Consider a biochemical reaction that is taking place in a 0.1 M buffer. The initial pH is 7.4, and the pKa of the buffer is 7.2. If, in a final reaction volume of 1.0 mL, 10 micromol of protons are generated, what would be the final pH of the solution?

The pH of the solution is 7,22

Explanation:

Using the Henderson–Hasselbalch equation we can find the pH of the solution.

First, we need to find the concentrations of [A-] and [HA]

Now we apply the antilogarithm function to both sides of the equation

using the previous equation and the ratio [A-] + [HA] = 0.1 we proceed to apply a system of equations to find the values of [HA] and [A-].

after solving the system of equations

[A-]=0,0613

[HA]= 0,0387

After the 10 micromol of protons are generated the protons will reduce [A-]  and increase [HA].

[H+] =

[H+] = 0,01M

now, the new value of pH is

3 1/4 %

explanation:

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.