Below are the values of the Ksp product constant for the most common salts
Table of Contents
What is the Ksp of calcium iodate?
Below are the values of the Ksp product constant for the most common salts
| Compound | Formula | Ksp (at 25 oC) |
|---|---|---|
| Calcium iodate | Ca(IO3)2 | 6.47 x 10-6 |
| Calcium iodate hexahydrate | Ca(IO3)2 x 6H2O | 7.10 x 10-7 |
| Calcium molybdate | CaMoO | 1.46 x 10-8 |
| Calcium oxalate monohydrate | CaC2O4 x H2O | 2.32 x 10-9 |
What is the Ksp of CaSO4?
Ksp of CaSO4 is 4 × 10^-12.
What is the Ksp of calcium hydroxide?
6.5 × 10–6
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 solubility product constant Ksp?
The solubility product constant, Ksp, is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the level at which a solute dissolves in solution. The more soluble a substance is, the higher the Ksp value it has.
How do you find the molar solubility of calcium iodate?
The molar solubility of calcium iodate will be equal to one half the iodate concentration {see Equations (3) and (4)}. Calculate the solubility product constant for calcium iodate {see Equation (5)}. Filter ~30mL of the saturated calcium iodate solution in 0.0100 M KIO3 through a short neck funnel.
How do you find the solubility constant?
To do this, simply use the concentration of the common ion as the initial concentration. Example: Estimate the solubility of barium sulfate in a 0.020 M sodium sulfate solution. The solubility product constant for barium sulfate is 1.1 x 10-10.
How do you calculate the solubility of CaSO4?
The solubility of CaSO4 is given by a two-term equation, S = [Ca2+] + [CaSO4]. (6) In equation (6), [Ca2+]= the molarity of Ca2+ ions in solution and [CaSO4] = the concentration of the ion pair, M.
What is the Ksp value?
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.
How do you write a solubility product constant expression?
The equilibrium expression, Ksp, is a ratio of products over reactants and can be written as Ksp = [products]/[reactants]. This expression represents the equilibrium between an ionic solid and its ions in solution.
How do you find the solubility product constant?
What is the Ksp of caco3?
Calcium Carbonate and Water An average value for the Ksp of calcium carbonate is about 5 x 10-9.
What is the Ksp expression for caco3?
Ksp, Solubility of Minerals
| compound | formula | Ksp |
|---|---|---|
| Barium carbonate | BaCO3 | 2.58 x 10-9 |
| Calcium carbonate (calcite) | CaCO3 | 3.36 x 10-9 |
| Calcium carbonate (aragonite) | CaCO3 | 6.0 x 10-9 |
| Calcium hydroxide | Ca(OH)2 | 5.02 x 10-6 |
How is Ksp calculated?
Next we write out the expression for Ksp , then “plug in” the concentrations to obtain the value for Ksp. Let’s do an example: The solubility of Ag2CrO4 in water is 1.31 x 10-4 moles/L. Calculate the value of Ksp . Using mole ratios, the [Ag+] will go up by (2 x 1.31 x 10-4 moles/L) = 2.62 x 10-4 moles/L.
How do I calculate Ksp?
Ksp is constant at a given temperature (van’t Hoff equation) for a saturated solution of a given compound.
- Problem: Write the Ksp expression for the following weak electrolytes: Mn(OH)3(s), Sr3(AsO4)2(s), and Co2S3(s).
- Calculating Solubility from Ksp:
- Ksp = [Ca2+][F-]2 = [2.14×10-4][4.28×10-4]2 = 3.9 x 10-11