Nitric acid molar mass

A series of criticality experiments has been performed at the Hanford Critical Mass Laboratory with plutonium (4.6 wt% Pu-240) nitrate solutions in thin stainless-steel spheres of 11.5-, 14- and 15.2-in. diam. Various types of neutron reflectors used in the experiments were water, concrete, paraffin and stainless steel. Criticality data were also obtained with the 15.2-in. sphere unreflected. The effect of partial reflection by concrete and the effect of an air gs between the core and its reflector were also examined. Critical plutonium concentrations were measured in the range from 24 to 435 g Pu/f, depending on the nitric acid molarity (0.2 to 7.7 molar) and the condition of neutron reflection. 

A series of experiments has been completed with plutonium obtained from extreme high burnup fuel to establish the combined effects of the various isotopes of plutonium on criticality. The isotopic composition of the plutonium, as measured on August 11, 1971, was Pu-0.2 wt%, Pu-41.4 Wt%, Pu-42.9wt%, Pu-10.8wt%, and Pu-4.7 wt%. A nonnegligible amount of Am also was present to the extent of 1.08 wt% of the total Pu. The experiments were performed in a 24-ln.-diam, water-reflected, cylindrical vessel. Ten data points were obtained with the critical heights and masses de rmined for various plutonium concentrations and nitric acid molarities in the plutonium nitrate solutions. Plutonium concentrations covered the range of about 40 to 140 g Phi/liter with nitric acid molarities ranging from about 1.5 to 5. 

Reagent grade nitric acid is 71.0% nitric acid by mass and has a density of 1.418 g/mL. Calculate the molarity, molality, and mole fraction of nitric acid in the solution. 

L.ll A sample of barium hydroxide of mass 9.670 g was dissolved and diluted to the mark in a 250.0-mL volumetric flask. It was found that 11.56 mL of this solution was needed to reach the stoichiometric point in a titration of 25.0 ml. of a nitric acid solution, (a) Calculate the molarity of the HN03 solution. 

The reason why SIA is higher in urban areas is less obvious as these are secondary aerosols. The observed increment is predominantly caused by more nitrate and sulphate. The reaction of nitric acid and sulphuric acid with the sea-salt aerosol in a marine urbanised environment follows an irreversible reaction scheme. In essence, the chloride depletion stabilises part of the nitrate and sulphate in the coarse mode and may partly explain part of the observed increment. However, it also raises the question how to assign the coarse mode nitrate in the mass closure. The sea salt and nitrate contributions cannot simply be added any more as nitrate replaces chloride. Reduction of NOx emissions may cause a reduction of coarse mode nitrate, which is partly compensated by the fact that chloride is not lost anymore. A reduction would yield a net result of ((N03-C1)/N03 = (62-35)/62=) 27/62 times the nitrate reduction (where the numbers are molar weights of the respective components), and this factor could be used to scale back the coarse nitrate fraction in the chemical mass balance. A similar reasoning may be valid for the anthropogenic sulphate in the coarse fraction. Corrections like these are uncommon in current mass closure studies, and consequences will have to be explored in more detail. 

The bare proton has an exceedingly small diameter compared with other cations, and hence has a high polarising ability, and readily forms a bond with an atom possessing a lone pair of electrons. In aqueous solution the proton exists as the H30+ ion. The existence of the H30+ ion in the gas phase has been shown by mass spectrometry [4], and its existence in crystalline nitric acid has been shown by NMR [5], Its existence in aqueous acid solution may be inferred from a comparison of the thermodynamic properties of HC1 and LiCl [6]. The heat of hydration of HC1 is 136 kcal mole"1 greater than that of LiCl, showing that a strong chemical bond is formed between the proton and the solvent, whereas the molar heat capacity, molar volume and activity coefficients are similar,... 

What is the molarity of the solution that is 63% nitric acid (HN03) by mass (The density of the solution is 1.4 g/mL)... 

The density of c% nitric acid solution by mass is p in g/mL. Prove that the molarity of the nitric acid solution is... 

The proposed feed to the stirred tank has the same concentration of nitric acid, no, but from the mass flow rates given it is evident that the molar proportions are changed. In fact, the feed of both BSA and nitric acid is 2 Ib-mole/hr and hence their feed concentrations will both be and their concentrations in the tank will be the same. Denoting the latter by n, a balance on the nitric acid gives... 

