“solubility product”的概念、定义、翻译、参考文献-科学参考

solubility product

Physics

Symbol K_s. The product of the concentrations of ions in a saturated solution. For instance, if a compound A_xB_y is in equilibrium with its solution

$A_{x} B_{y} ⇌ x A^{+} (aq) + y B^{-} (a q)$

the equilibrium constant is

$K_{c} = {[A^{+}]}^{x} {[B^{-}]}^{y} / [A_{x} B_{y}]$

Since the concentration of the undissolved solid can be put equal to 1, the solubility product is given by

$K_{s} = {[A^{+}]}^{x} {[B^{-}]}^{y}$

The expression is only true for sparingly soluble salts. If the product of ionic concentrations in a solution exceeds the solubility product, then precipitation occurs.

Chemistry

The product of the concentrations of ions in a saturated solution. For instance, if a compound A_xB_y is in equilibrium with its solution
$A_{x} B_{y} (s) ⇌ x A^{+} (aq) + y B^{-} (aq)$
the equilibrium constant is
$K_{c} = {[A^{+}]}^{x} {[B^{-}]}^{y} / [A_{x} B_{y}]$
Since the concentration of the undissolved solid can be put equal to 1, the solubility product is given by
$K_{s} {= [A}^{+}]^{x} {{[B}^{-}]}^{y}$
The expression is only true for sparingly soluble salts. If the product of ionic concentrations in a solution exceeds the solubility product, then precipitation occurs.

Geology and Earth Sciences

Constant which describes the product of ionic concentrations of any slightly soluble salt. The solubility of a substance is the maximum amount of that substance which can be dissolved in a solution that is in equilibrium with a solid source of the solute. The main technique for studying solubility involves the use of the solubility product, which is the total number of ions of each type in a compound that can coexist in a solution. At a given temperature and at equilibrium the value for the solubility product will always be the same. For example, in a solution of silver chloride, AgCl dissociates to Ag⁺ and Cl⁻. The solubility product K_sp is the product of their concentrations: K_sp = [Ag⁺][Cl⁻] mole²/litre². The solubility of AgCl in moles per litre is equal to the activity of Ag⁺ or Cl⁻ as one mole of AgCl dissolves in water to give one mole of each in solution. The value of K_sp for AgCl at 25°C is 10^−9.8.

单词	solubility product
释义	solubility product Physics Symbol K_s. The product of the concentrations of ions in a saturated solution. For instance, if a compound A_xB_y is in equilibrium with its solution $A_{x} B_{y} ⇌ x A^{+} (aq) + y B^{-} (a q)$ the equilibrium constant is $K_{c} = {[A^{+}]}^{x} {[B^{-}]}^{y} / [A_{x} B_{y}]$ Since the concentration of the undissolved solid can be put equal to 1, the solubility product is given by $K_{s} = {[A^{+}]}^{x} {[B^{-}]}^{y}$ The expression is only true for sparingly soluble salts. If the product of ionic concentrations in a solution exceeds the solubility product, then precipitation occurs. Chemistry The product of the concentrations of ions in a saturated solution. For instance, if a compound A_xB_y is in equilibrium with its solution $A_{x} B_{y} (s) ⇌ x A^{+} (aq) + y B^{-} (aq)$ the equilibrium constant is $K_{c} = {[A^{+}]}^{x} {[B^{-}]}^{y} / [A_{x} B_{y}]$ Since the concentration of the undissolved solid can be put equal to 1, the solubility product is given by $K_{s} {= [A}^{+}]^{x} {{[B}^{-}]}^{y}$ The expression is only true for sparingly soluble salts. If the product of ionic concentrations in a solution exceeds the solubility product, then precipitation occurs. Geology and Earth Sciences Constant which describes the product of ionic concentrations of any slightly soluble salt. The solubility of a substance is the maximum amount of that substance which can be dissolved in a solution that is in equilibrium with a solid source of the solute. The main technique for studying solubility involves the use of the solubility product, which is the total number of ions of each type in a compound that can coexist in a solution. At a given temperature and at equilibrium the value for the solubility product will always be the same. For example, in a solution of silver chloride, AgCl dissociates to Ag⁺ and Cl⁻. The solubility product K_sp is the product of their concentrations: K_sp = [Ag⁺][Cl⁻] mole²/litre². The solubility of AgCl in moles per litre is equal to the activity of Ag⁺ or Cl⁻ as one mole of AgCl dissolves in water to give one mole of each in solution. The value of K_sp for AgCl at 25°C is 10^−9.8.
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