At a pH of 11.3, which chemical dominates the water composition?

At a pH of 11.3, the water is quite alkaline, indicating a higher concentration of hydroxide ions. In this pH range, the dissociation of water and the equilibrium between various forms of carbonate species are important to consider.

At higher pH levels, hydroxide ions become increasingly dominant in the water chemistry. While carbonates and bicarbonates are also present, they tend to convert into especially hydroxide ions due to the elevated alkalinity. Specifically, at this pH, the concentration of hydroxide ions surpasses that of carbonic species, leading to the conclusion that hydroxide is the predominant form in the solution.

Understanding this behavior of water chemistry is crucial, as it helps in the assessment of water treatment processes and the management of water quality. In a more acidic environment, bicarbonate and carbon dioxide may play more significant roles, but at pH 11.3, the chemical balance clearly shifts towards the dominance of hydroxide ions.