## What is the KSP of calcium chromate?

Solubility Rules

Compound | Formula | Ksp |
---|---|---|

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)

Formula | Ksp |
---|---|

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.