scholarly journals ph of aqueous mixtures of potassium dihydrogen phosphate and disodium hydrogen phosphate at 0 degrees to 60 degrees C

1945 ◽  
Vol 34 (4) ◽  
pp. 373 ◽  
Author(s):  
R.G. Bates ◽  
S.F. Acree
Keyword(s):  
Potassium Dihydrogen Phosphate ◽  
Dihydrogen Phosphate ◽  
Aqueous Mixtures ◽  
Hydrogen Phosphate ◽  
Disodium Hydrogen Phosphate ◽  
Potassium Dihydrogen

The Effect of Phosphatic Composite on Magnesium Phosphate Cement Performance

2014 ◽  
Vol 809-810 ◽  
pp. 477-484
Author(s):  
Zhao Qing Qi ◽  
Hong Tao Wang ◽  
Jun Liang Dang ◽  
Shi Hao Zhang ◽  
Jian Hua Ding
Keyword(s):  
Setting Time ◽  
Potassium Dihydrogen Phosphate ◽  
Magnesium Phosphate ◽  
Dihydrogen Phosphate ◽  
Ammonium Dihydrogen Phosphate ◽  
Hydrogen Phosphate ◽  
Sodium Dihydrogen Phosphate ◽  
Disodium Hydrogen Phosphate ◽  
Potassium Dihydrogen ◽  
Sodium Dihydrogen

The capacity of 10%, 30%, and 50% ammonium dihydrogen phosphate were replaced with an equal amount of three phosphate (potassium dihydrogen phosphate, sodium dihydrogen phosphate, disodium hydrogen phosphate) respectively. Magnesium phosphate cement was made by phosphate of replaced, which strength, setting time, fluidity, hydration temperature, and the hydration products was researched. The results show that: MPC was made that replaced with the equal amount of three kind of phosphate, which has good mechanical properties. Setting time and fluidity change along with the replacment. Three kind of phosphate replace ammonium dihydrogen phosphate, which change the hydration process of MPC. When ammonium dihydrogen phosphate was replaced by an equal amount of disodium hydrogen phosphate, the temperature of hydration is only 69.4 °C. XRD showed that the diffraction peaks of composite’s magnesium phosphate cement increases.

Note on the loss of phosphoric acid during fusion with ammonium fluoride

1916 ◽  
Vol 8 (1) ◽  
pp. 136-138
Author(s):  
William A. Davis ◽  
James Arthur Prescott
Keyword(s):  
Calcium Phosphate ◽  
Alkali Metal ◽  
Phosphoric Acid ◽  
Potassium Dihydrogen Phosphate ◽  
Ammonium Fluoride ◽  
Dihydrogen Phosphate ◽  
Hydrogen Phosphate ◽  
Disodium Hydrogen Phosphate ◽  
Potassium Dihydrogen ◽  
Considerable Loss

1. When salts or minerals containing phosphoric acid are ignited with ammonium fluoride as in the ordinary process of analysis of silicates, considerable loss of the phosphoric acid may occur. It is probable that the phosphorus is volatilised in the form of a phosphorus fluoride.2. The loss is least in the case of salts containing an alkali metal. It is less in the case of disodium hydrogen phosphate than in that of potassium dihydrogen phosphate, and is greatest in the case of phosphates of the alkali earth metals, such as calcium phosphate or apatite.

Osmolarity of Human Serum and of Chemical Solutions of Biologic Importance

1961 ◽  
Vol 7 (2) ◽  
pp. 156-164 ◽  
Author(s):  
Edward B Hendry
Keyword(s):  
Human Serum ◽  
Freezing Point ◽  
Potassium Dihydrogen Phosphate ◽  
Dihydrogen Phosphate ◽  
Hydrogen Phosphate ◽  
Sodium Dihydrogen Phosphate ◽  
Disodium Hydrogen Phosphate ◽  
Normal Human ◽  
Chemical Solutions ◽  
Sodium Dihydrogen

