--- ## Acids - proton donors (H+) - Acids are molecules that when hydrated *release* positively charged hydrogen [[Ion]]s. *Also known as protons since they have 1 proton with no electron.* - Strong acids are also **strong electrolytes** *(see [[Solutions]] for more).* - **Acids are proton donors**. >[!tip] >#### Strong acids: >- Strong acids are also **strong electrolytes**. >- HCl is a very strong acid and when dissolved in water will undergo **complete ionization** meaning it splits up into ions. It is a strong acid **because it readily dissociates** pumping tons of H and Cl ions into the solution. >- ![[Pasted image 20230216114150.png|700]] > - Note here that the hydronium ion and chlorine ion are the **dominant species** since they will have the greatest effect on other chemicals in the solution. *not sure on this one though.* > </br> > >#### Weak acids: >- Weak acids are **weak electrolytes**. >- HF is an example of a weak acid **because when put in solution it does not dissociate as well** meaning there are less H and F ions in solution. >- Insoluble salts are also generally *weak acids*. >- ![[Pasted image 20230216114908.png|700]] >- Here **HF and water are the dominant species** since not many ions are dissociated. >[!caution] >- Its important to note that the **Arrhenius model of acids and bases says that acids product H+ ions and bases produce HO- ions**. >- On the other hand **the Bronsted-Lowery model says that acids are proton donors and bases are proton acceptors.** >- Both of these are true statements. #### What is hydronium? - When acids are dissolved in water they dissociate releasing H+ ions into the [[Solutions|solution]] which bond with water to create a positively charged H3O+ molecule *(known as hydronium)* - Hydronium is also called a *hydrated proton*. #### Acids to know: - **Strong acids: ** >![[Pasted image 20230216115607.png|500]] - **Polyprotic acids** lose their first H+ easily forming another *often weak* acid behind. > ![[Pasted image 20230216115848.png|500]] > ![[Pasted image 20230216115920.png]] --- ## Bases - proton acceptors (OH-) - Bases are molecules that when hydrated releases **OH hydroxide** molecules. - Like acids stronger bases are **stronger electrolytes**. - **Bases are proton-acceptors.** --- ## pH >[!quote] >![[Files/Acids and bases.png|800]] --- ## Titration - An acid base titration is a way of determining the **concentration** of a solution by slowly adding an acid into a basic solution *(or the other way around)* of unknown concentration. Using an **indicator which changes color at a certain pH level** we can calculate the concentration of the solution based on the amount of the acid we needed to add. - When the indicator changes color the **moles of the titrant are equal to the moles of the acid or base** with an unknown concentration. >[!quote] >![[Acids and bases 1.png|800]] --- #subpage