What is the KSP of calcium chromate?
|calcium chromate||CaCrO4||7.1 x 10-4|
|calcium fluoride||CaF2||5.3 x 10-9|
|calcium hydroxide||Ca(OH)2||5.5 x 10-6|
|calcium iodate||Ca(IO3)2||7.1 x 10-7|
What is the KSP of feoh2?
Problem: The Ksp of iron(II) hydroxide, Fe(OH)2, is 4.87 x 10-17.
Can you use KSP to find solubility?
The Ksp expressions in terms of s can be used to solve problems in which the Ksp is used to calculate the molar solubility as in the examples above. Molar solubility can then be converted to solubility.
How do you find the solubility of an expression?
In this case, we calculate the solubility product by taking the solid’s solubility expressed in units of moles per liter (mol/L), known as its molar solubility. The concentration of Ca2+ in a saturated solution of CaF2 is 2.1 × 10–4 M; therefore, that of F– is 4.2 × 10–4 M, that is, twice the concentration of Ca2+.
What is the value of KSP?
What is Ksp? Ksp (Solubility product constant) is the equilibrium between a solid and its respective ions in a solution. The value of the constant identifies the degree of which the compound can dissociate in water. For example the higher the Ksp the more soluble the compound is.
What is the KSP value of calcium hydroxide at 25 0c?
8 The approximate value of the Ksp for calcium hydroxide is 6.5 × 10–6, so calculate a rough value of the concentration of OH– ion, [OH–], in the saturated solution (see prelab question on WebAssign; to two significant figures).
What is the value of KSP for AgBr?
Table of Solubility Product Constants (Ksp at 25 oC)
|PbBr2||6.3 x 10-6|
|AgBr||3.3 x 10-13|
|BaCO3||8.1 x 10-9|
|CaCO3||3.8 x 10-9|
What is the KSP of BaSO4?
The solubility product (Ksp) of BaSO4 is 1.5 × 10^-9 .
What is the solubility of CaF2?
• Calculating Solubility from Ksp o The Ksp for CaF2 is 3.9 × 10–11 at 25 °C.