Change of the point of zero net proton charge (pHPZNPC) of clay minerals with ionic strength

Abstract

In a system where protons and hydroxide ions are the only aqueous species, the point of zero net proton charge (pHPZNPC) of a mineral defines the pH at which the positively and negatively charged functional groups on its surface are equal (Drever, 1997). Ascertaining the pHPZNPC of clay minerals, a ubiquitous component in soils, sediment and rivers, is useful in predicting its electrostatic interactions with charged aqueous species, colloids, and bacteria. While the pHPZNPC values of most clays have been reported, the variation of pHPZNPC with changing solution ionic strength (IS) and the mathematic relationship between them are not well-understood but critical in assessing the surface reactivity of clays in aqueous solutions ranging from freshwater to brines. To address this gap, we studied the relationship of the pHPZNPC of three clay minerals (kaolinite, illite, and montmorillonite) at seven ionic strengths (from 0.001 to 0.1 M). Titration data for each clay were used to calculate the pHPZNPC by two methods previously documented in literature: (1) using the difference between the blank titration and clay titrations, and (2) by the difference between the number of protons added during titration and the number of protons remaining in solution. The results show that: (1) unlike simple metal oxides (e.g., hematite, gibbsite, quartz), titration curves of clay minerals at different IS do not intersect at a common pHPZNPC value; (2) the pHPZNPC for kaolinite is around 5.6 to 6.6 while the pHPZNPC for illite and montmorillonite is in the range of 9 to10; (3) the pHPZNPC value decreases systematically with increasing IS for all three clay minerals studied; and (4) the change of pHPZNPC is linear with log(IS). A third method using surface complexation modeling (SCM) approach was applied to calculate the pHPZNPC of the clay minerals, and the results match well with Method 2. Our results allow for a more accurate estimation of clay surface charge property in aqueous environment, which, in turn, will improve model predictions of the adsorption of charged species in systems in which ionic strength changes.

The kaolinite shuttle links the Great Oxidation and Lomagundi events

“…2 ). However, the surface charge of kaolinite is pH-dependent 48 , 49 . Surface complexation modeling based on acid-base titrations of kaolinite shows that kaolinite surface functional groups are highly protonated at pH < 4.7, lending the clay a net positive charge (supplementary note 4), which can electrostatically attract negatively charged P species (dominantly H 2 PO 4 − at pH 2–7).…”

Trace Elemental Partitioning on Clays Derived From Hydrothermal Muds of the El Tatio Geyser Field, Chile

“…Surface complexation modeling (SCM) was used to model the protonation‐deprotonation behavior of functional groups on the surfaces of minerals in mud samples as a function of solution pH. Since the mud samples are mostly composed of clay minerals, we applied the same model for protonation and deprotonation surface reactions as used in previous clay studies (Barbier et al., 2000; Hao et al., 2018; Hao, Flynn, et al., 2019; Ikhsan et al., 2005; Lackovic et al., 2003; Peacock & Sherman, 2005). The following surface complexation reactions and corresponding mass action equations were used: …”

The influence of invertebrate faecal material on compositional heterogeneity, diagenesis and trace metal distribution in the Ogeechee River estuary, Georgia, USA

“…This global biological phenomenon has the effect of decreasing the grain size of surrounding sediments via the production of authigenic clay minerals, as is evident in the Ogeechee River estuary. Clays have a strong affinity to bind trace metals from aqueous solutions (Schroth & Sposito, 1998; Arda et al ., 2006; Liu et al ., 2018; Hao et al ., 2018). Indeed, D. cuprea and C. major faecal material at both Raccoon Key and Steamboat Pass were enriched in trace metals (notably As, Co, Mo and Pb) in comparison to the adjacent sand matrix (Table 1).…”