
(a)
Interpretation: The balanced chemical equation for the reaction of potassium carbonate and magnesium chloride needs to be written. The precipitate formed (if) needs to be indicated.
Concept Introduction:
Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution. Solubility is the property of a solid, liquid or gas.
(a)

Answer to Problem 45A
Salts containing Cl-, Br −or I - are generally soluble.
Salts containing group I elements (Li+, Na+, K+, Cs+, Rb+) are soluble.
Explanation of Solution
Potassium carbonate and magnesium chloride reacts-
Potassium chloride − KCl soluble in water.
(b)
Interpretation: The balanced chemical equation for the reaction of barium chloride and iron (II) nitrate needs to be written. The precipitate formed (if) needs to be indicated.
Concept Introduction:
Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution. The solubility is the property of a solid, liquid or gas.
(b)

Answer to Problem 45A
Salts containing Cl-, Br −or I - are generally soluble.
Explanation of Solution
Barium chloride and iron (II) nitrate reacts-
FeCl2 −soluble
No precipitate is formed
(c)
Interpretation: The balanced chemical equation for the reaction of calcium nitrate and sodium sulfate needs to be written. The precipitate formed (if) needs to be indicated.
Concept Introduction:
Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution. The solubility is the property of a solid, liquid or gas.
(c)

Answer to Problem 45A
Most sulphate salts are soluble. Few exceptions includes CaSO4, BaSO4, PbSO4, Ag2SO4and SrSO4.
Explanation of Solution
Calcium nitrate and sodium sulphate reacts-
CaSO4− Insoluble
(d)
Interpretation: The balanced chemical equation for the reaction of sodium phosphate and copper (II) nitrate needs to be written. The precipitate formed (if) needs to be indicated.
Concept Introduction:
Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution. Solubility is the property of a solid, liquid or gas.
(d)

Answer to Problem 45A
All phosphates are insoluble except those of Na+, K+, NH4+.
Salts containing group I elements(Li+, Na+, K+, Cs+, Rb+) are soluble.
Phosphates such as Ca3(PO4)2 and Ag3PO4 are frequently insoluble.
Salts containing nitrate ion (NO3)- are generally soluble.
Explanation of Solution
Sodium phosphate and copper (II) nitrate reacts-
NaNO3 − soluble
Cu3(PO4)2 − Insoluble
Thus, precipitate is formed and that is Cu3(PO4)2.
(e)
Interpretation: The balanced chemical equation for the reaction of potassium sulfate and lead (II) nitrate needs to be written. The precipitate formed (if) needs to be indicated.
Concept Introduction:
Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution. Solubility is the property of a solid, liquid or gas.
(e)

Answer to Problem 45A
Salts containing nitrate ion (NO3)- are generally soluble.
Most sulfate salts are soluble. Few exceptions include CaSO4, BaSO4, PbSO4, Ag2SO4and SrSO4.Salts containing group I elements(Li+, Na+, K+, Cs+, Rb+) are soluble.
Explanation of Solution
Potassium sulfate and lead (II) nitrate reacts-
PbSO4 − Insoluble
KNO3 − Soluble
Thus, PbSO4 is a precipitate.
(f)
Interpretation: The balanced chemical equation for the reaction of calcium nitrate and lithium sulfide needs to be written. The precipitate formed (if) needs to be indicated.
Concept Introduction:
Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution. Solubility is the property of a solid, liquid or gas.
(f)

Answer to Problem 45A
Salts containing nitrate ion (NO3)- are generally soluble.
Salts containing group I elements(Li+, Na+, K+, Cs+, Rb+) are soluble.
Explanation of Solution
Calcium nitrate and lithium sulfide react as follows:
According to the rule, no precipitate is formed.
Chapter 8 Solutions
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