SrSO4 is considered slightly soluble in water. It has a solubility of approximately 0.013 g/100 mL at 25°C. Hence, it exhibits low solubility compared to some other salts.
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.
solubility = [Ba2+]= 80 x 10-6 M When BaSO3 dissolves it gives equal concentration of Ba2+ and SO32-, so Ksp = [Ba2+][SO32-] = 6.4 x10-9
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.
SrSO4 is the chemical formula for strontium sulfate, a white crystalline solid that is insoluble in water. It is commonly used in the production of fireworks, pigments, and in the oil refining industry.
SrSO4 is considered slightly soluble in water. It has a solubility of approximately 0.013 g/100 mL at 25°C. Hence, it exhibits low solubility compared to some other salts.
The 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 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.
solubility = [Ba2+]= 80 x 10-6 M When BaSO3 dissolves it gives equal concentration of Ba2+ and SO32-, so Ksp = [Ba2+][SO32-] = 6.4 x10-9
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.
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.
SrSO4 is the chemical formula for strontium sulfate, a white crystalline solid that is insoluble in water. It is commonly used in the production of fireworks, pigments, and in the oil refining industry.
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.
Find the constant, which i think is 3.7*10^-4 and multiply it by 1.0. and you should get your answer
SrSO4
Strontium sulfate.