The Ksp value for magnesium carbonate, MgCO3, is 7.2 x 10-6. If 2.50 g of magnesium carbonate is placed in 1.00 x 102 mL of water, how much (in g) magnesium carbonate will dissolve?
Can you please explain the process?
The Ksp value for magnesium carbonate, MgCO3, is 7.2 x 10-6. If 2.50 g of magnesium carbonate is placed in 1.00 x 102 mL of water, how much (in g) magnesium carbonate will dissolve?
The Ksp value for magnesium carbonate, MgCO3, is 7.4 x 10-6. If 2.50 g of magnesium carbonate is placed in 1.00 x 102 mL of water, how much (in g) magnesium carbonate will dissolve?
Sure! To find out how much magnesium carbonate will dissolve in water, we need to compare the solubility product constant (Ksp) with the initial concentration of MgCO3 in the solution.
The Ksp value for magnesium carbonate, MgCO3, is given as 7.2 x 10^-6. This value represents the equilibrium constant for the dissolution of solid MgCO3 into its ions in water.
To begin solving this problem, we need to convert the given quantity of water (1.00 x 10^2 mL) to liters, since the Ksp value is typically expressed in terms of moles per liter.
1 L = 1000 mL, so 1.00 x 10^2 mL = 0.1 L
Next, we need to determine the initial concentration of magnesium carbonate in the solution. This can be calculated using the following formula:
Concentration (in mol/L) = mass of solute (in g) / molar mass of solute (in g/mol) / volume of solvent (in L)
The molar mass of MgCO3 can be calculated as follows:
Mg = 24.31 g/mol
C = 12.01 g/mol
O = 16.00 g/mol
Molar mass of MgCO3 = (1 x 24.31) + (1 x 12.01) + (3 x 16.00) = 84.32 g/mol
Now we can calculate the initial concentration of MgCO3:
Concentration = 2.50 g / 84.32 g/mol / 0.1 L
Concentration ≈ 2.97 x 10^-3 mol/L
Since MgCO3 and Mg2+ have a 1:1 stoichiometry, the concentration of Mg2+ is also 2.97 x 10^-3 mol/L.
Now we can compare the initial concentration of MgCO3 with the Ksp value to determine the amount of MgCO3 that will dissolve.
The equation for the dissolution of MgCO3 can be written as: MgCO3(s) ⇌ Mg2+(aq) + CO3²-(aq)
The solubility product expression is given by:
Ksp = [Mg2+][CO3²-]
Since MgCO3 and Mg2+ have a 1:1 stoichiometry, the concentration of Mg2+ is the same as the concentration of MgCO3, so we can write:
Ksp = (2.97 x 10^-3)² = 8.82 x 10^-6
Comparing the Ksp value (7.2 x 10^-6) with the calculated value (8.82 x 10^-6), we can see that the calculated value is greater than the Ksp value. This means that MgCO3 will exceed its solubility and not all of the compound will dissolve.
Therefore, the maximum amount of MgCO3 that will dissolve can be calculated by subtracting the original concentration from the solubility concentration:
Maximum amount dissolved = solubility concentration - original concentration
= (8.82 x 10^-6) - (2.97 x 10^-3)
≈ 8.82 x 10^-6
To find the mass of the dissolved MgCO3, we can use the following formula:
Mass of dissolved MgCO3 = maximum amount dissolved x molar mass of MgCO3
= (8.82 x 10^-6) x 84.32 g/mol
≈ 0.000742 g or 0.742 mg
Therefore, approximately 0.742 mg of magnesium carbonate will dissolve in 1.00 x 10^2 mL of water.
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Follow this problem.
https://www.jiskha.com/questions/1834091/determine-the-solubility-of-baf2-in-g-l-if-ksp-of-baf2-1-7-10-6
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