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