[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Acid/Base Reactions > Using Brønsted–Lowry Theory >[/cs_text][cs_text]Differences between concentrated and dilute acids[/cs_text][/cs_column][/cs_row][/cs_section][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]
| Concentrated Acids | Dilute Acids |
|---|---|
| Have relatively large amount of solute dissolved in solvent | Have less amount of solute dissolved in solvent |
| Have higher Ka value | Have low Ka value |
| pH ranges from 1 – 3.5 | pH ranges from 4 – 7 |
[/cs_text][/cs_column][/cs_row][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Differences between weak and strong acids[/cs_text][/cs_column][/cs_row][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]
| Strong Acids | Weak Acids |
|---|---|
| Completely dissociate in water to produce H+ | Dissociate partially in aqueous solution |
| Have lower pH value (0 – 1) | Have lower pH value (5 – 7) |
| Are mostly inorganic acids; Example: HCl, HNO3, H2SO4 etc. | Are mostly organic acids; Example: HCOOH, CH3COOH etc. |
[/cs_text][cs_text]Differences between concentrated and dilute bases[/cs_text][cs_text]
| Concentrated Bases | Dilute Bases |
|---|---|
| Have relatively large amount of basic solute dissolved in solvent | Have less amount of solute dissolved in solvent |
| Have higher Kb value | Have low Kb value |
| pH ranges from 7 – 10 | pH ranges from 12 – 14 |
[/cs_text][cs_text]Differences between weak and strong bases[/cs_text][cs_text]
| Strong Bases | Weak Bases |
|---|---|
| Completely dissociate in water to produce OH- | Dissociate partially in aqueous solution |
| pH ranges from 7.3 – 10 | pH ranges from 10 – 14 |
| Have higher electrical conductivity | Have lower electrical conductivity |
| Example: NaOH, KOH, Ca(OH)2 etc. | Example: Hydrazine, alanine, dimethylamine etc. |
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