Could someone clarify for me what a buffer exactly? I am confused as to both what they are and what their intended purpose is? Also, how do you identify them?
Thanks
Buffer Definition
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 105
- Joined: Wed Sep 30, 2020 9:48 pm
- Been upvoted: 2 times
Re: Buffer Definition
A buffer is an aqueous solution containing a weak acid and its conjugate base or a weak base and its conjugate acid. A buffer's pH changes very little when a small amount of strong acid or base is added to it. It is used to prevent any change in the pH of a solution so you would use it in an experiment that requires specific and stable pH values.
-
- Posts: 112
- Joined: Wed Sep 30, 2020 10:03 pm
Re: Buffer Definition
Hi there!
A buffer is a solution that can resist pH changes. They're super important for biological systems because these systems need to maintain homeostasis and avoid dramatic changes. Therefore, a lot of biological systems will have buffers. One example of these systems is the bicarbonate buffer system in blood. Blood contains H2CO3 and NaHCO3.
H₂CO₃ + H₂O ⇌ H₃O⁺+ HCO₃⁻
Since H3O+ determines pH, this buffer system serves to maintain the same H3O+ concentration. If there are too many H3O+, it will react with the bicarbonate and form water and carbonic acid (which removes the H3O from the system). If there are too little H3O+, the carbonic acid will revert into H3O+ and HCO3-.
Buffers are always solutions of a WEAK ACID (or base) AND ITS SALT/conjugate. In the above example, H2CO3 is the weak acid and NaHCO3 is its salt. The important thing to remember is that NaHCO3 contains the conjugate that we need.
Hope this helps :))
A buffer is a solution that can resist pH changes. They're super important for biological systems because these systems need to maintain homeostasis and avoid dramatic changes. Therefore, a lot of biological systems will have buffers. One example of these systems is the bicarbonate buffer system in blood. Blood contains H2CO3 and NaHCO3.
H₂CO₃ + H₂O ⇌ H₃O⁺+ HCO₃⁻
Since H3O+ determines pH, this buffer system serves to maintain the same H3O+ concentration. If there are too many H3O+, it will react with the bicarbonate and form water and carbonic acid (which removes the H3O from the system). If there are too little H3O+, the carbonic acid will revert into H3O+ and HCO3-.
Buffers are always solutions of a WEAK ACID (or base) AND ITS SALT/conjugate. In the above example, H2CO3 is the weak acid and NaHCO3 is its salt. The important thing to remember is that NaHCO3 contains the conjugate that we need.
Hope this helps :))
-
- Posts: 103
- Joined: Wed Sep 30, 2020 9:57 pm
Re: Buffer Definition
A buffer is a solution that resists pH change when an acidic or basic compound is added. It's composed of a conjugate acid and conjugate base that are present in equilibrium, and they neutralize acids and bases in the form of hydronium and hydroxide ions.
-
- Posts: 102
- Joined: Fri Sep 24, 2021 5:00 am
Return to “*Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)”
Who is online
Users browsing this forum: No registered users and 1 guest