The distance of dispersive following water (x), the distributio of water-drop's radius and cubic distribution of dispersive water were studied.
We made out following; namely, 1) the functional relation exists between x and the quantity of dispersive water, 2) all dispersive water drops in as far as x=30H (H is Height of Concentrator), 3) about a half quantity of dispersive water is with-drawn when the floor's area is spread H meter to the lee side.

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Catching of brine droplets by means of vinyl chloride nets was studied in a small wind tunnel (45×45cm). Prevention of splashing of brine in a “Shijoka” concentrator was also studied by hanging vinyl chloride nets, etc., around the concentrator.
The results were as follows:
(1) The following theoretical equation was derived.
Where η=D/I (I/sinθ+I) η: catching efficiency
D: diameter of the net yarn
I: pitch of the net
θ: angle of droplets crossing the net
(2) The experiment with a small wind tunnel showed that the catching ratio of the net agreed closely with the value calculated by equation (1).
(3) In the field test, the catching efficiency of the 12 mesh vinyl chloride net was 50-60%, while those of 8 and 10 mesh nets were slightly lower.
(4) The wind velocity was slightly decreased in the case of 8-12 mesh nets.

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The author investigated the corrosion inhibitor effect of Urotropin in various conditions of acid cleaning and following results were obtained.
(1) Urotropin exhibited the sufficient inhibitor effect at the concentration of 0.1-0.2%, and the effect was influenced little by concentration of acid and the area of steel.
(2) Urotropin exhibited the corrosion inhibitor action to steel also in a hot acid solution, but on heating the solution contained Urotropin to above 40°C the corrosion loss of steel increased. Then it was desirable that Urotropin was used in the acid solution below 40°C.
(3) Urotropin exhibited the same large inhibitor effect both in the hydrochloric acid and the sulphuric acid solution, but the smaller in the phosphoric acid solution and had none in the nitric acid solution.
(4) The corrosion inhibitor effect of Urotropin had no relation almost to all kinds of iron and steel.

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The chromium and the vanadium contents of solar salt and home product salt were determined colorimetrically with the diphenylcarbazide method and the sodium diphenylamine sulfonate method, respectively, after being collected by coprecipitation with ferric hydroxide in the water soluble part.
While, those of the water insoluble matter were directly determined after being incinerated and treated with hydrofluoric acid-sulfuric acid mixture.
0.149 p.p.m. Cr and 0.33 p.p.m. V in the solar salt and 0.008 p.p.m. Cr and 0.09 p.p.m. V in the home product salt.
The most of the chromium and the vanadium were contained in the water insoluble matter. These elements in the solar salt were derived mainly from the soil of the salt field, and it was presumed that those in the home product salt were derived from sea water and the salt making apparatus.

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In the previous report (4), the formation of basic magnesium hypochlorite by a non-diaphragm electrolysis to separate magnesium dissolved in sea water was studied, but magnesium could not be removed completely, and the amount of precipitate was so little its composition could not be considered.
In this report, magnesium chloride solution containing 1.7 mol per litre of magnesium was used, and the effects of electrolytic factors on the formation of basic hypochlorite and the formation of hypochlorous acid, hypochlorite and chlorate in electrolyte were studied. Factors that had been employed were amount of sodium chloride, current density, distance between electrodes, quantity of electrolytic current, temperature, leaving time after electrolysis, and the effect of calcium. And also oxidation current efficiency, decomposition ratio of chloride, and removal ratio of magnesium were determined.
Formation of basic hypochlorite was affected significantly by temperature and leaving time after electrolysis relating with the reaction velocity of magnesium hydroxide and hypochlorite. The amount of precipitate and of the hypochlorite in precipitate were reached to a maximum value at 50°C, and these amounts were increased considerably by the leaving time of 24 hours, and also were reached to a maximum value at 72 hours. Compositions of basic magnesium hypochlorites were varied by the conditions of their preparations, and the mole ratios in precipitates that obtained were Mg(ClO)₂: Mg(OH)₂: H₂O=1:18.5-3.1:11.3-0, but they gave a same results by the X-ray diffraction, and showed the patterns indicating diffused bands of weak intensity at 13°, 36° and 59°(2θ).
In the electrolysis of brine, amount of precipitate was increased more than in magnesium chloride solution, but amount of precipitate was increased more than in magnesium chloride solution, but amount of hypochlorite in precipitate was decreased, so the effect of addition of sodium chloride was recognized. But, in this case, removal ratio of magnesium was not so much as 17 percent.
It was considered to be difficult to remove completely magnesium by a process of formation of basic hypochlorite.

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Barium rhodizonate liberates rhodizonic acid when reacts with sulfate ion in aquous solution. The sulfates contents of bittern, sea brine and common salts were determined by measuring the absorbancy of thus liberated rhodizonic acid. The measurments were made at 530mμ, adding iso-propylalcohol or ethyl-cellosolve as color stabilizer, in pH range 4-7. Good results were obtained for each sample, and Ca⁺⁺, Mg⁺⁺ or Al⁺⁺⁺ did not interfer.

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Densities, thermogravimetric analyses and powder X-ray diffraction patterns of the following basic triple and double salts were studied: 1) new basic triple salt NS salt A (Na₂SO₄·2MgSO₄·Mg(OH)₂·4H₂O), 2) new basic triple salt NS salt B (K₂SO₄·2MgSO₄·Mg(OH) ₂·2H₂O), 3) 8MgSO₄·Mg(OH)₂·8H₂O, new basic double salt being crystallized from the solution containing magnesium sulfate, magnesium chloride and magnesium hydroxide at boiling point, 4) K₂SO₄·15MgSO₄·9Mg(OH)₂·18H₂O (?), new basic triple salt being crystallized from the 100° isotherm of the system K₂SO₄-MgSO₄-Mg(OH)₂-H₂O, 5) MgCl₂·2Mg(OH)₂·6H₂O, new basic double salt being deposited from the 100° isotherm of the system MgCl₂-Mg(OH)₂-H₂O, 6) MgCl₂·3Mg (OH)₂·8H₂O being deposited from the 50° isotherm of the same system, 7) MgSO₄·5Mg(OH)₂·3H₂O being deposited from 100° and 50° isotherms of the system MgSO₄-Mg(OH)₂-H₂O.

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