Question

what are concentrated ions​

Answer 1

Answer:

The ionic strength of a solution is a measure of the concentration of ions in that solution. Ionic compounds, when dissolved in water, dissociate into ions. The total electrolyte concentration in solution will affect important properties such as the dissociation constant or the solubility of different salts.

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Answer 2

Answer:

which water ionizes to hydronium ions and hydroxide ions) occurs to a very limited extent. When two molecules of water collide, there can be a transfer of a hydrogen ion from one molecule to the other. The products are a positively charged hydronium ion and a negatively charged hydroxide ion.

text{H}_2text{O}(l)+text{H}_2text{O}(l) rightleftarrows text{H}_3text{O}^+(aq)+text{OH}^-(aq)

We often use the simplified form of the reaction:

text{H}_2text{O}(l) rightleftarrows text{H}^+(aq)+text{OH}^-(aq)

The equilibrium constant for the self-ionization of water is referred to as the ion-product for water and is given the symbol K_w .

K_w = [ text{H}^+ ][ text{OH}^- ]

The ion-product of water (K_w) is the mathematical product of the concentration of hydrogen ions and hydroxide ions. Note that H 2 O is not included in the ion-product expression because it is a pure liquid. The value of K_w is very small, in accordance with a reaction that favors the reactants. At 25°C, the experimentally determined value of K_w in pure water is 1.0 × 10 -14 .

K_w=[text{H}^+][text{OH}^-]=1.0 times 10^{-14}

In pure water, the concentrations of hydrogen and hydroxide ions are equal to one another. Pure water or any other aqueous solution in which this ratio holds is said to be neutral. To find the molarity of each ion, the square root of K_w is taken.

[text{H}^+]=[text{OH}^-]=1.0 times 10^{-7} text{M}

An acidic solution is a solution in which the concentration of hydrogen ions is greater than the concentration of hydroxide ions. For example, hydrogen chloride ionizes to produce H + and Cl − ions upon dissolving in water.

text{HCl}(g) rightarrow text{H}^+(aq) + text{Cl}^-(aq)

This increases the concentration of H + ions in the solution. According to LeChâtelier’s principle, the equilibrium represented by text{H}_2text{O}(l) rightleftarrows text{H}^+(aq)+text{OH}^-(aq) is forced to the left, towards the reactant. As a result, the concentration of the hydroxide ion decreases.

A basic solution is a solution in which the concentration of hydroxide ions is greater than the concentration of hydrogen ions. Solid potassium hydroxide dissociates in water to yield potassium ions and hydroxide ions.

text{KOH}(s) rightarrow text{K}^+(aq)+text{OH}^-(aq)

The increase in concentration of the OH − ions causes a decrease in the concentration of the H + ions and the ion-product of [H + ][OH − ] remains constant