Hard water often contains dissolved Ca^2+ and Mg^2+ ions. One way to soften water is to add phos

step 1 To answer this question, we have to first direct two balanced chemical reaction of the calcium -

Hard water often contains dissolved Ca^2+ and Mg^2+ ions....

Hard water often contains dissolved $\mathrm{Ca}^{2+}$ and $\mathrm{Mg}^{2+}$ ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. A solution is 0.050 $\mathrm{Mn}$ calcium chloride and 0.085 $\mathrm{M}$ in magnesium nitrate. What mass of sodium phosphate would you add to 1.5 $\mathrm{Lof}$ this solution to completely eliminate the hard water ions? Assume complete reaction.

Key Concepts

Molarity and Mole Calculations

Molarity represents the concentration of a solution in terms of moles per liter. To determine the amount of a substance in a solution, the molarity is multiplied by the volume (in liters) of the solution. This concept is essential for calculating how many moles of ions are present before they react.

Stoichiometry in Precipitation Reactions

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In precipitation reactions, the balanced chemical equation indicates the mole ratios in which the reactants combine. This concept is fundamental when determining the amount of a reagent needed to react completely with the ions in solution.

Precipitation Reactions and Solubility

Precipitation reactions occur when two soluble salts react to form an insoluble compound, known as a precipitate. In water treatment, the formation of a precipitate removes specific ions from solution. Understanding solubility rules helps predict which combinations of ions will form precipitates, allowing the design of methods to remove unwanted components from water.

Molar Mass and Mass Conversion

Molar mass is the mass of one mole of a substance and is used to convert between moles and grams. Once the number of moles required for the reaction is determined via stoichiometric calculations, the molar mass is used to find out the mass of the reagent needed. This conversion is crucial for preparing the correct amount of a solid compound for a reaction.

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