Strong+and+weak+acids+and+bases

=** Strong & Weak acids **= A strong acid is one that is completely dissociated in a dilute aqueous solution. HCl (aq) ---> H +  (aq) + Cl -  (aq) Such solutions are good conductors of electricity as there are mobile ions present to conduct electricity. Other common strong acids are H 2 SO 4  and HNO 3 H 2 SO 4  (aq) ---> H +  (aq) + CH 3 COO -  (aq) Almost all organic acids are weak acids. Eg: CO 2 <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">(aq) + H 2 <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">O (l) H + <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (aq) + HCO3- (aq) //<span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Examples of inorganic weak acids: // <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Aqueous sulphur dioxide and Hydrochloric acid

=** Strong or Weak acid?? **= <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Strong and weak acids can be compared by using their solutions of equal concentrations.
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">The concentration of H + <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> ions is the weak acid will be much lower than for the strong acid.
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A weak acid has a higher pH than a strong acid of equal concentration.
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A weak acid doesn’t conduct electricity as good as a strong acid (of equal concentration) but it conducts electricity better than water
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Weak acids react less strongly than strong acids of equal concentration.

=** Strong and Weak bases **= <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A strong base is one that dissociates completely in aqueous solutions <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Eg: NaOH (aq) ---> Na + <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (aq) + OH - <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (aq) <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A weak base is one that dissociates slightly in aqueous solutions <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Eg: NH 3 <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (aq) + H 2 <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">O (l) NH 4 + <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (aq) + OH - <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (aq)

=** Strong or Weak Base?? **= <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Strong and weak bases can be compared by using their solutions of equal concentrations.
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A weak base has a lower pH than a strong base.
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A strong base conducts electricity better than a weak base.
 * <span style="font-family: Tahoma,sans-serif; font-size: 14pt;">A strong base reacts more strongly than a weak base.

<span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Note: distinguish between the terms //** strong & weak, ** ** dilute & concentrated **//<span style="font-family: Tahoma,sans-serif; font-size: 14pt;">. They don’t mean the same. //** Dilute & concentrated **//<span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> refers to whether there is a large or small number of moles of ions in a given volume.
 * // Strong & weak //**<span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> refers to whether the acid/base is fully or partially dissociated.

By the end of this lesson you should be able to;
 * Distinguish between strong and weak acids and bases
 * Know the characteristic of a strong/weak acid/base


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