What is KSP of PbSO4?

What is KSP of PbSO4?

The Ksp of PbSO4 is 1.3 x 10-8.

Why does NaCl not have a KSP?

Originally Answered: why solubility product concept is not applicable to soluble salts like NaCl? Nacl being very strong electrolyte has dissotiation constant ksp very very large.so it almost completly breaks into na+ and cl-. It means reaction go completly forward . so there is no need to consider ksp.

Is KSP constant?

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.

Does a higher KSP precipitate first?

If Q = Ksp, a precipitate will form. If Q > Ksp, a precipitate will form. Note that precipitation may not happen immediately if Q is equal to or greater than Ksp. Because Ksp for SrCrO4 is smaller than for BaCrO4, SrCrO4 will precipitate first.

How do you compare KSP?

The greater the Ksp the more ions are in solution, hence the greater the molar solubility. However, you can only directly compare salts that give equivalent numbers of ions in solution. For example, you can compare the Ksp’s of all salts with a 1:1 ion ratio like: AgBr, BaSO4 etc.

Which substance has the greatest solubility in water?

NiCO3

How does temperature affect KSP?

The effect of temperature on solubility can be explained on the basis of Le Chatelier’s Principle. Therefore, the solubility (concentration) increases with an increase in temperature. If the process is exothermic (heat given off). A temperature rise will decrease the solubility by shifting the equilibrium to the left.

How do you find KSP from grams?

2) divide the grams per liter value by the molar mass of the substance. This gives moles per liter, which is molar solubility. After the above conversion, the problem becomes calculate the Ksp from molar solubility data.

What is KSP of AgCl?

Ksp (AgCl) = 1.7 x10-10.

How do you find solubility given KSP?

Set up an ICE problem (Initial, Change, Equilibrium) in order to use the Ksp value to calculate the concentration of each of the ions. The concentration of the ions leads to the molar solubility of the compound. Use the molar mass to convert from molar solubility to solubility.

Which salt has the greatest solubility?

Hence, Ag2​CO3​ has the greatest molar solubility in pure water.

Which compound will have the lowest solubility?

hexanol

Which salt has the lowest solubility?

barium sulphate

Which compound has the lowest solubility in pure water?

MgF2, Ksp 6.9 X 10-9 The Correct Answer Is: FePO, Ksp 1.3 X 10-22.