It's a butter.
In order to have an effective buffer, one needs to have a weak acid or a weak base, and the salt (conjugate) of that weak acid or weak base. Examples would be :weak acid/conjugate base: acetic acid/sodium acetateweak base/conjugate acid: ammonia/ammonium chloride
In general, a buffer system can be represented by writing a salt followed by slash and an acid or conjugate base followed by slash and an acid like salt/acid or conjugate base/acid. Thus, the sodium acetate-acetic acid buffer system can be written asCH3COONa/ CH3COOH or CH3COO-/CH3COOHSimilarly, ammonia-ammonium chloride buffer system can be represented asNH3 / NH4+Note that NH4+ is an acid and NH3 is a conjugate base according to Lewry-Bronsted concept.
A strong acid and a strong base will react together to produce a neutral salt. E.g., HCl (strong acid) and NaOH (strong base) will react together to form H20 and NaCl (salt). The salt is neutral (if you dump table salt into water, the solution will be neutral) this is because the Na+ and Cl- are perfectly happy being charged atoms. If you have something that doesn't really like to be ionized, which is a weak acid or base (for example acetic acid, (vinegar) which is only 1.1% ionized (charged) in a water solution) will only be ionized if something forces it to be ionized, i.e., a strong acid or base. When there is a mixture of a weak acid and its conjugate salt (or weak base and its conjugate salt) a buffer is formed. This is due to the fact that if you add some strong acid it will simply react with the conjugate salt, and if you add some strong base it will react with the weak acid. This is how they "buffer solutions" by keeping things pretty balanced. So to answer your question, a buffer must contain something that is only weakly reactive, and can react further when the need is present. A strong acid/base will totally react, so there is nothing left over to do any buffering.
If you are titrating a base, using a weak acid as titrant would lead to the formation of a buffer as you added the weak acid. The weak acid would react with the base to form the salt of the weak acid + water, and this would buffer any changes in pH, thus making the titration meaningless.
You can mix Weak acid and its salt or weak base and its salt according to pH you want to get.But pH depend upoun the Ka or Kb value. According to Henderson's law pH=pKa+ log[salt]/[acid] Modify this if base is taken
No, NaOH is a strong base and NaCl is the salt of a strong acid and a strong base and so has no acidic or basic properties. A buffer solution requires an acidic or basic salt and the corresponding weak acid or base.
In order to have an effective buffer, one needs to have a weak acid or a weak base, and the salt (conjugate) of that weak acid or weak base. Examples would be :weak acid/conjugate base: acetic acid/sodium acetateweak base/conjugate acid: ammonia/ammonium chloride
Requirements for a Buffer Solution:There are three requirements for buffer:• Must be a mixture of weak acid and its salt or weak base and its salt• A buffer must contain relatively large concentration of acid to react with added base (OH-) and also must contain similar concentration of base to reaction with added acid (H+).• The acid and base components of the buffer must not consume each other in a neutralization reaction.
A buffer
you'll need a salt as well. Buffers are made up of an acid/base and its salt.
In general, a buffer system can be represented by writing a salt followed by slash and an acid or conjugate base followed by slash and an acid like salt/acid or conjugate base/acid. Thus, the sodium acetate-acetic acid buffer system can be written asCH3COONa/ CH3COOH or CH3COO-/CH3COOHSimilarly, ammonia-ammonium chloride buffer system can be represented asNH3 / NH4+Note that NH4+ is an acid and NH3 is a conjugate base according to Lewry-Bronsted concept.
Increase the concentration of salt and acid or base. If you are not suppose to increase concentration use more volume of buffer.
It is neither. Potassium Chlorite is a white crystalline substance that is actually a salt.
when the capacity equals PKa where concentrations of acid and salt are the same that means Log base/acid equals zero
The acid and base will neutralize each other and the resulting solution will be more neutral. If the base being neutralized is strong, the resulting salt will be neutral. If the base is weak the resulting salt will be acidic. A solution of such a salt may be called a buffer.
A strong acid and a strong base will react together to produce a neutral salt. E.g., HCl (strong acid) and NaOH (strong base) will react together to form H20 and NaCl (salt). The salt is neutral (if you dump table salt into water, the solution will be neutral) this is because the Na+ and Cl- are perfectly happy being charged atoms. If you have something that doesn't really like to be ionized, which is a weak acid or base (for example acetic acid, (vinegar) which is only 1.1% ionized (charged) in a water solution) will only be ionized if something forces it to be ionized, i.e., a strong acid or base. When there is a mixture of a weak acid and its conjugate salt (or weak base and its conjugate salt) a buffer is formed. This is due to the fact that if you add some strong acid it will simply react with the conjugate salt, and if you add some strong base it will react with the weak acid. This is how they "buffer solutions" by keeping things pretty balanced. So to answer your question, a buffer must contain something that is only weakly reactive, and can react further when the need is present. A strong acid/base will totally react, so there is nothing left over to do any buffering.
NaHS is known as an acid salt which acts as a "buffer". Therefore, it really depends on the solution and not just NaHS itself since an acid salt can be at times an acid and at times a base. Source: Acid Salt see link below: