Q. 9.9 - An Introduction to General, Organic, and Biological Chemistry

Question

Write a balanced equation for the dissociation of each of the following strong electrolytes in water:

a.  $KCl$

b. $CaC{l}_2$

c. $K_{3}P{O}_4$

d. $Fe{\left(N{O}_3\right)}_3$

Step-by-Step Solution

Answer

(part a) The strong electrolytes dissociation$KCl$ is published as $KCl\left(S\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{K}^{+}\left(aq\right)+{\mathrm{Cl}}^{-}\left(aq\right)$

(part b) The strong electrolyte dissociation$CaC{l}_2$ is published  as ${\mathrm{CaCl}}_2\left(S\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Ca}}^{2+}\left(aq\right)+2{\mathrm{Cl}}^{-}\left(aq\right)$

(part c) The strong electrolyte dissociation$K_{3}P{O}_4$ is published as ${\mathrm{K}}_3{\mathrm{PO}}_4( \mathrm{S})\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}3{ \mathrm{K}}^{+}\left(aq\right)+{\mathrm{PO}}_4^{3-}\left(aq\right)$

(part d) The strong electrolytes dissociation $Fe{\left(N{O}_3\right)}_3$ is published as $\mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_3( \mathrm{S})\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Fe}}^{3+}\left(aq\right)+3{\mathrm{NO}}_3^{-}\left(aq\right)$

Step1: Introduction (part a)

A strong electrolyte is a solution/solute which ionized particles or dissolved totally or almost entirely in solution. Inside the solution, such ions are known and respected of electric current.

Step2: Given Information (part a).

Find the balanced equation for the dissociation of the strong electrolyte:

$KCl$

Step3: Explanation (part a).

When $KCl$ reacts with water, it produces $K^{+}$ and $C{l}^{-}$ ions. The $KCl$ dissociative symptoms is written as follows:

$KCl\left(S\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{K}^{+}\left(aq\right)+{\mathrm{Cl}}^{-}\left(aq\right)$

Step4: Given Information (part b).

Find out the balanced equation for the dissociation of the strong electrolyte:

$CaC{l}_2$

Step5: Explanation (part b).

When $CaC{l}_2$ dissolved, it creates one calcium ion for every two chloride ions.$CaC{l}_2$ dissociation is written in the following form:

${\mathrm{CaCl}}_2\left(S\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Ca}}^{2+}\left(aq\right)+2{\mathrm{Cl}}^{-}\left(aq\right)$

Step6: Given Information (part c).

To find the balanced equation for the dissociation of the strong electrolyte:

$K_{3}P{O}_4$

Step7: Explanation (part c).

$K_{3}P{O}_4$ dissolves in the water, liberating three potassium ions in exchange for phosphate ions. $K_{3}P{O}_4$ dissociation is described as follows:

${\mathrm{K}}_3{\mathrm{PO}}_4( \mathrm{S})\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}3{ \mathrm{K}}^{+}\left(aq\right)+{\mathrm{PO}}_4^{3-}\left(aq\right)$

Step8: Given Information (part d).

Find the balanced equation for the dissociation of the strong electrolyte:

$Fe{\left(N{O}_3\right)}_3$

Step9: Explanation (part d).

In water, $Fe{\left(N{O}_3\right)}_3$ absorbs to give one iron ion for each and every three nitrate ions.$Fe{\left(N{O}_3\right)}_3$ dissociation is represented as follows:

$\mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_3( \mathrm{S})\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Fe}}^{3+}\left(aq\right)+3{\mathrm{NO}}_3^{-}\left(aq\right)$