhappygod]

On The Basis Of The General Solubility Rules Choose A Balanced Molecular Equation For The Precipitation Reactions That 1 (53.2 KiB) Viewed 9 times

On The Basis Of The General Solubility Rules Choose A Balanced Molecular Equation For The Precipitation Reactions That 2 (75.43 KiB) Viewed 9 times

On the basis of the general solubility rules, choose a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO) salts are soluble. 2. Most salts of Na, K, and NEL are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble. The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH), are only moderately soluble. 6. Most sulfide (8²), carbonate (CO₂), and phosphate (PO) salts are only slightly soluble." *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. a. Iron(III) chloride, FeCls, and sulfuric acid, H₂SO4 O Rule 4: an exception to the rule for sulfates; 2FeCl, (aq) + 3H₂SO4 (aq) → Fe₂(SO4)3(aq) + 6HCl(aq) O Rule 4: an exception to the rule for sulfates; 2FeCls (aq) + 3H₂SO4 (aq) → Fe₂(SO4)3 (8) + 6HCl(aq) There is no precipitate: both Fe2(SO4)3 and HCl are soluble; FeCl, (aq) + H₂SO4 (aq) → no precipitate Rule 4: an exception to the rule for sulfates; FeCls (aq) + H₂SO, (ag) → Fes (SO.)s(s) + HCl(aq) - b. Potassium carbonate, K₂CO3, and calcium chloride, CaCl₂ Rule 6: Most carbonate salts are only slightly soluble: K₂CO, (aq) +CaCl₂ (aq) → CaCO, (a) + KCl(aq) Rule 6: exeption to rule for carbonates; 2K.CO (ao) +CaCl(aq) → CaCOx(s) +2KCl(aq) <Previous Next
[References] b. Potassium carbonate, K₂CO3, and calcium chloride, CaCl₂ Rule 6: Most carbonate salts are only slightly soluble; K₂CO3(aq) + CaCl₂ (aq) → CaCO3(s) + KCl(aq) O Rule 6: exeption to rule for carbonates; 2K₂CO3(aq) +CaCl₂ (aq) → CaCO3(s) +2KCl(aq) O Rule 6: Most carbonate salts are only slightly soluble; K₂CO3(aq) +CaCl₂ (aq) → CaCO, (aq) + 2KCl(aq) Rule 6: Most carbonate salts are only slightly soluble; K₂CO3(aq) +CaCl₂ (aq) → CaCO3(s) + 2KCl(aq) - c. Ammonium chloride, NH, Cl, and lead(11) nitrate, Pb(NO3)2 O Rule 3: an exception to the rule for chlorides; NH, Cl(aq) + Pb(NO3)2 (aq) → PbCl₂ (aq) + NH4NO₂ (aq) Rule 3: an exception to the rule for chlorides; NH, Cl(aq) + Pb(NO3)2 (aq) → PbCl2 (s) + NH4NO3(aq) Rule 3: an exception to the rule for chlorides; 2NH4Cl(aq) + Pb(NO3)2 (aq) → PbCl₂ (s) + 2NH, NO, (aq) Rule 3: an exception to the rule for chlorides; 2NH₂Cl(aq) + Pb(NO3)2 (aq) → PbCl₂ (aq) + 2NH4NO₂ (aq) d. Nickel(II) sulfate, NiSO4, and potassium hydroxide, KOH Rule 5: an exception to the rule for hydroxides; NISO, (aq) + 2KOH(aq) → Ni(OH)2 (8) + K₂SO4 (aq) Rule 5: an exception to the rule for hydroxides; NISO4 (aq) + 2KOH(aq) → Ni(OH)2 (aq) + K₂SO4 (aq) → Rule 5: an exception to the rule for hydroxides; NiSO4 (aq) + KOH(aq) Ni(OH)2 (8) + K₂SO4 (aq) Rule 5: an exception to the rule for hydroxides; NiSO4 (aq) + 3KOH(aq) → Ni(OH)2 (s) + K₂SO4 (aq)