Water and Solute Permeability of Plant Cuticles: Measurement and ...
Water and Solute Permeability of Plant Cuticles: Measurement and ...
Water and Solute Permeability of Plant Cuticles: Measurement and ...
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68 4 <strong>Water</strong> <strong>Permeability</strong><br />
potentials were highest, but did not quite reach the Nernst potential <strong>of</strong> 17.8 mV,<br />
hence they were not perfectly permselective for cations. Under natural condition<br />
the pH at the surfaces <strong>of</strong> the cuticles will be lower, <strong>and</strong> exclusion <strong>of</strong> anions will<br />
be far from complete. This means that diffusion <strong>of</strong> salt can take place, <strong>and</strong> this<br />
has been confirmed experimentally. Self-diffusion <strong>of</strong> NaBr across Citrus MX membranes<br />
was studied at pH 3 <strong>and</strong> 8.5 at 25 ◦ C, <strong>and</strong> Na + <strong>and</strong> Br − permeances were<br />
calculated (Schönherr <strong>and</strong> Huber 1977). The concentration <strong>of</strong> NaBr <strong>and</strong> pH was the<br />
same on both sides <strong>of</strong> the membrane (4 × 10 −3 moll −1 ), which implies that there<br />
was no net driving force. Radio-labelled ions were used ( 24 Na + <strong>and</strong> 82 Br − ), <strong>and</strong><br />
the fluxes <strong>of</strong> the ions were not coupled <strong>and</strong> both ions could diffuse independently.<br />
At pH 3 the ratio <strong>of</strong> the permeances <strong>of</strong> Na + /Br − ranged from 0.58 to 0.69, showing<br />
that permeance for Br − was higher because the membranes carried a net positive<br />
charge <strong>and</strong> co-ion (Na + ) diffusion was reduced by relative Donnan exclusion. At pH<br />
8.5 the ratio <strong>of</strong> permeances ranged from 3.83 to 4.39, because the membranes were<br />
negatively charged <strong>and</strong> now Br − experienced Donnan exclusion. Thus, depending<br />
on pH, cuticles are either cation or anion exchangers. The nature <strong>and</strong> concentration<br />
<strong>of</strong> the fixed charges will be dealt with next.<br />
4.3 Ion Exchange Capacity<br />
The concentration <strong>of</strong> charges covalently bound to the polymer matrix can be determined<br />
by potentiometric titration, as can be done with soluble electrolytes. The<br />
main difference is the fact that it takes longer to obtain equilibrium, because ions<br />
must diffuse into the polymer matrix, where diffusion coefficients are much smaller<br />
than in water <strong>and</strong> mixing is absent. The progressive batch method can be employed<br />
(Schönherr <strong>and</strong> Bukovac 1973). Small amounts (200 mg) <strong>of</strong> isolated CM or MX<br />
are weighed into glass tubes, <strong>and</strong> a constant volume <strong>of</strong> degassed water or salt solutions<br />
are added. To determine cation exchange capacity, increasing amounts <strong>of</strong> base<br />
is added under a stream on nitrogen, the vessels are closed airtight <strong>and</strong> agitated at<br />
constant temperature (25◦C). After 1–4 days, equilibrium is obtained. The pH <strong>of</strong> an<br />
aliquot from the supernatant is determined under a stream <strong>of</strong> nitrogen. If pH deviates<br />
significantly from 7 the supernatant is titrated back to pH 7 with st<strong>and</strong>ard acid<br />
or base, to determine the amount <strong>of</strong> H + released or base that was not used up in<br />
ion exchange. The reaction is stoichiometric <strong>and</strong> the equilibrium condition can be<br />
written as<br />
RH+ NaOH ⇄ RNa+H + + OH − ,<br />
H + + OH − (4.4)<br />
⇄ H2O,<br />
where R − is the polyanion <strong>and</strong> barred quantities refer to the polymer phase. The<br />
exchange capacity at a given pH is calculated from the amount <strong>of</strong> base added, minus<br />
the amount <strong>of</strong> base left at equilibrium. If a solution <strong>of</strong> a neutral salt is added to the<br />
cuticle, some ion exchange takes place <strong>and</strong> the supernatant becomes acidic:<br />
RH + NaCl ⇄ RNa + H + + Cl − . (4.5)