In an alkaline solution with a high Na* concentration, a glass pH electrode tend

Question

In an alkaline solution with a high Na* concentration, a glass pH electrode tends to indicate a pH that is lower than the actual pH. identical to the actual pH, higher than the actual pH. Why does this occur? 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 O 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. 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 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 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 glass electrode only responds to H^+ ions and not Na^+ ions. Therefore the apparent pH will be identical to the actual pH.

Explanation / Answer

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

This occurs because 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. This leads to an apparent pH that is lower than the actual pH.

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.