Samples weighing 2-5 mg are then dissolved in 5-molar nitric acid. The strontium fraction is purified using ion-specific resin and eluted with nitric acid followed by water. This solution is loaded onto a titanium filament for placement in the instrument (Fig. 4.20). Isotopic compositions are obtained on the strontium fraction thermal ionization mass spectrometer (TIMS). This is a single focusing, magnetic sector instrument equipped with multiple Faraday collectors. Strontium is placed on a thin filament and measured. Sr/ Sr ratios are corrected for mass fractionation using an exponential mass fractionation law. Sr/ Sr ratios are reported relative to a value of 0.710250 for the NIST 987 standard (e.g., if the Sr/ Sr ratios for the standards analyzed with the samples average 0.710260, a value of 0.000010 is subtracted from the ratio for each sample). 

How many milliliters of 1.50 M nitric acid, HNCVag), are required to just consume 25.0 g of barium oxide, BaO The molar mass of BaO is 153.3 g. The balanced equation is... 

Figure 1. (A) Effect of the titration temperature during Fe-decomplexation exchanged on the N2O decomposition activity using citrate Fe-precursor at ( ) 333 ( ) 353 and (A) 373 K. For comparison, a reference catalyst based on ion-exchange using ferric nitrate (same Fe loading) is included (O). Reaction conditions 4.5 mbar N2O, He balance. (B) Stability test for ( ) in A spot under typical conditions for nitric acid plants in The Netherlands 4.5 mbar N2O + 0.6 mbar NO + 15 mbar H2O + 75 mbar O2. In both cases, total pressure was 3 bar-a and a space time W/F (N20) of 900 kgxsxmoT (W is the catalyst mass and F (N20) the molar flow of N2O in the reactor inlet) was applied.

Feed and removal volumetric flow Concentration of hexamine in feed Molar mass of hexamine Concentration of nitric acid in feed Molar mass of nitric acid Pre-exponential factor Apparent energy of activation Order of the reaction Thermal capacity of hexamine Feed temperature of hexamine Thermal capacity of nitric acid Feed temperature of nitric acid Overall coefficient of heat transfer Area for heat transfer (jacket + coU) Enthalpy of reaction Reaction temperature... 

Nitric acid HNO3 Molar mass MhNOs 63.01 kg/kmol... 

Deionised water or nitric acid solutions of different molarities were used for the hydrodynamic and mass transfer experiments. The HNO3 solutions were prepared in the UCL laboratory from aqueous nitric acid (65 %) solutions of general purpose grade ( 14.4 M) by Fisher Scientific (p = 1370-1400 kg m p = 0.0023 kg m s ). 

Other solvents and initiators are, for example, butanone [495] or ethyl methyl ketone [470,476] with AIBN [496-499] and dioxane with benzoyl peroxide [474,484,500,503]. In benzene as solvent the resulting polymer forms a slurry [504]. AIBN can be used as an initiator in aqueous solutions by solubilizing the initiator with 4% ethanol [504]. Methacrylic acid polymerizes in nitric acid at 5 to 30 °C to a molar mass of 2 x 10 and the product precipitates in acetone as a white powder [505]. Nitrogen dioxide reacts as an initiator in benzene to synthesize poly(acrylic acid) at 50 °C with molar masses of 48,000 [506]. Sodium bisulfite initiates polymerization of methacrylic acid in an aqueous medium but is ineffective for acrylic acid [507]. 

A 30.00%-by-mass solution of nitric acid, HNO3, in water has a density of 1.18 g/cm at 20 °C. What is the molarity of HNO3 in this solution ... 

Thanks to gas chromatography and atmospheric-pressure chemical-ionization mass-spectrometry analyses, a mechanism of nPr-BTP degradation has been proposed. The first step is assumed to be the attack at one CH2 group on the a position of the triazine rings to form a nitro compound observed by 15N NMR. In the second step, the compound is degraded into an alcohol (which is the main degradation product observed in the absence of acidic aqueous phase) or into a ketone (which is the main degradation product observed after the hydrolysis of nPr-BTP by molar nitric... 

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