Solubility Of Boric Acid Research Articles

Экспериментальное исследование растворимости борной кислоты в кипящем паре при атмосферном давлении

Экспериментальное исследование растворимости борной кислоты в кипящем паре при атмосферном давлении

Solubility, Metastable Zone Width, and Nucleation Kinetics of Boric Acid in the NaCl–KCl–CaCl2–H2O System

The solubility and metastable zone width of boric acid in the simulated oilfield brine system of NaCl–KCl–CaCl2–H2O were studied at low temperature by the turbidity method. The nucleation kinetic constant A and the interfacial energy γ of boric acid were calculated with nucleation theory. Results showed that the solubility of boric acid in the simulated oilfield brine system was mainly determined by the coexisting salt of CaCl2 and decreased with increasing concentrations of CaCl2, even though the presence of NaCl and KCl has a salt-in effect on the solubility. However, the metastable zone width was affected by the three coexisting salts and it changes differently with the varied concentrations. The possible reason can be explained by the dependence of the interfacial energy γ on the slat concentration. On the basis of the above results, the crystallization behavior of boric acid during oilfield brine evaporation was investigated for the first time. It was deeply affected by the coexisting salts in brine.

The Solubility of Boric Acid in Electrolyte Solutions

The solubility of boric acid [B] in LiCl, NaCl, KCl, RbCl, and CsCl was determined as a function of ionic strength (0–6 mol ⋅ kg−1) at 25 ∘C. The results were examined using the Pitzer equation $$ \ln \{ [{\rm B}]^0 /[{\rm B}]\} = \ln \gamma _{\rm B} = (2\nu _{\rm c} \lambda _{{\rm Bc}} + 2\nu _{\rm a} \lambda _{{\rm Ba}})m + \nu _{\rm c} \nu _{\rm a} \zeta _{{\rm B - a - c}} m^2 $$ where [B]0 is the concentration of boric acid in water and [B] in solution, γB is the activity coefficient, νi is the number of ions (i), λBc, λBa are parameters related to the interaction of boric acid with cation c and anion a, ζB-a−c is related to the interaction of boric acid with both cation and anion and m is the salt molality. The literature values for the solubility of boric acid in a number of other electrolytes were also examined using the same equation. The results for the 2νcλBc+2νaλBa term (equal to the salting coefficient k S) were examined in terms of the ionic interactions in the solutions. The solubility of boric acid in LiCl, NaCl, and KCl solutions is not a strong function of temperature and the results can be used over a limited temperature range (5–35 ∘C). Boric acid is soluble in the order SO4 > NO3 and F > Cl > Br > I in common cation solutions. In common anion salt solutions, the order is Cs > Rb > K > Na > Li > H and Ba > Sr > Ca > Mg. The results were examined using correlations of k S with the volume properties of the ions. When direct measurements were not available, k S and ζB-c−a were estimated from known values of λBc and λBa. The values of λBc, λBa, and ζB-a−c can be used to estimate the boric acid activity coefficients γB and solubility [B] in natural mixed electrolyte solutions (seawater and brines) using the more general Pitzer equation $$ \hspace*{20pt}\ln \{ [{\rm B}]^0 /[{\rm B}]\} = \ln \lambda _{\rm B} = (2\Sigma _{\rm c} \nu _{\rm c} \lambda _{{\rm Bc}} + 2\Sigma _{\rm a} \nu _{\rm a} \lambda _{{\rm Bac}})m + \Sigma _{\rm c} \Sigma _{\rm a} \nu _{\rm c} \nu _{\rm a} \zeta _{{\rm B - a - c}} m^2 $$

Solubility of boric acid in aqueous solutions of chloride salts

Solubility of boric acid in aqueous solutions of sodium chloride, potassium chloride and of both sodium and potassium chlorides was measured in a wide range of salt concentrations at temperatures from 303–373 K. These data, together with solubility data of chloride salts in aqueous solutions of boric acid, are used to parameterize a general thermodynamic model which uses the Wilson equation, along with contributions from Debye-Huckel and a Born term, in order to express the activity coefficients. The model, which contains only binary interaction parameters, can be used to correlate and predict thermodynamic properties of multicomponent aqueous systems containing boric acid along with both sodium and potassium chlorides.

Solubility of boric acid in aqueous solutions of sulfate salts

Solubility of boric acid in aqueous solutions of sodium sulfate, potassium sulfate and of both sodium and potassium sulfates and solubility of sulfate salts in aqueous solutions of boric acid were measured in a wide range of salt concentrations at temperatures from 303–373 K. The experimental data have been correlated by a thermodynamic model which uses the Wilson equation along with contributions from Debye-Huckel and a Born term in order to express the activity coefficients. The predictive capability of this model, which contains only binary interaction parameters, has been verified on multicomponent systems in the whole range of the process operating conditions.

Study of the Boric Acid-Glycerin Complex II: Formation of the Complex at Elevated Temperatures

A study of the boric acid-glycerin complex was conducted at temperatures of 30, 40, 50, and 60° and the effect of increasing the concentration of glycerin upon the solubility of boric acid was studied. This may then be indicative of the degree of complex formation taking place between these two substances. Concentrations of glycerin varying from 0 to 100% were utilized. The results of these experiments show the relationship between (a) solubility of boric acid and (b) temperature and concentration of glycerin. A phase diagram was constructed at these temperatures showing the quantitative relationship among boric acid, water, and glycerin. From a plot of the log solubility of boric acid versus the reciprocal of absolute temperature, the heat of solution at various concentrations of glycerin was calculated. It was found that the degree of complex formation between boric acid and glycerin increased with an increase in temperature but showed little, if any, increase with an increase in glycerin concentration from 0 to about 40%. However, above this concentration of glycerin, the degree of complex formation, as indicated by the solubility, increased with an increase in concentration of glycerin.

A Solubility Study of the Boric Acid-Glycerin Complex I : Solubility of Boric Acid in Glycerin Solution at 25°

A solubility study of the boric acid-water-glycerin system was made at 25°. The effect of concentration of glycerin upon the solubility of boric acid was noted. Concentrations of glycerin ranging from 0 per cent to 100 per cent, by weight, were utilized in this study. A phase diagram of this three-component system was constructed at 25°. The results of this investigation were compared to the boric acid-water-sorbitol system and a difference was noted between the nature of the boric acid-sorbitol complex and the boric acid-glycerin complex.

A Solubility Study of the Boric Acid-Water-Sorbitol System at Various Temperatures

A study of the effect of various concentrations of sorbitol and temperature on the solubility and heat of solution of boric acid in water has been made. This system was studied at temperatures of 21°, 25°, 30°, 40°, 50°, and 60°. Concentrations of sorbitol ranging from 0 to 70 per cent by weight sorbitollin increments of 5 per cent were utilized in this study. The results of these experiments showed the relationship between (1) solubility of boric acid and (2) temperature and concentration of sorbitol. A phase diagram of the boric acid-water-sorbitol system is given. The heat of solution for the various systems was calculated. The specific gravity of all solutions was determined by the pycnometric method.

Solubility of Boric Acid

Solubility of Boric Acid