weak acids are different than strong acids. strong acids completely dissociate in water. weak acids, having…

weak acids are different than strong acids. strong acids completely dissociate in water. weak acids, having the generic formula ha, only partially dissociate. which bar chart describes this weak - acid behavior? (the bar charts represent initial and final amounts of chemicals dissolved in water.) initial amounts final amounts initial amounts final amounts ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ initial amounts final amounts initial amounts final amounts ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻

weak acids are different than strong acids. strong acids completely dissociate in water. weak acids, having the generic formula ha, only partially dissociate. which bar chart describes this weak - acid behavior? (the bar charts represent initial and final amounts of chemicals dissolved in water.) initial amounts final amounts initial amounts final amounts ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ initial amounts final amounts initial amounts final amounts ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻ ha h₃o⁺ a⁻

Answer

Explanation:

Step1: Understand weak - acid dissociation

A weak acid HA in water has the equilibrium reaction $HA + H_2O\rightleftharpoons H_3O^++A^-$. Initially, there is only HA.

Step2: Analyze dissociation result

Since it is a partial - dissociation, at equilibrium, there will still be some HA remaining along with the formed $H_3O^+$ and $A^-$ ions.

Step3: Evaluate bar - charts

The bar - chart should show a non - zero amount of HA in the final amounts, along with non - zero amounts of $H_3O^+$ and $A^-$. The first bar - chart in the top left (where in the initial amounts there is only HA and in the final amounts there is some HA left along with $H_3O^+$ and $A^-$) is correct.

Answer: The first bar - chart in the top left (where in the initial amounts there is only HA and in the final amounts there is some HA left along with $H_3O^+$ and $A^-$)