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- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Foundations_of_Introductory_Chemistry-1/17%3A_Chemical_Equilibrium/17.7%3A_Solubility_EquilibriaIn order to write the expression for the equilibrium constant for this solubility reaction, we need to recall the rules stated in Section 10.2 of this chapter; Rule #4 states, “Reactants or products t...In order to write the expression for the equilibrium constant for this solubility reaction, we need to recall the rules stated in Section 10.2 of this chapter; Rule #4 states, “Reactants or products that are present as solids or liquids or the solvent, all have an activity value of 1, and so they do not affect the value of the equilibrium expression.” Because silver chloride is a solid, and water is the solvent, the expression for the equilibrium constant is simply,
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.13%3A_Conversion_of_(K_textsp)_to_SolubilityThis page outlines the purification of drinking water, emphasizing the removal of heavy metals through the formation of insoluble compounds using carbonates and sulfates. It details the calculation of...This page outlines the purification of drinking water, emphasizing the removal of heavy metals through the formation of insoluble compounds using carbonates and sulfates. It details the calculation of molar solubility via solubility product constants (\(K_\text{sp}\)), including the creation of an ICE table to find ion concentrations and deriving molar solubility. The final conversion from molar solubility to solubility is also addressed.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)/10%3A_Principles_of_Chemical_Equilibrium/10.7%3A_Solubility_EquilibriaIn order to write the expression for the equilibrium constant for this solubility reaction, we need to recall the rules stated in Section 10.2 of this chapter; Rule #4 states, “Reactants or products t...In order to write the expression for the equilibrium constant for this solubility reaction, we need to recall the rules stated in Section 10.2 of this chapter; Rule #4 states, “Reactants or products that are present as solids or liquids or the solvent, all have an activity value of 1, and so they do not affect the value of the equilibrium expression.” Because silver chloride is a solid, and water is the solvent, the expression for the equilibrium constant is simply,
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.07%3A_Solving_Equilibrium_ProblemsThis page discusses using ladder diagrams and algebraic solutions to evaluate and solve equilibrium problems related to chemical reactivity and solubility. It begins with a straightforward example of ...This page discusses using ladder diagrams and algebraic solutions to evaluate and solve equilibrium problems related to chemical reactivity and solubility. It begins with a straightforward example of calculating the solubility of Pb(IO3)2 in deionized water and proceeds to more complex scenarios considering the common ion effect and the presence of ligands.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Chem_51/17%3A_Chemical_Equilibrium/17.7%3A_Solubility_EquilibriaIn order to write the expression for the equilibrium constant for this solubility reaction, we need to recall the rules stated in Section 10.2 of this chapter; Rule #4 states, “Reactants or products t...In order to write the expression for the equilibrium constant for this solubility reaction, we need to recall the rules stated in Section 10.2 of this chapter; Rule #4 states, “Reactants or products that are present as solids or liquids or the solvent, all have an activity value of 1, and so they do not affect the value of the equilibrium expression.” Because silver chloride is a solid, and water is the solvent, the expression for the equilibrium constant is simply,
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/16%3A_Appendix/16.10%3A_Solubility_ProductsThis document lists pKsp and Ksp values for various compounds, categorized by their anions. The information originates from the reference "Critical Stability Constants, Vol. 4" by Martell and Smith. T...This document lists pKsp and Ksp values for various compounds, categorized by their anions. The information originates from the reference "Critical Stability Constants, Vol. 4" by Martell and Smith. The values, unless noted otherwise, are measured at 25??C and zero ionic strength. Compounds are organized under anions such as Bromide, Carbonate, Chloride, Chromate, and others, with specific pKsp and Ksp indicated for each, providing important data for assessing compound solubility.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.15%3A_Common_Ion_EffectThis page discusses lithium carbonate's role in lithium batteries, produced through a reaction with carbon dioxide. It explains the common ion effect, where adding a common ion decreases a compound's ...This page discusses lithium carbonate's role in lithium batteries, produced through a reaction with carbon dioxide. It explains the common ion effect, where adding a common ion decreases a compound's solubility, illustrated by adding calcium nitrate to calcium sulfate. This shifts equilibrium, causing precipitation. Additionally, calculations show how common ions, like hydroxide with zinc hydroxide, affect ion concentrations in solutions.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/09%3A_Titrimetric_Methods/9.05%3A_Precipitation_TitrationsThe document discusses precipitation titrimetry, a type of titration where the analyte and titrant form an insoluble precipitate. It covers historical applications, calculation of titration curves, an...The document discusses precipitation titrimetry, a type of titration where the analyte and titrant form an insoluble precipitate. It covers historical applications, calculation of titration curves, and methods for identifying the end point using indicators or potentiometric titrations. The document also provides quantitative applications and calculations for estimating analyte concentrations in mixtures.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.12%3A_Conversion_of_Solubility_to_(K_textsp)This page details the preparation of sodium bicarbonate from ammonia and sodium chloride via a reaction with carbon dioxide, leading to its precipitation. It covers solubility measurements in grams pe...This page details the preparation of sodium bicarbonate from ammonia and sodium chloride via a reaction with carbon dioxide, leading to its precipitation. It covers solubility measurements in grams per liter and their conversion to molar solubility. Using lead (II) fluoride as a case study, the page illustrates how to calculate the solubility product constant (K_sp) from molar solubility by determining ion concentrations and applying the K_sp equation.
