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Acids/Bases
Question | Answer |
---|---|
What ion is involved with acids and bases? | Hydrogen Ion |
What could alter the chemical make up of an acid or base? | Placing them in water. |
When acids are place in water... | Dissolves and splits into 2 ions. (Hydrogen Ions) |
When bases are placed in water... | Dissolves and splits into 2 ions. |
What is different about a base being added to water? | The hydrogen ion binds to oxygen and forms a (OH-) Hydroxide Ion. |
What is the term used to describe the splitting of acid and base ions? | Dissociation |
So when an acid and base undergo dissociation, what are the doing? | Neutralizing |
What makes an acid more acidic? | More dissociation and release of hydrogen ions. |
What makes a base more basic? | More dissociation of hydrogen ions and more binding to release OH-. |
How are acids and bases measured? | pH scale |
What does pH equal? | pH= -log(H+) |
What are the ranges of the pH scale? | 0-14 |
Which side of the scale is acid and which side of the scale is basic? | 0 = most acidic 14 = most basic |
What does 7 on the pH scale represent? Example | Neutral, Water |
What are buffers? | Compounds that maintain neutrality of pH by combing with H+ or OH- ions. |
What is important to know about buffers? | They maintain homeostatic pH in organisms to prevent them from becoming too acidic or basic. |
What is the pH of blood? | 7.35-7.45 |
What are the buffers that maintain physiologic pH? | Carbonate / Phosphate / Proteins |
What is the protein called in our body? | Albumin |
How does our renal system relate to buffers? | It releases Ammonia as a buffer in the renal tubules. |
What is the term used to describe the concept of acid and base? | Bronsted-Lowry Definition |
What is a Bronsted Acid? | A molecule that donates a proton (H+) |
What is a Bronsted Base? | A molecule that accepts a proton (H+) |
When an acid donates a proton, what remains? | Conjugate Base |
When a base accepts a proton, what remains? | Conjugate Acid |
Describe Strong acids? | This molecule completely dissociates in water to yield a high H+ ion concentration. |
Describe Weak acids? | This molecule does not completely dissociate in water yielding a low H+ ion concentration. |
Describe Strong bases? | This molecule completely ionizes in a solution. |
Describe Weak bases? | This molecule does not completely ionizes in a solution. |
What is a common chemical we use in Anesthesia? What type of chemical is it? Where is it found? | Barium Hydroxide / Strong Base / CO2 Absorbent |
What is another example of a strong base? What is the pKa of this example? | Propofol pKa 11 |
What is clinically significant about strong bases? | They burn during injection. |
What do acids and bases contribute to? | Water solubility, ability of a drug to dissolve and enter the system circulation. |
What is also influenced by acids and bases? | Molecular binding to a receptor. |
Acid examples | HCL acid, Lactic acid, Carbonic acid, Ketoacids, Pyruvic acids, Uric acids proteins |
Base examples | Bicarbonate, Phosphates, Proteins, Ammonia |