Question

Rank the following in order of increasing molar solubility. Question List (5 items) (Drag and drop into the appropriate area) Calcium fluoride Calcium phosphate Kp 2.1X10-33 Calcium hydroxide Ksp 4.7 X10-6 Ksp 3.9 x10-11 Calcium carbonate Calcium sulfate Ksp = 5.0×10-9 Ksp = 7.1 ×10-5

Answer 1

The molar solubility of the compounds, listed in order of increasing solubility, is calcium phosphate, calcium carbonate, calcium hydroxide, calcium sulfate, and calcium fluoride.

Step-by-step explanation:

1. Calcium phosphate (Ksp = 2.07 × 10-33)
2. Calcium carbonate (Ksp = 4.5 × 10-9)
3. Calcium hydroxide (Ksp = 7.1 × 10-5)
4. Calcium sulfate (Ksp = 5.0 × 10-9)
5. Calcium fluoride (Ksp = 3.9 × 10-11)

The molar solubility of a compound can be determined based on its solubility product constant (Ksp). The compounds with lower Ksp values have lower molar solubilities. In this case, the molar solubility increases from calcium phosphate to calcium fluoride.

Answer 2

The compounds are ranked from least to most soluble based on their Ksp values: calcium phosphate, calcium fluoride, calcium carbonate, calcium sulfate, and finally calcium hydroxide.

Step-by-step explanation:

To rank the compounds calcium fluoride, calcium phosphate, calcium hydroxide, calcium carbonate, and calcium sulfate in order of increasing molar solubility using their solubility product constants (Ksp), one must consider that a lower Ksp generally indicates a lower solubility. Given the Ksp values, we can determine this order:

1. Calcium phosphate (Ksp = 2.1×10⁻³³)
2. Calcium fluoride (Ksp = 3.9×10⁻¹¹)
3. Calcium carbonate (Ksp = 5.0×10⁻⁹)
4. Calcium sulfate (Ksp = 7.1×10⁻⁵)
5. Calcium hydroxide (Ksp = 4.7×10⁻⁶)

The order is from the least soluble (lowest Ksp) to the most soluble (highest Ksp). Remember that the actual solubility can be influenced by factors such as the presence of common ions or changes in pH.