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∙ 12y agoThe molar solubility of silver oxalate can be calculated using the given Ksp value. First, calculate the solubility product (Ksp) by taking the square root of the given value, which is √(5.4x10^12) ≈ 2.3x10^6. This means the molar solubility of silver oxalate is approximately 2.3x10^-6 mol/L.
To calculate the molar solubility of lead thiocyanate in 0.500 L of water, you need to know the Ksp value for lead thiocyanate. Can you provide that information?
The molar solubility of PbBr2 in water is approximately 1.6 x 10^-3 mol/L at 25°C. This means that at this temperature, 1.6 x 10^-3 moles of PbBr2 will dissolve in one liter of water.
That's correct. The molar solubility of Na3PO4, NaF, KNO3, AlCl3, and MnS is not affected by the pH of the solution because these compounds do not contain any acidic or basic groups that can significantly influence their solubility as pH changes. The solubility of these compounds is primarily determined by their intrinsic properties and the interactions between the ions in the compound.
Helium is an inert gas which does not readily dissolve in water, so it does not have a well-defined molar solubility in water at 1.0 ATM pressure.
From the definition of Ksp, the product of the concentrations of Ag+ and Cl- can be no more than (1.8 X 10-10)/0.35 = 5.1 X 10-10. Since the only named material that is a source of silver ions is AgCl and the concentrations are molar, this is the maximum possible solubility of AgCl.
The molar solubility of PbBr2 in water is approximately 1.6 x 10^-3 mol/L at 25°C. This means that at this temperature, 1.6 x 10^-3 moles of PbBr2 will dissolve in one liter of water.
The molar mass of sodium oxalate (Na2C2O4) is approximately 134.00 grams/mole.
The molecular formula of ammonium oxalate is (NH4)2C2O4. The molecular mass of ammonium oxalate is 124.10 g/mol.
To calculate the molar solubility of lead thiocyanate in 0.500 L of water, you need to know the Ksp value for lead thiocyanate. Can you provide that information?
The molar solubility of Iron (II) phosphate (Fe3(PO4)2) is about 1.4 x 10^-22 mol/L at 25°C. It is a sparingly soluble salt with a low solubility product constant.
The solubility product constant (Ksp) for BaSO3 can be calculated using the molar solubility provided. In this case, Ksp = (molar solubility)^2 = (80 x 10^-6)^2 = 6.4 x 10^-9.
The molar mass of silver sulfite (Ag2SO3) is calculated by adding the atomic masses of silver (Ag), sulfur (S), and oxygen (O) atoms in the compound. The molar mass of silver sulfite is approximately 311.8 g/mol.
To calculate the molar solubility of copper(II) sulfide, you need to consider the solubility product constant (Ksp) of CuS. Once you have the Ksp value, set up an equilibrium expression for the dissociation of CuS into Cu^2+ and S^2- ions. Use the initial concentration of CuCl2 to determine the concentration of Cu^2+ ions and then solve for the molar solubility of CuS.
That's correct. The molar solubility of Na3PO4, NaF, KNO3, AlCl3, and MnS is not affected by the pH of the solution because these compounds do not contain any acidic or basic groups that can significantly influence their solubility as pH changes. The solubility of these compounds is primarily determined by their intrinsic properties and the interactions between the ions in the compound.
The molar mass of silver (Ag) is approximately 107.87 grams per mole.
Helium is an inert gas which does not readily dissolve in water, so it does not have a well-defined molar solubility in water at 1.0 ATM pressure.
To calculate the number of moles in 108g of silver, you need to divide the mass of silver by its molar mass. The molar mass of silver is approximately 107.87 g/mol. Dividing 108g by the molar mass gives you around 1 mole of silver.