Use the Henderson-Hasselbalch equation:
[H+] = Ka * [HA] / [A-]
where
and
and
[H+] = Ka * [HA] / [A-] = (4.7*10-4) * (0.15) / (0.20) = 3.5*10-4 ,
so :
pH = -log[H+] = -log(3.5*10-4) = 3.45
Solutions that resist change in pH when added to a strong acid or base are known as buffer solutions.
a solution which does not fulfills the property of a buffer solution but act as buffer solution.
If the solution is not a buffer, the HCl will react with the solution to form a product.
The buffer solution is destroyed if the amount of acid or base that can be absorbed is exceded.
H2CO3 is not used as buffer.
A buffer
Solutions that resist change in pH when added to a strong acid or base are known as buffer solutions.
a solution which does not fulfills the property of a buffer solution but act as buffer solution.
HCl + NaF -> HF + NaCl
If the solution is not a buffer, the HCl will react with the solution to form a product.
The buffer solution is destroyed if the amount of acid or base that can be absorbed is exceded.
tris, EDTA (TE solution) and NaCl, TNE buffer is a buffer solution used in molecular biology, especially for DNA and RNA
Buffer Resist and Maintains the PH of the solution if there change in the environment of the solution.
Phosphate buffered saline is a buffer solution commonly used in biological research. It is a water-based salt solution containing sodium phosphate, sodium chloride and, in some formulations, potassium chloride and potassium phosphate. The osmolarity and ion concentrations of the solutions match those of the human body.
H2CO3 is not used as buffer.
donate H+ ions
A buffer solution is one involving a weak base/weak acid with its conjugate acid/base. In a buffer solution, the pH must be changed to only a small amount. Thus, any solution with a STRONG acid or a STRONG base is not a successful buffer solution because there would be a relatively large change in the initial pH.