What is the ph of a buffer solution when the concentrations of both buffer components (the weak acid and its conjugate base) are equal? what happens to the ph when the buffer contains more of the weak acid than the conjugate base? more of the conjugate base than the weak acid?

Explanation:

Considering the Henderson- Hasselbalch equation for the calculation of the pH of the buffer solution as:

pH=pKa+log[base]/[acid]

When the the concentrations of both buffer components (the weak acid and its conjugate base) are equal:

[base] = [acid]

So, pH=pKa+log1 = pKa

pH is equal to pKa of weak acid of buffer system .

When buffer contains more of weak acid than conjugate base:

[base] < [acid]

log [base]/[acid] = Negative,

So,

When more of acid component is present, the pH is more acidic. (It decreases)

When buffer contains more of conjugate base than weak acid:

[base] > [acid]

log [base]/[acid] = Positive,

So,

When more of acid component is present, the pH is more acidic. (It increases)

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.