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Understanding Acid Strength and Concentration in Solutions

The extent to which acid dissociates determines its strength; polar water allows acids to dissolve. Strong acids dissociate completely, while weak acids release fewer hydrogen ions. Lower pH indicates stronger acid strength. Strong acids, like H2SO4 and HCl, almost fully dissociate, while weak acids, like H2CO3 and CH3COOH, partially dissociate. Understanding the difference between strength (strong or weak) and concentration (dilute or concentrated) is vital in chemistry.

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Understanding Acid Strength and Concentration in Solutions

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  1. extent to which the acid dissociates determines its strength Polar water allows for acids to dissolve Strong Acid - Dissociates completely in a solvent Weak Acid - Releases few hydrogen ions in the solution. ** Lower the pH the stronger the acid** Strength of Acids

  2. strong acids almost completely dissociate 10 H2SO4 18 H+ + 9 SO4-2 + 1 H2SO4 10 HCl 9 H+ + 9 Cl- + 1 HCl weak acids only partially dissociate 10 H2CO3 2 H+ + 2 HCO3-2 + 8 H2CO3 18 CH3COOH 3 H+ + 3 CH3COO- + 7 CH3COOH

  3. Often confused Strength (strong or weak) – how acid dissociates Concentration (dilute or concentrated) – amount of acid dissolved in the solution. It is possible to have a dilute solution of a strong acid! Strength and concentration

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