JP2000185921A - Production of ferric sulfate solution - Google Patents
Production of ferric sulfate solutionInfo
- Publication number
- JP2000185921A JP2000185921A JP10363641A JP36364198A JP2000185921A JP 2000185921 A JP2000185921 A JP 2000185921A JP 10363641 A JP10363641 A JP 10363641A JP 36364198 A JP36364198 A JP 36364198A JP 2000185921 A JP2000185921 A JP 2000185921A
- Authority
- JP
- Japan
- Prior art keywords
- iron oxide
- ferrous sulfate
- sulfuric acid
- iron
- solution
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Granted
Links
Landscapes
- Inorganic Compounds Of Heavy Metals (AREA)
Abstract
Description
【０００１】[0001]
【発明の属する技術分野】本発明は硫酸第二鉄溶液の製
造方法、殊に酸化鉄溶解液として硫酸第一鉄と硫酸とを
含んだ溶液を使用することを特徴とする硫酸第二鉄溶液
の製造方法に関する。BACKGROUND OF THE INVENTION 1. Field of the Invention The present invention relates to a method for producing a ferric sulfate solution, and more particularly to a ferric sulfate solution characterized by using a solution containing ferrous sulfate and sulfuric acid as a solution for dissolving iron oxide. And a method for producing the same.
【０００２】[0002]
【従来の技術】硫酸第二鉄溶液は、近年特に有用な水処
理剤として注目され、特に硫酸第二鉄溶液、塩基性硫酸
第二鉄溶液はアルミニウム系水処理剤である硫酸アルミ
ニウム溶液、塩基性塩化アルミニウム溶液に比べて生成
フロックの沈降速度が早く、また脱臭力も優れているこ
とから製紙工業廃水、食品工業廃水、化学工業廃水等の
水処理剤として、あるいは下水汚泥の脱水助剤として汎
用されている。2. Description of the Related Art In recent years, ferric sulfate solutions have attracted attention as particularly useful water treatment agents. In particular, ferric sulfate solutions and basic ferric sulfate solutions are aluminum-based water treatment agents such as aluminum sulfate solutions and bases. Higher sedimentation rate of generated floc and superior deodorizing power compared to aqueous aluminum chloride solution.Generally used as a water treatment agent for paper industry wastewater, food industry wastewater, chemical industry wastewater, etc., or as a dewatering aid for sewage sludge. Have been.
【０００３】この硫酸第二鉄溶液、塩基性硫酸第二鉄溶
液は一般に硫酸第一鉄を水に溶解し適量の硫酸を加え、
空気酸化あるいは酸化剤で酸化することにより製造され
ていたが、近年鋼板等の酸洗によりあるいはチタン工業
より排出・副生される硫酸第一鉄が減少し、原料逼迫を
招来しているのが現状である。This ferric sulfate solution and basic ferric sulfate solution are generally prepared by dissolving ferrous sulfate in water and adding an appropriate amount of sulfuric acid.
It was manufactured by air oxidation or oxidation with an oxidizing agent.However, in recent years, ferrous sulfate discharged and by-produced from the pickling of steel sheets or from the titanium industry has been reduced, which has led to tightness in raw materials. It is the current situation.
【０００４】そこで、本発明者らは酸化鉄を原料として
硫酸第二鉄溶液を製造する研究に着手し、種々検討を重
ねた結果、酸化鉄を硫酸で溶解するに際し、これを硫酸
第一鉄の存在下で行えば酸化鉄の溶解性が著しく向上す
ることを発見し、かかる知見に基づき本発明を完成した
ものである。Accordingly, the present inventors have started research on producing a ferric sulfate solution using iron oxide as a raw material, and as a result of various studies, found that when dissolving iron oxide with sulfuric acid, the ferrous sulfate was dissolved. It has been found that the solubility of iron oxide is remarkably improved if carried out in the presence of, and the present invention has been completed based on such findings.
【０００５】従来より、酸化鉄は塩酸にはよく溶解する
が硫酸に対しては難溶なことは良く知られている。これ
まで、溶解方法について種々の提案がなされてきた。例
えば、特公平２−２２０１２号公報には四三酸化鉄（Ｆ
ｅ3Ｏ4）１モルに対し、硫酸を３モル以上４モル未満使
用してポリ硫酸第二鉄溶液を製造する方法が開示されて
いる。また、特公平５−１３０９５号公報には、四三酸
化鉄等の溶解方法として、濃度３５〜５０％の硫酸を用
い、７５℃以上の温度で溶解する方法が開示され、特公
平５−１３０９４号公報には四三酸化鉄等と金属鉄とを
濃度４０〜４５％の硫酸を用い、７５℃以上の温度で溶
解する方法が開示されている。[0005] It is well known that iron oxide is well soluble in hydrochloric acid but hardly soluble in sulfuric acid. Until now, various proposals have been made on the dissolution method. For example, Japanese Patent Publication No. 2-22012 discloses iron trioxide (F
A method for producing a ferric polysulfate solution using sulfuric acid in an amount of 3 to less than 4 mols per mol of e 3 O 4 ) is disclosed. Japanese Patent Publication No. 5-13095 discloses a method for dissolving iron trioxide and the like at a temperature of 75 ° C. or higher using sulfuric acid having a concentration of 35 to 50%. Japanese Patent Application Laid-Open Publication No. H11-176,055 discloses a method of dissolving triiron tetroxide or the like and metallic iron at a temperature of 75 ° C. or higher using sulfuric acid having a concentration of 40 to 45%.
【０００６】特公平５−５３７３０号公報には四三酸化
鉄を主成分とする酸化鉄に、当該四三酸化鉄１モルに対
して３モル以上１０モル未満であって３０〜５０％濃度
の硫酸と、当該四三酸化鉄中のＦｅ2Ｏ3分に対して０．
１乃至０．５当量の還元剤とを添加し、７５℃以上で溶
解し硫酸鉄溶液を得る方法が開示されている。特開平７
−２４１４０４号公報には、酸化鉄を硫酸に溶解し、必
要に応じて酸化処理が施される鉄系凝集剤において、該
酸化鉄の三価の鉄原料に塩化第二鉄溶液から生成する酸
化水酸化鉄を用いることが開示されている。しかしなが
ら、これらの方法は使用する酸化鉄原料が制約されるば
かりでなく、未だ酸化鉄の溶解性が充分満足できるもの
ではない。Japanese Patent Publication No. 5-53730 discloses that an iron oxide containing triiron tetroxide as a main component has a concentration of 30 to 50% in a concentration of 3 to less than 10 mol per 1 mol of the triiron tetroxide. 0.1% of sulfuric acid and Fe 2 O 3 in the ferric oxide.
A method is disclosed in which 1 to 0.5 equivalent of a reducing agent is added and dissolved at 75 ° C. or higher to obtain an iron sulfate solution. JP 7
JP-A-241404 discloses an iron-based coagulant in which iron oxide is dissolved in sulfuric acid and oxidized as necessary to produce an iron oxide trivalent iron raw material from a ferric chloride solution. The use of iron hydroxide is disclosed. However, in these methods, not only is the iron oxide raw material used restricted, but also the solubility of iron oxide is not yet sufficiently satisfactory.
【０００７】[0007]
【発明が解決しようとする課題】そこで、本発明は酸化
鉄の溶解性を顕著に向上させることにより、安価に且
つ、工業的に容易に硫酸第二鉄溶液を製造する方法を提
供することを目的とする。SUMMARY OF THE INVENTION Accordingly, the present invention is to provide a method for producing a ferric sulfate solution inexpensively and industrially easily by remarkably improving the solubility of iron oxide. Aim.
【０００８】[0008]
【課題を解決するための手段】即ち、本第１の発明は、
硫酸第一鉄と硫酸とを含んだ溶液を用いて酸化鉄を溶解
した後、２価の鉄を３価の鉄に酸化することを特徴とす
る硫酸第二鉄溶液の製造方法に関する。更に、本第２の
発明は、本第１の発明における酸化鉄と硫酸第一鉄の使
用割合が、硫酸第一鉄由来Ｆｅ／（硫酸第一鉄由来Ｆｅ
＋酸化鉄由来Ｆｅ）（モル比）≧０．１である硫酸第二
鉄溶液の製造方法に関する。本第３の発明は、本第１ま
たは２の発明において、溶解時における全鉄に対する全
硫酸の割合が１．２５≦ＳＯ4／Ｆｅ（モル比）≦１．
５である硫酸第二鉄溶液の製造方法に関する。また、本
第４の発明は、本第１、２または３の発明において溶解
温度が７０℃以上である硫酸第二鉄溶液の製造方法に関
する。That is, the first aspect of the present invention provides:
The present invention relates to a method for producing a ferric sulfate solution, comprising dissolving iron oxide using a solution containing ferrous sulfate and sulfuric acid, and then oxidizing divalent iron to trivalent iron. Further, in the second invention, the use ratio of the iron oxide and the ferrous sulfate in the first invention is such that the ratio of ferrous sulfate-derived Fe / (ferrous sulfate-derived Fe
(Fe) derived from iron oxide (molar ratio) ≧ 0.1. According to the third invention, in the first or second invention, the ratio of total sulfuric acid to total iron at the time of dissolution is 1.25 ≦ SO 4 / Fe (molar ratio) ≦ 1.
5 relates to a method for producing a ferric sulfate solution. Further, the fourth invention relates to a method for producing a ferric sulfate solution having a dissolution temperature of 70 ° C. or higher in the first, second, or third invention.
【０００９】[0009]
【発明の実施の形態】本発明の硫酸第二鉄とは、ＳＯ4
／Ｆｅ（モル比）＝１．２５〜１．５の範囲にあるも
の、即ち硫酸第二鉄の正塩溶液及び塩基性硫酸第二鉄溶
液を意味する。また、本発明酸化鉄とはα−Ｆｅ2Ｏ3、
γ−Ｆｅ2Ｏ3、四三酸化鉄、α−ＦｅＯＯＨ、β−Ｆｅ
ＯＯＨ、γ−ＦｅＯＯＨ及びこれらの含有物を意味す
る。BEST MODE FOR CARRYING OUT THE INVENTION Ferric sulfate according to the present invention refers to SO 4
/ Fe (molar ratio) = 1.25 to 1.5, that is, a normal salt solution of ferric sulfate and a basic ferric sulfate solution. The iron oxide of the present invention is α-Fe 2 O 3 ,
γ-Fe 2 O 3 , triiron tetroxide, α-FeOOH, β-Fe
OOH, γ-FeOOH and their contents are meant.
【００１０】本発明は酸化鉄を硫酸を用いて溶解するに
当たり、硫酸第一鉄を使用するものであるが、後述する
如く硫酸第一鉄を使用することにより酸化鉄の溶解度は
著しく向上する。硫酸第一鉄は鋼板、鋼線等の酸洗によ
るものであっても、チタン工業より排出する粉状、また
は液状のものであっても良い。しかして、その使用割合
は、硫酸第一鉄由来Ｆｅ／（硫酸第一鉄由来Ｆｅ＋酸化
鉄由来Ｆｅ）（モル比）≧０．１以上である。より好ま
しくは０．３以上である。０．１以下の場合、酸化鉄の
溶解率が小さく、本発明の効果を期待することができな
い。In the present invention, ferrous sulfate is used for dissolving iron oxide using sulfuric acid. As will be described later, the use of ferrous sulfate significantly improves the solubility of iron oxide. Ferrous sulfate may be obtained by pickling steel plates, steel wires, or the like, or may be powdery or liquid discharged from the titanium industry. Thus, the ratio of use is as follows: ferrous sulfate-derived Fe / (ferrous sulfate-derived Fe + iron oxide-derived Fe) (molar ratio) ≧ 0.1 or more. It is more preferably at least 0.3. If it is less than 0.1, the dissolution rate of iron oxide is small, and the effects of the present invention cannot be expected.
