Buffer solutions

Use of buffer solutions

Buffer solutions play an important role in chemistry. An example is the precipitation of aluminum hydroxide at a constant as possible $\text{pH}$Value of 9, otherwise OH in the course of the precipitation⁻-Ions are consumed from the solution and with decreasing $\text{pH}$ the solubility of Al (OH)₃ increases again. One could compensate for the loss of hydroxide ions in the solution by adding caustic soda, but would then have to do this several times $\text{pH}$-Check the value. It is easier to find the one you want $\text{pH}$- Stabilize the value by buffering.

For complexometric titrations with Na₂EDTA releases protons in the course of complex formation; by the sinking $\text{pH}$Value would affect the stability of the complex. That is why one also works here in a buffered solution. Buffers are extremely important for the course of biochemical reactions. This is how human blood has one $\text{pH}$-Value from 7.35 to 7.45. Greater deviations are life-threatening. Since lactic acid is produced primarily during muscle work, there is a risk of over-acidification in unbuffered blood. (The main buffer systems in the blood are CO₂/ HCO₃⁻ and buffering the amphoteric serum proteins.)