Aph 4 buffer solution is prepared by dissolving one mole of a weak acid ha (pka = 4.0) and one mole naa in 1 l of water. when the volume is increased to 10 l by adding distilled water, the ph of the resulting solution is closest to:

pH is closest to 4.0

Explanation:

According to Henderson-Hasselbalch equation for a buffer consist of an weak acid (HA) and it's conjugate base ()-

where and [HA] represents concentration (in molarity) of and HA respectively.

We know,

Number of moles of HA and remains same even after diluting the solution to 10 L.

So,

So,

Hence pH is closest to 4.0

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.

dynamic equilibrium is the answer.