Abstract With the use of the Fiske Osmometer, the mean total osmolarity of normal human serum was found to be 289 mOsM (S.D., 4), which is equivalent to a mean freezing point of -0.537°. The isosmotic concentrations of some important biologic solutions were determined. It was also found that M/15 solutions of disodium hydrogen phosphate and of potassium dihydrogen phosphate are very hypotonic, and that 3.8% sodium citrate is hypertonic. Hemolysis of erythrocytes in isosmotic ammonium chloride solution can be considerably delayed by the addition of 3.0% glucose to the solution. Isosmotic concentrations of disodium hydrogen phosphate and sodium dihydrogen phosphate were precisely determined, as were pH levels of buffer solutions made from these two salts. The cause of the slight changes in osmolarity that occur when these two isosmotic solutions are mixed is discussed.

Activity Coefficients of Potassium Dihydrogen Phosphate in Aqueous Solutions at 25°C and in Aqueous Mixtures of Urea and this Electrolyte in the Temperature Range 20–35°C

2003 ◽  
Vol 217 (6) ◽  
pp. 723-738 ◽  
Author(s):  
Jaakko I. Partanen ◽  
Yuko Mori ◽  
Marjatta Louhi-Kultanen ◽  
Juha J. Kallas
Keyword(s):  
Aqueous Solutions ◽  
Osmotic Coefficients ◽  
Potassium Dihydrogen Phosphate ◽  
Dihydrogen Phosphate ◽  
Pitzer Equation ◽  
Aqueous Mixtures ◽  
Potassium Dihydrogen ◽  
Parameter Estimations ◽  
Aqueous Urea ◽  
Parameter Values

AbstractSimple two-parameter Hückel and Pitzer equations were determined for the calculation of the activity and osmotic coefficients of aqueous solutions of potassium dihydrogen phosphate at 25°C up to a molality of the saturated solution (= 1.83 mol kg−1). The isopiestic data measured by Stokes (1945) were used in the parameter estimations. The resulting parameter values were tested with all thermodynamic data found in the literature for this electrolyte at this temperature. In these tests it was observed, that the Hückel equation applies to the data within experimental error up to a molality of 1.0 mol kg−1, and the Pitzer equation applies well to the data in the molality range 1.0–1.83 mol kg−1 but not very well in dilute solutions. Therefore, also a three-parameter Pitzer equation was determined that applies to all data. The activity and osmotic coefficients calculated by these three models were compared to the values suggested by Robinson and Stokes (1959) and to those calculated by the equations of Hamer and Wu (1972) and of Pitzer and Mayorga (1973) for this electrolyte. Solubility measurements of KH2PO4 at 20, 25, 30 and 35°C were made in aqueous urea solutions, and the molality of urea varied in these measurements from 0 to 2.5 mol kg−1. The thermodynamics of these studies were analyzed by using the Pitzer formalism. It was observed that only one interaction parameter between urea molecules and ions (this parameter is linearly dependent on the temperature) was needed to describe almost completely the new solubility data.

scholarly journals Optical Absorption Spectra of Vanadyl Ion (Impurities) in Three Host Crystal Compounds

1985 ◽  
Vol 40 (11) ◽  
pp. 1164-1166
Author(s):  
O. P. Agarwal ◽  
Prem Chand
Keyword(s):  
Optical Absorption ◽  
Potassium Dihydrogen Phosphate ◽  
Optical Data ◽  
Dihydrogen Phosphate ◽  
Host Crystal ◽  
Optical Absorption Study ◽  
Potassium Dihydrogen ◽  
Vanadyl Complexes ◽  
Vanadyl Ion ◽  
Magnesium Ammonium

Results of the optical absorption study of vanadyl ion doped in magnesium ammonium sulphate hexahydrate, rubidium sulphate and potassium dihydrogen phosphate single crystals at RT are reported. The nature of optical bands suggests a C4v symmetry of the Vanadyl complexes in conformity with the EPR results. Powder EPR data and optical data are correlated to obtain the MO coefficients.

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