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PubMed1996

Evaluation for antisperm antibodies after storage of sperm in TEST-yolk buffer.

OBJECTIVE: To determine if TEST-yolk buffer, consisting of TES (N-tris [hydroxymethyl]-methyl-2-aminoethanesufonic acid), Tris (Tris[hydroxymethyl]aninomethane), and chicken egg yolk, affects the presence of antisperm antibodies on the sperm surface as detected by the immunobead test. DESIGN: A prospective study of antisperm antibodies on sperm surface before and after incubation in TEST-yolk buffer. Direct immunobead test and indirect immunobead test were done the day of collection of the semen sample to detect the presence of human immunoglobulin class G (IgG) and immunoglobulin class A (IgA); immunobead tests were repeated on the same sperm samples after 24 hours of storage in TEST buffer. SETTING: Academic tertiary institution. PARTICIPANTS: Patients undergoing evaluation for infertility. RESULTS: There was no significant difference in the outcome of the direct immunobead test after extending semen samples with TEST-yolk buffer for 24 hours at 4 degrees C. Eleven samples that were initially negative for IgG and 13 samples that were negative for IgA remained negative after 24-hour storage in TEST-yolk buffer. Eleven samples that were positive for IgG and nine samples that were positive for IgA by the direct immunobead test the first day remained positive the next day. Five extended sperm samples used in the indirect immunobead test with IgG positive serum gave positive results and four of five used with IgA positive serum gave positive results. CONCLUSIONS: These findings suggest that TEST-yolk buffer can be used to extend semen without affecting the presence of antibodies on the sperm surface as indicated by the direct immunobead test. The higher variability of the indirect immunobead tests indicates there may be some alteration of sperm antigens after storing in TEST-yolk buffer. These findings indicate that TEST-yolk buffer can be used to store semen for batched processing of samples or as a transport medium for delivery to a central laboratory for antibody testing.

Antibodies↗
PubMed2001

Effect of buffer concentration on gradient chromatofocusing performance separating protiens on a high-performance DEAE column.

Gradient chromatofocusing is a recently developed chromatographic technique that overcomes the limitations of conventional chromatofocusing. This technique employs a HPLC gradient system and simple low-molecular-mass buffer components to generate linear or other function pH gradients on ion-exchange columns. Results of the present work show a superior separation of beta-lactoglobulin A and B in gradient chromatofocusing compared to salt gradient chromatography using the same DEAE column, with an optimized resolution of 2.3 obtained with gradient chromatofocusing compared to 1.1 obtained with NaCl gradients at constant pH. A significant advantage of the gradient chromatofocusing technique over the conventional chromatofocusing technique is its ability to employ a relatively wide range of buffer concentrations in the mobile phase, the effect of which is studied in the present work. Five proteins (conalbumin, ovalbumin, bovine serum albumin, beta-lactoglobulin A and B) are chromatographed on a DEAE-polymethacrylate HPLC anion-exchange column using the same approximately linear pH gradient profile but different mobile phase buffer concentrations. Results show a significant effect of buffer concentration on peak width, separation factor and resolution. For example, resolution increases from 1.5 to 2.3 in the separation of beta-lactoglobulin A and B when the concentration of each of the components in the 100% elution buffer is increased from 6.25 to 25.0 mM (with the same outlet pH gradient). This separation trend is also seen in the chromatography of ovalbumin from a commercial source, noting a progressive increase in resolution of two peaks in the sample (resolution increased from 0.7 to 2.4) when the concentration of each of the components in the 100% elution buffer is increased from 6.25 to 37.5 mM (same outlet pH gradient). The gains in the resolution are attributed to an increase in the separation factor, since the peak widths are generally noted to also increase with increased buffer concentration. These results point to a significant interplay between buffer concentration and pH, which is not effectively exploited in either conventional chromatofocusing or in conventional ion-exchange chromatographic procedures employing salt gradient elution at constant pH. Gradient chromatofocusing has the ability of optimizing both parameters, thus providing it with unique capabilities in protein separations.

Buffers↗
PubMed2002

Electroosmotic flow variations caused by the volatility of buffer components: diagnosis and therapy.

In order to separate a polar amine pharmaceutical and its potential impurities, a micellar electrokinetic chromatography method was developed. The main compound and 11 other substances were completely separated using a 20 mM Tris buffer, pH 8.0, containing 50 mM sodium dodecylsulfate (SDS) and 24% (v/v) acetonitrile. However, a strong, continuous reduction in the EOF occurred and quantification was not possible. The EOF reproducibility could not be improved by suitable rinsing procedures. Surface effects or interactions did not cause the EOF changes, but the evaporation of acetonitrile was identified as the major source for EOF instability. However, a high concentration of acetonitrile was decisive for selectivity. Thus a reliable protection against the evaporation of this buffer constituent had to be found. Paraffin and various silicon oils were tested as covering film. In order to quickly test buffer systems if the evaporation of electrophoresis solutions is acceptable, an alternative experimental design without doing CE experiments had to be found. Electrical conductivity was chosen as parameter, because it can be determined simply and fast. The buffers under investigation were placed in a 50-ml beaker with a magnetic stirring rod, placed on a magnetic stirrer. The buffer solution was kept in motion at 120 rev./min. The beaker was covered around the measuring head with laboratory film and in addition to this with paraffin or silicon oil. An acetonitrile content up to 10% (v/v) was acceptable if a coverage was used. The various cover liquids had a similar effect. A content of 15% (v/v) already increased the evaporation effect significantly. Higher acetonitrile contents are not acceptable. A buffer similar to the originally transferred method, 20 mM Tris (pH 8.0), 50 mM SDS containing 10% (v/v) acetonitrile as well as 10% (v/v) isopropanol showed an acceptably low evaporation in the conductivity experiments. With this buffer, a stable EOF was also obtained. Conductivity measurements are generally applicable to quickly test buffers that contain organic solvents.

Buffers↗
PubMed1999

General experimental aspects of the use of isoelectric buffers in capillary electrophoresis.

Four acidic, isoelectric buffers, for peptide and protein separations, have been recently described and adopted in capillary zone electrophoresis: cysteic acid [Cys-A, isoelectric point (pI) 1.85], iminodiacetic acid (IDA, pI 2.23), aspartic acid (Asp, pI 2.77) and glutamic acid (Glu, pI 3.22). These four buffers allow to explore an acidic portion of the titration curves of macroions, covering about 1.6 pH units (from pH 1.85 to ca. 3.45), thus permitting resolution of compounds having coincident titration curves at a given pH value. Given the rather acidic pI values of these buffers, their long-term stability has been investigated, by monitoring pH and conductivity changes upon increasing storage times. When dissolved in plain water, all four buffers appear to give constant pH and conductivity readings up to 15 days; after that, the conductivity keeps steadily increasing in a similar fashion. The same parameters, when the same buffers are dissolved in 6 M urea, appear to be stable for only one week, with the conductivity progressively augmenting after this period. A similar behaviour is exhibited by histidine (pI 7.70), a neutral, isoelectric buffer adopted for separation of DNA fragments. By mass spectrometry, Cys-A shows minute amounts (ca. 1%) of a degradation product after ageing for 3 weeks; in the same time period, Glu is extensively degraded (20%). No degradation species could be detected in IDA and Asp solutions. It is additionally shown that the acidic buffers are not quite stationary in the electric field, but can be transported at progressively higher rates (according to the pI value) from the cathodic to the anodic vessel. This is due to the fact that, at their respective pI values, a fraction of the amphotere has to be negatively charged in order to provide counterions to the excess of protons due to bulk water dissociation. Guidelines are given for the proper use and storage of such buffers.

Buffers↗
PubMed1988

Pain reduction in local anesthetic administration through pH buffering.

The effects of pH buffering on the pain of administration and efficacy of three local anesthetics (1% lidocaine, 1% lidocaine with 1:100,000 epinephrine, and 1% mepivacaine) were investigated in a randomized, prospective, double-blind study of 25 adult volunteers. Plain and buffered solutions of the three local anesthetics were prepared, and a 0.5 intradermal injection of each was administered. Pain of anesthetic infiltration was rated from zero to ten. The area of anesthetized skin surrounding each injection site was measured at time intervals following each injection. Buffering the local anesthetics significantly reduced the mean quantitative pain estimates compared to the nonbuffered controls: 1) 1% lidocaine compared with buffered 1% lidocaine, 4.9 +/- 0.4 versus 1.1 +/- 0.2 (P less than 10(-6)); 2) 1% lidocaine with epinephrine compared with buffered 1% lidocaine with epinephrine, 5.1 +/- 0.4 versus 1.8 +/- 0.4 (P less than 10(-6)); and 3) 1% mepivacaine compared with buffered 1% mepivacaine, 5.1 +/- 0.4 versus 0.9 +/- 0.2 (P less than 10(-6)). Onset, extent, and duration of skin anesthesia were not statistically altered by pH buffering. The pain of local anesthetic administration can be dramatically reduced by buffering the local anesthetic prior to its infiltration. Anesthetic efficacy is not compromised, and patient acceptance may be significantly increased.

Adult↗
PubMed1998

Alteration of redox stability of hemoglobins A and S by biological buffers.

Several organic and inorganic buffers, including Hepes, Tris and potassium phosphate, are often used for the maintenance of pH in hemoglobin solution work. It has often been assumed these buffers do not significantly affect the solution stability of these proteins. This investigation has focused on the effect these buffers have on the redox stability of the heme-iron, [Fe+2-->Fe+3], of hemoglobins A and sickle cell S (beta 6 glu-->val) over extended periods of time. Initial results indicate that: 1) the use of different buffers under similar ionic strength conditions at pH 7.0 affect conformational changes that produce substantial differences in redox stability between Hb A and Hb S; 2) spectral analysis of these hemoglobins in the visible region (700-500 nm) at 37 degrees C for extended periods of time indicated that a slower rate of autoxidation is observed with a Hepes buffered system over a wide ionic strength range than for either Tris or potassium phosphate buffers; 3) Hb S autoxidized at a faster rate in the presence of each of these buffers than Hb A; and 4) in contrast to Hb A, Hb S showed extensive hemichrome formation after 15 hr in the presence of potassium phosphate buffer.

Buffers↗
PubMed2000

An investigation into the release of cefuroxime axetil from taste-masked stearic acid microspheres. III. The use of DSC and HSDSC as means of characterising the interaction of the microspheres with buffered media.

Stearic acid coated cefuroxime axetil (SACA) microspheres have been studied using differential scanning calorimetry (DSC) and high sensitivity DSC (HSDSC) in order to examine the interaction between the spheres and a range of buffer systems, with a view to further enhance the understanding of the mechanism of drug release developed in earlier studies [Robson et al., 1999, 2000]. DSC studies indicated that after immersion in Sorensens modified phosphate buffer (SMPB) pH 5.9 followed by washing and drying, no change in the thermal properties of the spheres was detected up to 60 min of immersion, with a single endotherm noted at circa 56 degrees C, that corresponded to the melting of the stearic acid used in this study; similar results were obtained for systems immersed in distilled water. After immersion in SMPB pH 7.0 and 8.0, however, a second peak was noted at approximately 67 degrees C that increased in magnitude relative to the lower temperature endotherm with increasing exposure time to the medium. Spheres that had not been previously washed prior to drying showed complete conversion to the higher temperature endotherm for these two buffers. Systems which had been exposed to a range of pH 7.0 buffers (citrate-phosphate buffer (CPB), phosphate buffer mixed (PBM), boric acid buffer (BAB)) were then examined. Only the CPB systems showed evidence for conversion to the higher melting form. PBM systems to which further sodium had been added were then examined. A maximum conversion was found at 0.05 M sodium, which was in agreement with the maximum in release rate found in a previous study [Robson et al., 2000]. HSDSC was then used to examine systems that were immersed in the buffer. For SMPB, pH 5.9 and distilled water, only the endotherm corresponding to the stearic acid melting was seen. However, for SMPB pH 7.0 and 8.0, three peaks were seen, two corresponding to those seen for the DSC studies and a further lower temperature peak at circa 44 degrees C. Studies on PBM systems to which additional sodium had been added showed small levels of conversion to the higher temperature form at higher sodium contents. The data was discussed in terms of the correlation with earlier dissolution studies on the same systems [Robson et al., 1999; 2000].

Buffers↗
PubMed1997

Comparison of wound infection rates using plain versus buffered lidocaine for anesthesia of traumatic wounds.

Buffered lidocaine has been shown to be less painful than plain lidocaine for anesthetizing wounds. However, the effect of a buffering agent on the local host defenses has not been evaluated. The infection rates of wounds anesthetized with plain lidocaine versus buffered lidocaine were compared in an observational cohort study. Consecutive emergency department patients with traumatic wounds that required sutures had a closed-question wound registry sheet prospectively completed. Follow-up data were obtained at the time of the return visit. Patients failing to return were contacted by telephone. Data were analyzed for wound infection rates comparing plain lidocaine with buffered lidocaine. Chi-squared or Fisher exact tests were used for statistical analysis. Of 2,711 patients analyzed, 2,279 had received plain and 432 had received buffered lidocaine. The infection rate for patients treated with plain lidocaine was 3.5%, versus that for patients treated with buffered lidocaine, 3.9% (P = .63). After adjustment for confounding variables, the infection rate did not differ between plain and buffered lidocaine. The infection rates of wounds repaired after anesthesia with either plain or buffered lidocaine are similar.

Adult↗
PubMed2002

Thermophysical properties of pharmaceutically compatible buffers at sub-zero temperatures: implications for freeze-drying.

PURPOSE: To evaluate crystallization behavior and collapse temperature (Tg') of buffers in the frozen state, in view of its importance in the development of lyophilized formulations. METHODS: Sodium tartrate, sodium malate, potassium citrate, and sodium citrate buffers were prepared with a pH range within their individual buffering capacities. Crystallization and the Tg' were detected during heating of the frozen solutions using standard DSC and modulated DSC. RESULTS: Citrate and malate did not exhibit crystallization, while succinate and tartrate crystallized during heating of the frozen solutions. The citrate buffer had a higher Tg' than malate and tartrate buffers at the same pH. Tg' vs. pH graphs for citrate and malate buffers studied had a similar shape, with a maximum in Tg' at pH ranging from 3 to 4. The Tg' maximum was explained as a result of a competition between two opposing trends: an increase in the viscosity of the amorphous phase because of an increase in electrostatic interaction, and a decrease in the Tg' because of an increase in a water concentration of the freeze-concentrated solution. CONCLUSION: Citrate buffer was identified as the preferred buffer for lyophilized pharmaceuticals because of its higher Tg' and a lower crystallization tendency.

Buffers↗
PubMed2003

Use of a physiologic bicarbonate buffer system for dissolution characterization of ionizable drugs.

PURPOSE: The aim of this study was to examine if sparging with CO2(g) could be used to establish stable biorelevant bicarbonate buffers, in aqueous medium, for use in dissolution characterization of low-solubility ionizable drugs. METHODS: Preparation of the bicarbonate-containing dissolution medium was monitored by use of a commercially available fiberoptic probe to measure the concentration of dissolved CO2(aq). Intrinsic dissolution measurements at 100 rpm, 37 degrees C for indomethacin and dipyridamole were performed using a rotating disk and UV detection at pH 6.8 and 5.0 in a USP dissolution vessel apparatus. RESULTS: Indomethacin dissolution at pH 6.8 was significantly impacted by the concentration of CO2(g) in the sparging gas. Dipyridamole flux at pH 6.8 was independent of buffer species or buffer concentrations studied. However, dipyridamole dissolution at pH 5 was also a strong function of the concentration of CO2(g) in the sparging gas. CONCLUSIONS: Stable bicarbonate biorelevant buffers could be established to perform intrinsic dissolution rate determinations for indomethacin and dipyridamole as long a continuous gas sparging of CO2(g) was used. Depending of the pH of the dissolution medium, the intrinsic dissolution rates of both indomethacin and dipyridamole were affected by the bicarbonate concentration. Sparging with CO2(g) to create physiologic buffers has a unique advantage over conventional buffers in that gas sparging serves as a continuous source of bicarbonate buffer species. This advantage was demonstrated by performing dissolution experiments at pH values typically associated with the fed state (pH 5) and applying relatively low CO2(g) pressures, resulting in bicarbonate concentrations less than 0.5 mM. It was demonstrated that CO2(g) sparging at a pH consistent with the fed state created an in-situ bicarbonate buffer at low concentrations, which had a significant impact on the dissolution of a basic drug such as dipyridamole.

Bicarbonates↗
PubMed1991

Intracellular H+ buffering power and its dependency on intracellular pH.

Intracellular hydrogen ion (H+) buffering power, conventionally defined as the amount of acid or base that would have to be introduced into the cell cytosol to decrease or increase ipH by one pH unit, is generally said to increase as intracellular pH (ipH) decreases. This implies that the cell has a lesser capability to resist acute acid or base perturbations at its steady state ipH than at any lower ipH. We re-examined this notion, reasoning that the logarithmic nature of the pH unit could limit the validity of the conventional expression of buffering power in imparting physiologic insight into the mechanisms of cellular H+ homeostasis. The mathematical derivation of the formula, delta i[NH4+]/delta ipH, conventionally used to estimate buffering power using the NH4Cl technique, revealed that this parameter is, by design, inversely proportional to the exponential of ipH. This a priori dependence on pH dictates an increase in buffering power with decreasing ipH, and thereby interferes with the assessment of the physiologic capability of the intracellular milieu to buffer protons at different ipH levels. To circumvent this problem, buffering power was defined as the amount of hydrogen ions that would have to be added to or removed from the cell to effect a change in the concentration of H+ in the cell cytosol of 1 mM (a term heretofore referred to as the cell H+ buffering coefficient). The mathematical derivation of the formula used to calculate the cell H+ buffering coefficient, delta i[NH4+]/delta[H+]i, does not suffer from an a priori dependence on ipH.(ABSTRACT TRUNCATED AT 250 WORDS)

Acid-Base Equilibrium↗
PubMed1997

Increased ELISA sensitivity using a modified extraction buffer for detection of Xanthomonas campestris pv. vesicatoria in leaf tissue.

In vitro and in planta sensitivity of an indirect enzyme-linked immunoassay technique, using a monoclonal antibody specific for the lipopolysaccharide (LPS) of Xanthomonas campestris pv. vesicatoria, was increased 10-fold by using a new extraction buffer (gl of: KH2PO4, 2; NaHPO4, 11.5; EDTA disodium, 0.14; thimerosal, 0.02; and lysozyme, 0.2). The procedure improved sensitivity without increasing background levels. In vitro, the limit of detection was between 1 x 10(7) and 1 x 10(8) cells ml-1 with the conventional extraction buffer phosphate-buffered saline (PBS) and less than 1 x 10(6) cells ml-1 when lysozyme extraction buffer was substituted for PBS. In comparing 22 X. c. vesicatoria strains, absorbance readings were increased close to three-fold with the lysozyme extraction buffer as opposed to PBS. When leaf tissue extract was spiked with the bacterium, the limit of detection was 1 x 10(7) cfu ml-1 and 1 x 10(8) cfu ml-1 with the lysozyme solution and PBS, respectively, as the extraction buffers. When using the lysozyme extraction buffer in combination with a commercial amplification system, the limit of detection was decreased to less than 1 x 10(5) cfu ml-1 in leaf tissue. The addition of the lysozyme and EDTA to the phosphate buffer resulted in release of a significant quantity of LPS and concomitant dramatic increase in sensitivity. The new procedure, termed lysozyme ELISA (L-ELISA), should increase sensitivity of ELISA reactions where LPS is the reacting epitope.

Antigens, Bacterial↗
PubMed1999

Volatile buffers can override the "pH memory" of subtilisin catalysis in organic media.

The protonation state and activity of enzymes in low-water media are affected by the aqueous pH before drying ("pH memory"). However, both protonation and activity will change if buffer ions can be removed as volatile or organic-extractable weak acids or bases. With NH4OOCH buffers, in which both ions can be removed, pH memory disappears completely for subtilisin-catalyzed transesterification in hexane. Only weak pH memory is found with buffers having one volatile component, NH4-phosphate and NaOOCH. The changes in ionization state result from proton exchanges like Protein-COO-NH4+ --> Protein-COOH + NH3 (g) and Protein-NH3+HCOO- --> Protein-NH2 + HOOCH (g). An equivalent, complementary picture is that net charges on the protein and buffer ions must remain equal and opposite. With NaOOCH buffers, loss of some HCOO- ions gives a more negative net charge on the protein, balanced by the excess Na+. With NH4-phosphate buffers, loss of NH3 gives protein with a more positive net charge. The resulting catalytic activities were high and low, respectively, similar to those after drying from Na-phosphate buffers of optimal (8.5) and acid pH. All of the above effects have been demonstrated for both covalently immobilized subtilisin and the lyophilized free enzyme. Subtilisin lyophilized from NH4OOCH buffers gave pH approximately 4 after redissolution in water, probably because removal of HCOO- counterions remains incomplete. The resulting catalytic activity was low. The effects are discussed in relation to the possible locations, in low-dielectric media, of the positive charge that balances the net negative catalytic triad in active subtilisin.

Animals↗
PubMed1990

Effect of buffer systems and pHi on the measurement of [Ca2+]i with fura 2.

The fluorescent probe, fura 2, is widely used to measure agonist-induced changes in intracellular calcium concentration ([Ca2+]i) in cultured cells. However, in many instances, the results obtained in the same cell type have differed from one study to the next. The possibility that such differences might be due to experimental conditions was examined by using fura 2 in four different cell types responding to appropriate agonists when the cells were incubated in either CO2/HCO3-- or HEPES-buffered media. Examined were: 1) the response of rat glomerular mesangial cells to arginine vasopressin, 2) the response of vascular smooth muscle cells to angiotensin II, 3) the response of adrenal glomerulosa cells to angiotensin II, and 4) the response of hypothalamic cells to insulin-like growth factor-1. In each cell type there was a significant difference in the pattern of agonist-induced change in [Ca2+]i when HEPES vs. CO2/HCO3- was used as the buffer system: in HEPES buffer, agonist addition led to a transient rise in [Ca2+]i followed by a fall to a sustained plateau 27 to 34 nM higher than the original basal value, whereas in CO2/HCO3- buffer, agonist addition led to an identical transient increase in [Ca2+]i followed by a fall to a value within 10 nM or less of the preagonist level. The plateau value of [Ca2+]i in the different buffers was examined in relationship to known differences in intracellular pH (pHi). It was found that measurements of [Ca2+]i with fura 2 were influenced by shifts in pHi that occur when cells are incubated in either HEPES-buffered or CO2/HCO3- media of differing pHo values. However, at any given value of pHi, the apparent [Ca2+]i measured in cells incubated in HEPES-buffered media was slightly higher than in cells incubated in CO2/HCO3- buffered media.

Adrenal Medulla↗
PubMed1989

Effects of lead salts on the uptake, release, and binding of gamma-aminobutyric acid: the importance of buffer composition.

The effects of lead on the uptake and release of gamma-[3H]aminobutyric acid [( 3H]GABA) from rat brain slices were examined in solutions buffered with Tris-HCl, sodium phosphate, and sodium bicarbonate. Lead acetate (10-250 microM) inhibited uptake and potassium-stimulated release and facilitated spontaneous efflux only in solutions buffered with Tris-HCl. Calcium-independent binding of [3H]GABA was unaffected by lead acetate (1-100 microM) in Tris-citrate buffer but was significantly inhibited by 3 microM lead acetate in Tris-HCl solution. At the rat soleus neuromuscular junction, lead caused a dose-dependent reduction of end-plate potential amplitude at concentrations of 10-100 microM lead acetate in HEPES-buffered solution but had no effect at these concentrations in phosphate-buffered solution. Stability constants of lead complexes indicate that buffers containing carbonate and phosphate are unlikely to contain a significant concentration of Pb2+, as complexing by these anions would reduce the availability of free Pb2+. This study indicates that the choice of buffer is important when investigating the effects of lead on biological systems and that negative findings may result from the use of inappropriate buffers. It also has important clinical implications suggesting that some effects of lead poisoning may result from its ability to affect neurotransmitter systems directly and that local changes in pH and complexing anion concentrations in the CNS may influence its biological availability and, hence, variable biological responses.

