Answer: I don't know if this helps you or not, but this is from study.com:
I'm so sorry if it doesn't:
Explanation: Iron(III) oxide reacts with carbon monoxide according to the balanced equation:
Fe₂O₃ + 3CO ➡️ 2Fe + 3CO₂
A reaction mixture initially contains 23.00g Fe₂O₃ and 15.40g CO.
<span>H2CO3 <---> H+ + HCO3-
NaHCO3 <---> Na+ + HCO3-
When acid is added in the buffer, the excess H+ of that acid reacts with HCO3- to form H2CO3, and due to this NaHCO3 dissociates into HCO3- to attain the equilibrium. and hence there is no net effect of H+ due to pH remain almost constant.
when a base is added to the buffer, the OH- ion of base react eith H+ ion present in buffer, then to attain equilibrium of H+ ion, the H2CO3 dissociates to produce H+ ion, but now there is the excess of HCO3- due to which Na+ ion react with them to attain equilibrium of HCO3-. hence there is again no net change in H+ ion due to which pH remain constant.....</span>
