Suppose, in the saturated solution of Ca(OH)2 prepared by the TA, some of the dissolved Ca2+ jons re-precipitate as Caco3. This removes Ca2+ ions from the solution. What will the solid Ca(OH)2 present in the bottom of the beaker do in order to minimize the effect of this shift away from equilibrium? What would the effect be on the [OH -] and the calculated Ksp value? O The removal of Ca2+ ions by the precipitation of CaCO3 from solution results in the dissolution of more Ca2+ from Ca(OH)2. As a result, the [OH-] will increase and the estimate of Kep will be too high. O Solid substances are not part of equilibrium equations, so their presence would leave the value of Ksp unaffected. O The removal of Ca2+ ions by the precipitation of CaCo3 from solution results in the co-precipitation of Ca(OH)2 as it attempts to maintain its equilibrium concentrations. As a result, the [OH ] will decrease and the estimate of Ksp will be too low.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
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