【００１１】次に硫酸について述べると、硫酸第一鉄と
硫酸とを含んだ溶液中の硫酸の濃度は、酸化鉄の種類、
溶解させる酸化鉄中のＦｅ含有量とも関連するが、一般
に２５〜５０重量％が良い。より好ましくは３０〜４０
重量％である。２５重量％以下では、酸化鉄の溶解に長
時間を要し、５０重量％以上の場合、原料の添加順序、
酸化鉄と硫酸との使用割合、溶解温度等にもよるが、一
般に酸化鉄の溶解率は小さくなる。Next, regarding sulfuric acid, the concentration of sulfuric acid in a solution containing ferrous sulfate and sulfuric acid depends on the type of iron oxide,
Although it is related to the Fe content in the iron oxide to be dissolved, 25 to 50% by weight is generally good. More preferably, 30 to 40
% By weight. When the content is 25% by weight or less, it takes a long time to dissolve the iron oxide.
In general, the dissolution rate of iron oxide decreases, depending on the ratio of iron oxide and sulfuric acid used, the dissolution temperature, and the like.
【００１２】硫酸の使用割合について云えば、酸化鉄と
硫酸第一鉄の鉄の合量、即ち全鉄に対し、硫酸第一鉄中
の硫酸イオンと使用硫酸とを合わせて１．２５≦ＳＯ4
／Ｆｅ（モル比）≦１．５になるように調整使用する。
更に好ましくは１．３≦ＳＯ 4／Ｆｅ（モル比）≦１．
５である。１．２５以下の場合、酸化鉄の溶解率が充分
でなく、また酸化後の溶液安定性が悪く、使用すること
が困難となる。一方、１．５以上になると酸化後の硫酸
第二鉄溶液のｐＨが低くその用途が著しく制限される。Regarding the use ratio of sulfuric acid, iron oxide and
The total amount of iron in ferrous sulfate, that is,
Sulphate ion and sulfuric acid used in total 1.25 ≦ SOFour
/ Fe (molar ratio) ≦ 1.5.
More preferably 1.3 ≦ SO Four/ Fe (molar ratio) ≦ 1.
5 In the case of 1.25 or less, the dissolution rate of iron oxide is sufficient
Not to be used and the solution stability after oxidation is poor.
Becomes difficult. On the other hand, when it becomes 1.5 or more, sulfuric acid after oxidation
The low pH of the ferric solution severely limits its use.
【００１３】本発明の製造方法においては、上記各原料
を反応槽に投入するが、添加順序としては、先ず所定濃
度の硫酸を反応槽に投入し、次いで硫酸第一鉄を添加し
撹拌する。その後、酸化鉄を添加する。硫酸第一鉄溶液
に酸化鉄を加え、撹拌しながら硫酸を添加しても良い。
いずれにしても、三者の使用割合は上記の範囲とすべき
である。次いで反応温度に関しては７０℃以上が推奨さ
れ、より好ましくは９０℃以上である。最も好ましい反
応温度は沸点近傍である。勿論、加圧釜を使用すること
もできる。In the production method of the present invention, each of the above-mentioned raw materials is charged into a reaction tank. As for the order of addition, sulfuric acid having a predetermined concentration is first charged into the reaction tank, and then ferrous sulfate is added and stirred. Thereafter, iron oxide is added. Iron oxide may be added to the ferrous sulfate solution, and sulfuric acid may be added with stirring.
In any case, the usage ratio of the three should be in the above range. Next, regarding the reaction temperature, 70 ° C. or higher is recommended, and more preferably 90 ° C. or higher. The most preferred reaction temperature is near the boiling point. Of course, a pressure cooker can also be used.
【００１４】反応時間は、酸化鉄の種類、硫酸第一鉄
と、硫酸を含んだ溶液の濃度等他の反応条件により異な
り、一該に論じることはできないが一般には３時間で充
分である。これ以上の反応時間をかけても酸化鉄の溶解
率を向上させることはできない。以上の方法により酸化
鉄を充分溶解させたならば、放冷、水冷等により冷却し
て、反応溶液をフィルタープレス、遠心分離機等任意の
濾過機により濾過する。The reaction time varies depending on other reaction conditions such as the type of iron oxide, the concentration of a solution containing ferrous sulfate and sulfuric acid, and cannot be discussed in any way, but generally 3 hours is sufficient. Even if the reaction time is longer than this, the dissolution rate of iron oxide cannot be improved. After the iron oxide is sufficiently dissolved by the above method, the reaction solution is cooled by standing cooling, water cooling, or the like, and the reaction solution is filtered by an optional filter such as a filter press or a centrifuge.
【００１５】次いで、この濾液は２価の鉄を３価の鉄に
酸化するために酸化工程に付される。酸化方法は通常の
酸化方法と全く異なるところはない。酸化は酸素、空気
等による直接酸化の外、過酸化水素、二酸化マンガン、
塩素酸ソーダ等の酸化剤により、あるいは、チッソ酸化
物を触媒とした酸素、空気などにより行うことができ
る。以上の方法により酸化鉄の溶解率を高め、濃度の高
い安定な硫酸第二鉄溶液を製造することができる。以下
に実施例を挙げて更に詳記する。尚、特に断らない限り
％は全て重量％を示す。Next, the filtrate is subjected to an oxidation step to oxidize divalent iron to trivalent iron. There is no difference between the oxidation method and the ordinary oxidation method. Oxidation includes direct oxidation with oxygen, air, etc., hydrogen peroxide, manganese dioxide,
It can be carried out with an oxidizing agent such as sodium chlorate, or with oxygen or air using nitrogen oxide as a catalyst. By the above method, the dissolution rate of iron oxide can be increased, and a stable ferric sulfate solution having a high concentration can be produced. Hereinafter, the present invention will be described in more detail with reference to examples. All percentages are by weight unless otherwise specified.
【００１６】[0016]
【実施例】（実施例１）表１に記した量の酸化鉄、硫酸
第一鉄、硫酸、硫酸マグネシウム、水を四つ口フラスコ
に入れ、撹拌機、温度計、環流冷却器をセットした。２
４０ｒｐｍで撹拌し、下記の温度で３時間加熱溶解を行
った。５０℃まで冷却後、Ｎｏ．５Ｃ濾紙と珪藻土で濾
過を行った。その後、成分中に含まれる第一鉄（Ｆ
ｅ2+）を過酸化水素で酸化し、本発明の硫酸第二鉄溶液
を製造した。EXAMPLES (Example 1) The amounts of iron oxide, ferrous sulfate, sulfuric acid, magnesium sulfate and water shown in Table 1 were placed in a four-necked flask, and a stirrer, a thermometer and a reflux condenser were set. . 2
The mixture was stirred at 40 rpm, and heated and dissolved at the following temperature for 3 hours. After cooling to 50 ° C., Filtration was performed with 5C filter paper and diatomaceous earth. Then, ferrous iron (F
e 2+ ) was oxidized with hydrogen peroxide to produce a ferric sulfate solution of the present invention.
【００１７】酸化鉄の溶解率は、（使用乾燥酸化鉄重量
−乾燥溶解残渣重量）／（使用乾燥酸化鉄重量）×１０
０（％）で求めた。各原料使用量と溶解率を以下に示
す。使用した試薬は、α−ＦｅＯＯＨは関東化学製試
薬、ＦｅＳＯ4・７Ｈ2Ｏは関東化学製試薬、９５％Ｍｇ
ＳＯ4は和光純薬工業製試薬、７０％硫酸は和光純薬工
業製９８％硫酸を水で希釈し使用した。溶解温度は９０
℃である。The dissolution rate of iron oxide is (weight of dry iron oxide used−weight of dry dissolved residue) / (weight of dry iron oxide used) × 10
It was determined as 0 (%). The use amount and dissolution rate of each raw material are shown below. Reagents used were, alpha-FeOOH is Kanto Chemical reagents, FeSO 4 · 7H 2 O is produced by Kanto Chemical reagent, 95% Mg
SO 4 was a reagent manufactured by Wako Pure Chemical Industries, and 70% sulfuric acid was used by diluting 98% sulfuric acid manufactured by Wako Pure Chemical Industries with water. Melting temperature is 90
° C.
