How does the pH of the solution affect the formation of rust?

Question

Accepted Answer

Well in this problem, we are given the statement, increasing the ph of the solution will favor the conversion of iron to rest. Rest of the statement is true or false. So the formation of rust is due to the oxidation of iron metal two iron too, in the presence of oxygen and water. So our reduction half reaction would be the reduction of oxygen under acidic conditions to form water. So we can combine these two half reactions to get the overall reaction. The number of electrons that are being lost should equal those being gained. So we'll multiply the oxidation reaction by two and by doing that, then the number of electrons being lost will be equal to those gains. So those will cancel And then have two moles. Byron reacts with oxygen gas under acidic conditions. Give us two moles of iron too And two moles of water. So if we increase hydro nine concentration, Then according to principle, this will drive the reaction towards the formation of Iron two, which means that it will favor the conversion of iron to rust increasing hydro nines. Then means that we are going to have a lower ph so it will be more acidic and so decreasing the ph of the solution will favor the conversion of iron to rust increasing it will not. So this statement then is false. Thanks for watching. Hope that helps

How does the pH of the solution affect the formation of rust?

Verified Solution

Key Concepts

pH Scale

Rust Formation

Corrosion Mechanism