The buffer solution target has a pH value smaller than that of pKw (i.e., pH < 7.) The solution is therefore acidic. It contains significantly more protons than hydroxide ions . The equilibrium equation shall thus contain protons rather than a combination of water and hydroxide ions as the reacting species.
Assuming that of the 0.307 sodium hydroxide solution was added to the acetic acid. Based on previous reasoning, is sufficiently small that acetic acid was in excess, and no hydroxide ion has yet been produced in the solution. The solution would thus contain moles of acetic acid and moles of acetate ions.
Let denotes an acetic acid molecule and denotes an acetate ion. The RICE table below resembles the hydrolysis equilibrium going on within the buffer solution.
The buffer shall have a pH of 4.250, meaning that it shall have an equilibrium proton concentration of . There were no proton in the buffer solution before the hydrolysis of acetic acid. Therefore the table shall have an increase of in proton concentration in the third row. Atoms conserve. Thus the concentration increase of protons by would correspond to a decrease in acetic acid concentration and an increase in acetate ion concentration by the same amount. That is:
By definition:
The question states that
such that
Thus it takes of sodium hydroxide to produce this buffer solution.
The molecule CO2 have 2 lone pairs located in the oxygen atoms. It has two double bonds also connecting carbon atom to the two oxygen atoms. It does obey the octet rule so the atoms need 8 electrons in each of them that is why electrons are shared.
The hydrostatic pressure is defined as the pressure that is exerted by a fluid at equilibrium at a given point within the fluid, due to the force of gravity, the formula is: