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20 lip 2023 · Equilibrium constants can be used to calculate the equilibrium concentrations of reactants and products by using the quantities or concentrations of the reactants, the stoichiometry of the balanced chemical equation for the reaction, and a tabular format to obtain the final concentrations of all species at equilibrium.
- 15.4: Heterogeneous Equilibria - Chemistry LibreTexts
The result is that the equilibrium constant expressions...
- 14: Ionic Equilibria in Aqueous Solutions - Chemistry LibreTexts
Many reactions in aqueous solutions involve weak acids or...
- 15.4: Heterogeneous Equilibria - Chemistry LibreTexts
Equilibrium and Acid Reactions. 1.1. Static and Dynamic Equilibrium. 1.2. Factors that Affect Equilibrium. 1.3. Calculating the Equilibrium Constant (K eq) 1.4. Solution Equilibria.
If such a stress is applied, the reversible reaction will undergo a shift in order to re-establish its equilibrium. This is known as Le Chatelier’s Principle. Consider a hypothetical reversible reaction already at equilibrium: A + B ↽−−⇀ C + D A + B ↽ − − ⇀ C + D.
Many reactions in aqueous solutions involve weak acids or bases or slightly soluble substances, and in such cases one or more equilibria are achieved in solution. Furthermore, the equilibrium state is usually reached almost instantaneously, and so we can use the equilibrium law to calculate the concentrations and amounts of substance of ...
The equilibrium constant (\(\text{K}_{\text{c}}\)) is the ratio between the concentration of products and reactants in a chemical reaction. When the concentration of the reactants is much larger than the concentration of the products \(\text{K}_{\text{c}}\) will be small (normally less than one).
It covers equilibrium constant calculations starting with the most trivial cases, and gradually getting harder - up to the moderately difficult examples which may be asked in a UK A' level examination.
Ammonia (base1) reacts with water (acid2) to give the conjugate acid ammonium ion (acid1) and hydroxide ion (base2) of the acid water. On the other hand, water acts as a proton acceptor, or base, in an aqueous solution of nitrous acid. H O + HNO ↔.
