In an alkaline solution with a high Na^+ concentration, a glass pH electrode ten

Question

In an alkaline solution with a high Na^+ concentration, a glass pH electrode tends to indicate a pH that is identical to the actual pH. higher than the actual pH. lower than the actual pH. Why does this occur? The Na^+ ions bind to the same exchange sites as the H^+ ions on the surface of the glass O electrode. The electrode responds to Na^+ as if H^+ is present, leading to an apparent pH that is lower than the actual pH. The Na^+ ions compete with the H^+ ions for the exchange sites on the surface of the glass electrode. This prevents some of the H+ ions from binding to the glass, leading to an apparent pH that is higher than the actual pH. The Na^+ ions bind to the same exchange sites as the H^+ ions on the surface of the glass electrode. The electrode responds to Na^+ as if H+ is present, leading to an apparent pH that is higher than the actual pH. The glass electrode only responds to H^+ ions and not Na^+ ions. Therefore the apparent pH will be identical to the actual pH. The Na^+ ions compete with the H^+ ions for the exchange sites on the surface of the glass electrode. This prevents some of the H^+ ions from binding to the glass, leading to an apparent pH that is lower than the actual pH. The Na^+ ions compete with the H^+ ions for the exchange sites on the surface of the glass electrode. Since both Na^+ and H^+ have the same charge, the glass electrode responds to both in the same way, resulting in an apparent pH that is identical to the actual pH.

Explanation / Answer

In an alkaline solution with high Na+ concentration, a glass pH electrode tends to indicate a pH that is lower than the actual pH.

The reason why this occurs is that the Na+ ions compete with the H+ ions for the exchange sites on the surface of the glass electrode. This prevents some of the H+ ions from binding to the glass, leading to an apparent pH that is lower than the actual pH.

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