The solubility of nickel (II) carbonate at 25 degrees celsius is 0.042 g/L.

Calculate Ksp for nickel (II) carbonate.
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To calculate the Ksp (solubility product constant) for nickel (II) carbonate, we need to know the dissociation equation for the compound.

The dissociation equation for nickel (II) carbonate is:

NiCO3(s) ⇌ Ni2+(aq) + CO3^2-(aq)

According to the solubility information given, the concentration of Ni2+ ions in the solution at equilibrium is equal to 0.042 g/L. Since NiCO3 dissociates into one Ni2+ ion and one CO3^2- ion, this concentration can be used as the solubility of Ni2+(aq).

Ksp can be calculated using the equation:

Ksp = [Ni2+][CO3^2-]

However, we need the solubility of CO3^2- to proceed. Since there is no explicit information given about the concentration of CO3^2-, we can assume that the solubility of Ni2+(aq) is equal to the solubility of CO3^2-(aq) because they are both produced in equal amounts during the dissociation.

Thus, the solubility of CO3^2-(aq) is also 0.042 g/L.

Therefore, we can substitute the values into the Ksp expression:

Ksp = (0.042 g/L) * (0.042 g/L) = 0.001764 g^2/L^2

So, Ksp for nickel (II) carbonate at 25 degrees Celsius is 0.001764 g^2/L^2.

Note: Make sure to convert the units appropriately if needed.

To calculate the solubility product constant (Ksp) for nickel (II) carbonate, we need to know the balanced chemical equation for its dissociation in water.

The formula for nickel (II) carbonate is NiCO3. In water, it dissociates into its ions:

NiCO3 (s) ↔ Ni2+ (aq) + CO3^2- (aq)

The balanced chemical equation shows that for every 1 mole of NiCO3 that dissolves, 1 mole of Ni2+ ions and 1 mole of CO3^2- ions are formed.

Now, let's determine the molar solubility of nickel (II) carbonate:

Molar solubility (mol/L) = Mass of solute (g/L) / Molar mass of solute (g/mol)

Given that the solubility of nickel (II) carbonate is 0.042 g/L at 25 degrees Celsius, we can substitute the values into the equation:

Molar solubility (mol/L) = 0.042 g/L / molar mass of NiCO3

To find the molar mass of NiCO3, we need to know the atomic masses of nickel (Ni), carbon (C), and oxygen (O) and sum them up according to their molecular formula.

Atomic mass of Ni = 58.69 g/mol
Atomic mass of C = 12.01 g/mol
Atomic mass of O = 16.00 g/mol

Molar mass of NiCO3 = 58.69 g/mol + 12.01 g/mol + (16.00 g/mol × 3) = 118.69 g/mol

Substituting the value of the molar mass into the equation:

Molar solubility (mol/L) = 0.042 g/L / 118.69 g/mol

Now we can calculate the molar solubility:

Molar solubility (mol/L) = 3.54 × 10^-4 mol/L

Since the coefficients in the balanced equation are 1 for both the nickel ion and carbonate ion, the Ksp expression for nickel (II) carbonate is as follows:

Ksp = [Ni2+][CO3^2-]

Given that the nickel (II) carbonate dissociates completely into its ions, the molar solubility is equal to the concentration of the ions:

[Ni2+] = [CO3^2-] = 3.54 × 10^-4 mol/L

Now we can substitute the concentration into the Ksp expression:

Ksp = (3.54 × 10^-4 mol/L)(3.54 × 10^-4 mol/L)

Calculating this expression, the Ksp value for nickel (II) carbonate at 25 degrees Celsius is:

Ksp = 1.25 × 10^-7

Therefore, the solubility product constant (Ksp) for nickel (II) carbonate is 1.25 × 10^-7.

NiCO3 ==> Ni^+2 + CO3^-2

Ksp = (Ni^+2)(CO3^-2)
Make an ICE chart (using the 0.042 g/L but convert to moles), substitute into Ksp expression and solve for Ksp.