Percentage of calcium ions removed from the hard water containing Ca 2 + ions by adding soda ash Na 2 CO 3 in the water has to be calculated. Concept introduction: The solubility of a salt is defined as the maximum amount of salt that can be dissolved in definite amount of solvent. It is expressed in moles per liter or grams per liter. Solubility in terms of moles per liter is called molar solubility and is defined as the number of moles of solute (salt) dissolved in per liter of solution. Solubility product constant K sp is an equilibrium constant and is defined as the product of the equilibrium concentration of the ions of the salt raised to the power of their coefficients in the balanced chemical equation. The expression for K sp of a salt is given as, A x B y ( s ) ⇌ x A y + ( aq ) + y B − x ( aq ) K sp = [ A y + ] x [ B − x ] y
Percentage of calcium ions removed from the hard water containing Ca 2 + ions by adding soda ash Na 2 CO 3 in the water has to be calculated. Concept introduction: The solubility of a salt is defined as the maximum amount of salt that can be dissolved in definite amount of solvent. It is expressed in moles per liter or grams per liter. Solubility in terms of moles per liter is called molar solubility and is defined as the number of moles of solute (salt) dissolved in per liter of solution. Solubility product constant K sp is an equilibrium constant and is defined as the product of the equilibrium concentration of the ions of the salt raised to the power of their coefficients in the balanced chemical equation. The expression for K sp of a salt is given as, A x B y ( s ) ⇌ x A y + ( aq ) + y B − x ( aq ) K sp = [ A y + ] x [ B − x ] y
Solution Summary: The author explains that the solubility of a salt is defined as the maximum amount of salt that can be dissolved in definite amounts of solvent.
Percentage of calcium ions removed from the hard water containing Ca2+ ions by adding soda ash Na2CO3 in the water has to be calculated.
Concept introduction:
The solubility of a salt is defined as the maximum amount of salt that can be dissolved in definite amount of solvent. It is expressed in moles per liter or grams per liter. Solubility in terms of moles per liter is called molar solubility and is defined as the number of moles of solute (salt) dissolved in per liter of solution.
Solubility product constant Ksp is an equilibrium constant and is defined as the product of the equilibrium concentration of the ions of the salt raised to the power of their coefficients in the balanced chemical equation.
If 4.5 moles of nitric acid falls into 8000 L of pure water, what will be the change of the pH of the solution? (Note that nitric acid dissociates completely and puts in one hydrogen ion for each molecule of nitric acid)
If 50.0 g of barium arsenate (Ksp = 1.1 x 10 13) are placed in enough water to generate 500.0 mL of solution, calculate the following: %3D The molar solubility of the barium arsenate solution. b. The molar solubility of the barium ion if 30.0 mL of 0.400 M barium nitrate solution is added to the original solution. а. The molar solubility of the barium arsenic solution.
b. The molar solubility of the barium ion if 30.0 mL of 0.400 M barium nitrate solution is added to the original solution.
6. CaF2 (s) ⇌ Ca2+ (aq) + 2 F- (aq)
Dissolution of the slightly soluble salt Calcium Fluoride is shown by the equation above. Which of the following changes will increase [Ca2+] in a saturated solution of Calcium Fluoride, and why? (assume that after each change some Calcium Fluoride (s) remains in contact with the solution)
a)Allowing some of the water to evaporate from the solution, because more Calcium Fluoride (s) will precipitate.
b) Adding 1.0 M HNO3 (aq), because some F- (aq) ions will become protonated.
c) Adding 0.1 M NaNO3 (aq), because additional liquid will dilute the solution.
d) Adding NaF (s), because the reaction will proceed toward reactants.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell