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Sulfuric acid titration curve

Also appearing in Fig. 4-12 is the sulfuric acid titration curve obtained with the standard slurry. It should be noted that the sulfate concentration regions of temperature instability bracket the break in the pH curve and the region of temperature stability occurs between pH 6 and 7. [Pg.157]

The alkalinity is determined by titration of the sample with a standard acid (sulfuric or hydrochloric) to a definite pH. If the initial sample pH is >8.3, the titration curve has two inflection points reflecting the conversion of carbonate ion to bicarbonate ion and finally to carbonic acid (H2CO2). A sample with an initial pH <8.3 only exhibits one inflection point corresponding to conversion of bicarbonate to carbonic acid. Since most natural-water alkalinity is governed by the carbonate—bicarbonate ion equiUbria, the alkalinity titration is often used to estimate their concentrations. [Pg.230]

Principle. By means of potentiometric titration (in nonaqueous media) of a blend of sulfonic and sulfuric acids, it is possible to split the neutralization points corresponding to the first proton of sulfuric acid plus that of sulfonic acid, and to the second proton of sulfuric acid. The first derivate of the titration curve allows identification of the second points the corresponding difference in the volume of titrating agent is used as a starting point in the calculation method (Fig. 4). [Pg.678]

By recognizing species in solution and their dominant equilibrium, we can construct titration curves for other diprotic acids. Example shows how this is done for sulfurous acid. [Pg.1303]

Titrations curves for polyprotic acids have an inflection point for each hydrogen in the formula if the dissociation constant (Ka) for each hydrogen is very different from the others and if any dissociation constant is not too small. The titration curves of the polyprotic acids H2S04 and H3P04 are shown in Figures 5.6 and 5.7. Sulfuric acid has essentially one inflection point (like hydrochloric acid—compare with Figure 5.1(a)), while phosphoric acid has two apparent inflection points. Both hydrogens on the... [Pg.103]

Repeat problem 3, but compare the titration curves of 0.10 M sulfuric acid and 0.10 M phosphoric acid titrated with 0.10 M sodium hydroxide. [Pg.139]

Titration of a polyprotic acid results in multiple equivalence points and a curve with more "bumps" as shown below for sulfurous acid and the carbonate ion. [Pg.180]

The end points, like those for conductometric titration of soluble acids, are found at the intersection of the extrapolated linear portions of the titration curves. The first end point corresponds to sulfonic acid sulfur and the second to the total acid content, i.e., sulfonic plus carboxylic. [Pg.476]

Wolfrom and coworkers have summated their analytical data on the barium acid salt of heparin, and have expressed the data in terms of a tetrasaccharide unit which comprises two molecular proportions each of 2-amino-2-deoxy-D-glucose residue and D-glucuronic acid residue, and 5 (rather than 6) ester sulfate groups, in an N S ratio of 2 5. The barium sulfur ratio was 1 2, which indicated that the sulfur is essentially present as ester sulfate, and hence the acidity must be due to the carboxyl group, in accordance with the shape of the titration curve. " ... [Pg.352]

Some of these effects are illustrated in the experimental curves of Figures 15-1 and 15-2. In the titration of Fe(II), before the end point the shapes are independent of the nature of the oxidant. The value of El is highest with perchloric acid, because hydrolysis of Fe(III) is largely suppressed and the perchlorate ion has little tendency to form complexes. With sulfuric acid and with Ce(IV) as titrant, the two effects of hydrolysis and complex formation tend to counteract each other. In the presence of phosphoric acid, complex formation predominates, and El is distinctly lower. The shape of the curve beyond the end point is determined primarily by the properties of the oxidant. For Ce(TV) in various media the value of El is different, and the potential varies correspondingly. The reasons for these effects are qualitatively the same as for the Fe(III)-Fe(II) couple. Note that three of the experimental curves with Ce(IV) in Figure 15-1 closely resemble the expected shapes the distortion of the curve for hydrochloric acid after the end point is due to the gradual oxidation of chloride by the excess Ce(IV). For further details see the discussion of Ce(TV) as a reagent (Chapter 18). [Pg.287]

Figure 15-2 (left) depicts several titration curves of Fe(II) with permanganate. Beyond the end point the experimental curves differ from the theoretical shape, which is nearly flat beyond the end point (5-equivalent reduction). The essential symmetry of the curves suggests that the potential is determined by the Mn(III)-Mn(II) couple beyond the end point. Evidence for this behavior can be seen in solutions containing sulfate or phosphate, which tend to stabilize Mn(III) (Section 17-1). That sulfuric and phosphoric acids have about the same effect before and after the end point is consistent with the similarity of the behavior of the Mn(III)-Mn(II) and the Fe(III)-Fe(II) systems with respect to changes in activity coefficients as well as with respect to hydrolysis and complex formation. [Pg.287]

In the following experiment a thin paste of arrow-root starch was treated with malt a-amylase. The degree of hydrolysis was ascertained by titration with hypoiodite and n-glucose and maltose were determined by fermentative methods. After the fermentation, the average chain lengths of the a-dextrins was determined by titration with hypoiodite before and after complete hydrolysis with sulfuric acid. In Fig. 4, curve... [Pg.274]

Curve C is the titration curve for sulfuric acid, a substance that has one fully dissociated proton and one that is dissociated to a relatively large extent K 2 1 02 X 10 ). Because of the similarity in strengths of the two acids, only a single end point, corresponding to the titration of both protons, is observed. [Pg.415]

The data obtained will allow the plotting of what is called a titration curve, a plot of pH on the y-axis and the volume of NaOH added (in mL) on the x-axis. There are some unique features of this curve for each of the two acids in question and these will be the basis for the identification. What I suggest you do is create such a curve for both sulfuric acid and phosphoric acid. You can then create the same curve for the unknown waste acid and then match the curve for the unknown to that of one of the two acids and thereby identify it. Additional details are given in my attached procedure. [Pg.184]

Thus in 2bN sulfuric acid the semiquinone ion III is so stable that the oxidation-reduction titration curve shows a definite step at the 50 per cent point and the color of the semiquinone is quite clearly apparent throughout one half of the titration. [Pg.331]

Fig. 5 shows the results of both titration experiments. The experimental results are in good agreement with the predictions based upon the equilibrium expressions for Kb the Ka for each indicator, and the mass and charge balances[13]. The data from the acid titration show a sharp equivalence point at approximately 10 m HCl, which suggests that B(OH)4 is still a strong base at 350°C and 0.622 g/mL and capable of neutralizing HCl. This strong acid base titration curve, as was also observed for HCl and KOH, may be contrasted with the weak acid-base behavior observed for the sulfuric acid-ammonia system at 380 C[41]. [Pg.331]

Fig. 17.4 Titration curve of a 10 mol/L ferrous ion solution with a 1/6 mol/L potassium dichromate solution in sulfuric acid solution (1 mol/L) (V =50ml, ° i= 0.68 V,... Fig. 17.4 Titration curve of a 10 mol/L ferrous ion solution with a 1/6 mol/L potassium dichromate solution in sulfuric acid solution (1 mol/L) (V =50ml, ° i= 0.68 V,...
Nuclear magnetic resonance spectrometry has solved so many problems that one would hope it could be applied to the determination of aliphatic weak bases. Taft and Levins (338) have succeeded in using this method through the effect of protonation on the fluorine resonance of several p-fluorinated bases. Unfortunately, the flu-orinated aromatic system is required and also a relatively concentrated solution of indicator so that the use of aqueous acid is ruled out. In acetic-sulfuric acid solutions Taft finds serious medium effects for Hammett indicators but sharp titration curves for car-bonium ion bases. This result is in complete agreement with the conclusions described previously (II-D) for solvation of carbonium ions compared to other onium ions. [Pg.247]

Palieri (1952) distilled two 7.5-ml. portions from 20 ml. o Jwine. The second 7.5-ml. portion was titrated and contained about 60% of the acetic acid, largely free of sulfur dioxide or lactic acid. In general, the amount of acetic acid present in the distillate was a function of the volume distilled, and a curve, y , where y is the total amount present and x the per cent distilled, could be constructed. [Pg.409]


See other pages where Sulfuric acid titration curve is mentioned: [Pg.510]    [Pg.324]    [Pg.75]    [Pg.342]    [Pg.262]    [Pg.288]    [Pg.292]    [Pg.219]    [Pg.185]    [Pg.131]    [Pg.2381]    [Pg.263]    [Pg.119]    [Pg.9]    [Pg.197]    [Pg.48]    [Pg.98]    [Pg.780]    [Pg.50]    [Pg.172]    [Pg.241]    [Pg.247]    [Pg.136]    [Pg.318]    [Pg.414]   
See also in sourсe #XX -- [ Pg.138 , Pg.139 ]




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