What is the KSP of caco3?
What is the KSP of caco3?
Conversion of Ksp to Solubility
| Compound | Ksp |
|---|---|
| CaCO 3 | 4.5 × 10 -9 |
| Ca(OH) 2 | 6.5 × 10 -6 |
| Ca 3 (PO 4 ) 2 | 1.2 × 10 -26 |
| CaSO 4 | 2.4 × 10 -5 |
Is MgCO3 soluble or insoluble?
Explanation: Per the solubility rules, the carbonates of Group 2 metals are insoluble. Thus, MgCO3 is insoluble. Its solubility is only 14 mg/100 mL.
What is the KSP of magnesium hydroxide?
The Ksp of magnesium hydroxide Mg(OH)2 is 5.61 x 10^-12.
What is the molar solubility of MgCO3 in water?
2.61×10-3 M
What is the solubility of MgCO3?
Magnesium carbonate
| Names | |
|---|---|
| Solubility in water | anhydrous: 0.0139 g/100ml (25 °C) 0.0063 g/100ml (100 °C) |
| Solubility product (Ksp) | 10−7.8 |
| Solubility | soluble in acid, aqueous CO2 insoluble in acetone, ammonia |
| Magnetic susceptibility (χ) | −32.4·10−6 cm3/mol |
Which of the following salts would have the greatest solubility in water?
Hence, Ag2CO3 has the greatest molar solubility in pure water.
Which compound has the highest molar solubility?
MgCO3
What is the solubility of mgf2 in pure water?
2 Answers. Stefan V. In your case, the molar solubility of magnesium fluoride will be 6.4⋅10−7mol/L .
Which salt will precipitate first CaF2 or baf2?
(b i) CaF2 will precipitate first. Its Ksp value is smaller (and the salt is the same number of ions; MX2), thus the ion- concentration product [Ca2+] [F−]2 will be the first to exceed the Ksp value. When a Q exceeds Ksp the solution will begin to precipitate.
How do you calculate GL solubility?
Divide the number of moles by the solution volume in liters to calculate solubility in mole/L. In our example, the solution volume is 55 mL or 0.055 L. The solubility of NaNO3=0.258 moles/0.055 L=4.69 mole/L.
What are the units of KSP?
The K s p value does not have any units because the molar concentrations of the reactants and products are different for each equation.
What is a high KSP?
Ksp (Solubility product constant) is the equilibrium between a solid and its respective ions in a solution. For example the higher the Ksp the more soluble the compound is.
How does pressure affect KSP?
An increase in pressure and an increase in temperature in this reaction results in greater solubility. An increase in pressure results in more gas particles entering the liquid in order to decrease the partial pressure. Therefore, the solubility would increase.