Animals↗
PubMed1986

A new framework for assessment of potassium-buffering mechanisms.

A new concept, that of "buffer capacity," is defined for potassium-buffering mechanisms in neural tissue. Buffer capacities for different mechanisms can be added and compared, thus simplifying quantitative assessment of diffusion, cytoplasmic uptake, and spatial buffering under varied conditions. The characteristic frequency components for potassium disturbances due to neural events are identified. The effect of buffering by a reservoir of fluid at a tissue surface is analyzed, together with its intrinsic limitations. The role of retinal Müller cells in spatial buffering is considered quantitatively: both buffering to the tissue surface and buffering sideways through cell-to-cell connections.

Animals↗
PubMed2006

The pH change after HCl titration into resting and stimulated saliva for a buffering capacity test.

BACKGROUND: Saliva collection can provide clinical information about individual patients. However, a correlation between ranking buffering capacity using resting and stimulated saliva is still unknown. The aim of this study was to evaluate the pH change after HCl titration into resting and stimulated saliva for a salivary buffering capacity test. METHODS: Resting and stimulated saliva (by chewing paraffin wax) were collected from 80 patients. After the pH of both saliva samples was measured using a hand-held pH meter, the saliva samples were titrated with 0.1N HCl to evaluate the buffering capacity. Correlations of ranking buffering capacity (high, medium, low) between stimulated saliva and resting saliva with 30 microL HCl titration and between stimulated saliva and resting saliva with 40 microL HCl titration were statistically analysed by Spearman Rank Correlation Test (p < 0.05). RESULTS: At 50 microL HCl titration, stimulated saliva buffering capacities were ranked into high (above pH 5.5), medium (pH from 5.5 to 4.5) and low (below pH 4.5). At 30-40 microL HCl titration, the resting saliva buffering capacities were ranked into the same categories. Spearman Rank Correlation indicated significant positive coefficients for the stimulated saliva and resting saliva buffering capacity at 30 microL titration and the stimulated saliva and resting saliva at 40 microL titration. CONCLUSION: Stimulated saliva is more resistant to variation in pH change during HCI titration than resting saliva. Stimulated saliva sampling is a good method to determine buffering capacity during a comprehensive oral health assessment.

Adolescent↗
PubMed1979

Viral aggregation: buffer effects in the aggregation of poliovirus and reovirus at low and high pH.

The effects of the buffer employed in maintaining a given pH value were tested on the aggregation of two viruses, poliovirus and reovirus. Poliovirus was found to aggregate at pH values of 6 and below, but not at pH 7 or above, except in borate buffer. Reovirus aggregated at pH 4 and below, but was found to aggregate only in acetate or tris(hydroxymethyl)aminomethane-citrate buffers at pH 5. Other buffers tested for aggregation of reovirus at pH 5 (succinate, citrate, and phosphate-citrate) induced little aggregation. No significant aggregation was found for reovirus at pH 6 and above. For both viruses, the most effective aggregation was induced by buffers having a substantial monovalently charged anionic component, such as acetate at pH 5 and 6 or citrate at pH 3. Cationic buffers at low pH, such as glycine, were generally weaker in aggregating ability than anionic buffers at the same pH. These results, when correlated with the isoelectric point of the viruses (poliovirus at pH 8.2; reovirus at pH 3.9) indicated that both viruses aggregated strongly when their overall charge was positive, but only under certain circumstances when their overall charge was negative. Although reovirus aggregated massively at its isoelectric point, poliovirus remained dispersed at its isoelectric point. The conclusion can be drawn that those pH and buffer conditions which induced aggregation of one virus do not necessarily induce it in another.

Acetates↗