【００１８】[0018]
【表１】 [Table 1]
【００１９】表１より、全ＳＯ4／全Ｆｅ（モル比）が
低い場合であっても、また７０％硫酸由来ＳＯ4／酸化
鉄由来Ｆｅ（モル比）が低い場合であっても、硫酸第一
鉄を使用することにより酸化鉄の溶解率が向上すること
が判る。また同じ２価の可溶性硫酸塩であっても、硫酸
第一鉄と硫酸マグネシウムは、酸化鉄の溶解率向上に於
いて格段に差異のあることが判る。 （実施例２〜４）実施例１に使用した装置を用い、同様
の方法により硫酸第二鉄溶液を製造し、酸化鉄の溶解率
を測定した。その結果を表２に示す。使用した試薬は、
α−ＦｅＯＯＨは関東化学製試薬、ＦｅＳＯ4・７Ｈ2Ｏ
は関東化学製試薬特級、７０％硫酸は和光純薬工業製９
８％硫酸を水で希釈し使用した。溶解温度は９０℃であ
る。From Table 1, it can be seen that even when the total SO 4 / total Fe (molar ratio) is low or when the 70% sulfuric acid-derived SO 4 / iron oxide-derived Fe (molar ratio) is low, It turns out that the dissolution rate of iron oxide improves by using ferrous iron. Also, even with the same divalent soluble sulfate, ferrous sulfate and magnesium sulfate are found to have a marked difference in improving the solubility of iron oxide. (Examples 2 to 4) Using the apparatus used in Example 1, a ferric sulfate solution was produced in the same manner, and the dissolution rate of iron oxide was measured. Table 2 shows the results. The reagents used were
alpha-FeOOH is Kanto Chemical reagents, FeSO 4 · 7H 2 O
Is Kanto Chemical's special grade, 70% sulfuric acid is Wako Pure Chemical Industries 9
8% sulfuric acid was diluted with water and used. The dissolution temperature is 90 ° C.
【００２０】[0020]
【表２】 [Table 2]
【００２１】表２より、硫酸第一鉄由来Ｆｅ／（硫酸第
一鉄由来Ｆｅ＋酸化鉄由来Ｆｅ）（モル比）が０．１以
下になると溶解率が低下することが判る。 （実施例５〜８）実施例１に使用した装置を用い、同様
の方法により硫酸第二鉄溶液を製造し、酸化鉄の溶解率
を測定した。その結果を表３及び表４に示す。使用した
薬剤はα−Ｆｅ2Ｏ3は和光純薬工業製試薬、Ｆｅ3Ｏ4は
関東化学製試薬、７０％硫酸は和光純薬工業製９８％硫
酸を水で希釈し使用した。γ−Ｆｅ2Ｏ3及びβ−ＦｅＯ
ＯＨは新化学講座（丸善株式会社出版）に記された方法
に従って作製し使用した。溶解温度は７０℃である。From Table 2, it can be seen that the dissolution rate decreases when the ferrous sulfate-derived Fe / (ferrous sulfate-derived Fe + iron oxide-derived Fe) (molar ratio) is 0.1 or less. (Examples 5 to 8) Using the apparatus used in Example 1, a ferric sulfate solution was produced in the same manner, and the dissolution rate of iron oxide was measured. The results are shown in Tables 3 and 4. As the chemicals used, α-Fe 2 O 3 was a reagent manufactured by Wako Pure Chemical Industries, Fe 3 O 4 was a reagent manufactured by Kanto Kagaku, and 70% sulfuric acid was 98% sulfuric acid manufactured by Wako Pure Chemical Industries, diluted with water. γ-Fe 2 O 3 and β-FeO
OH was prepared and used according to the method described in Shinkagaku Koza (published by Maruzen Co., Ltd.). The dissolution temperature is 70 ° C.
【００２２】[0022]
【表３】 [Table 3]
【００２３】[0023]
【表４】 [Table 4]
【００２４】表３及び表４から明らかなように、硫酸第
一鉄を使用することにより各種酸化鉄の溶解率は著しく
向上する。As is clear from Tables 3 and 4, the use of ferrous sulfate significantly improves the dissolution rate of various iron oxides.
【００２５】[0025]
【発明の効果】本発明の硫酸第二鉄溶液の製造方法によ
ると、酸化鉄の溶解性が顕著に向上し、安価に且つ、工
業的に容易に硫酸第二鉄溶液を製造することができると
いう優れた効果を有する。According to the method for producing a ferric sulfate solution of the present invention, the solubility of iron oxide is remarkably improved, and the ferric sulfate solution can be produced at low cost and industrially easily. It has an excellent effect.
Claims (4)
て酸化鉄を溶解した後、２価の鉄を３価の鉄に酸化する
ことを特徴とする硫酸第二鉄溶液の製造方法。1. A method for producing a ferric sulfate solution, comprising dissolving iron oxide using a solution containing ferrous sulfate and sulfuric acid, and then oxidizing divalent iron to trivalent iron. Method.
第一鉄由来Ｆｅ／（硫酸第一鉄由来Ｆｅ＋酸化鉄由来Ｆ
ｅ）（モル比）≧０．１である請求項１記載の硫酸第二
鉄溶液の製造方法。2. The use ratio of iron oxide and ferrous sulfate is as follows: ferrous sulfate-derived Fe / (ferrous sulfate-derived Fe + iron oxide-derived F
2. The method for producing a ferric sulfate solution according to claim 1, wherein e) (molar ratio) ≧ 0.1.
合が１．２５≦ＳＯ 4／Ｆｅ（モル比）≦１．５である
請求項１または２記載の硫酸第二鉄溶液の製造方法。3. The ratio of total sulfuric acid to total iron during dissolution.
1.25 ≦ SO Four/ Fe (molar ratio) ≦ 1.5
The method for producing a ferric sulfate solution according to claim 1 or 2.
２または３記載の硫酸第二鉄溶液の製造方法。4. The method according to claim 1, wherein the melting temperature is 70 ° C. or higher.
4. The method for producing a ferric sulfate solution according to 2 or 3.
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|---|---|---|---|
| JP36364198A JP3999387B2 (en) | 1998-12-22 | 1998-12-22 | Method for producing ferric sulfate solution |
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| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| JP36364198A JP3999387B2 (en) | 1998-12-22 | 1998-12-22 | Method for producing ferric sulfate solution |
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| Publication Number | Publication Date |
|---|---|
| JP2000185921A true JP2000185921A (en) | 2000-07-04 |
| JP3999387B2 JP3999387B2 (en) | 2007-10-31 |
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ID=18479821
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| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| JP36364198A Expired - Fee Related JP3999387B2 (en) | 1998-12-22 | 1998-12-22 | Method for producing ferric sulfate solution |
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Cited By (4)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US6375919B1 (en) | 1999-07-08 | 2002-04-23 | Taki Chemical Co., Ltd. | Method for the manufacture of ferric sulfate solution and a water treatment agent using the same |
| JP2013527112A (en) * | 2010-05-17 | 2013-06-27 | テイオキサイド・ユーロプ・リミテツド | Method for producing ferrous sulfate monohydrate |
| GB2567655A (en) * | 2017-10-18 | 2019-04-24 | Industrial Chemicals Group Ltd | Polyferric sulphate solution |
| CN114466824A (en) * | 2019-09-30 | 2022-05-10 | 日铁矿业株式会社 | High-concentration iron-series flocculant and production method thereof |
-
1998
- 1998-12-22 JP JP36364198A patent/JP3999387B2/en not_active Expired - Fee Related
Cited By (7)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US6375919B1 (en) | 1999-07-08 | 2002-04-23 | Taki Chemical Co., Ltd. | Method for the manufacture of ferric sulfate solution and a water treatment agent using the same |
| JP2013527112A (en) * | 2010-05-17 | 2013-06-27 | テイオキサイド・ユーロプ・リミテツド | Method for producing ferrous sulfate monohydrate |
| GB2567655A (en) * | 2017-10-18 | 2019-04-24 | Industrial Chemicals Group Ltd | Polyferric sulphate solution |
| WO2019077302A1 (en) * | 2017-10-18 | 2019-04-25 | Industrial Chemicals Group Limited | Polyferric sulphate solution |
| GB2567655B (en) * | 2017-10-18 | 2020-05-20 | Industrial Chemicals Group Ltd | Polyferric sulphate solution |
| US11008221B2 (en) | 2017-10-18 | 2021-05-18 | Industrial Chemicals Group Limited | Polyferric sulphate solution |
| CN114466824A (en) * | 2019-09-30 | 2022-05-10 | 日铁矿业株式会社 | High-concentration iron-series flocculant and production method thereof |
Also Published As
| Publication number | Publication date |
|---|---|
| JP3999387B2 (en) | 2007-10-31 |
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