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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Fantarics on September 09, 2019, 10:08:14 PM

Title: Lab on the corrosion process.
Post by: Fantarics on September 09, 2019, 10:08:14 PM

Steel mesh is placed into different beakers with different solutions in them ranging from 1 to 14 pH. The trend of the amount of the reacted Iron (doesn't mean ONLY iron which turned into rust) has the shape of the letter W. Peaks are at 1 pH, 7 pH and 14 pH. I read that the corrosion rate of the Iron decreases as the pH increases. So, here is the question. What happens to the Iron in the pH 7 and pH 14 solutions so that they actually go up (the amount of reacted Iron increases)?

Title: Re: Lab on the corrosion process.
Post by: chenbeier on September 10, 2019, 06:43:57 AM

In Low pH Fe is solouble, in high pH ironoxide-hydroxide is formed and it is not solouble and it protects the Iron below för longer Time.

Title: Re: Lab on the corrosion process.
Post by: Fantarics on September 10, 2019, 02:36:03 PM

Quote from: chenbeier on September 10, 2019, 06:43:57 AM

In Low pH Fe is solouble, in high pH ironoxide-hydroxide is formed and it is not solouble and it protects the Iron below för longer Time.

Yeah, that's right. But the data I collected during the lab shows that there was about the same amount of the reacted iron as it was in the acid. Why is that so?