US2160391A - Bleaching process and composition - Google Patents

Bleaching process and composition Download PDF

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Publication number
US2160391A
US2160391A US65326A US6532636A US2160391A US 2160391 A US2160391 A US 2160391A US 65326 A US65326 A US 65326A US 6532636 A US6532636 A US 6532636A US 2160391 A US2160391 A US 2160391A
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United States
Prior art keywords
magnesium
silicate
solution
soluble
bleach
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Expired - Lifetime
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US65326A
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English (en)
Inventor
Joseph S Reichert
Wilbie S Hinegardner
Howard L Potter
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EIDP Inc
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EI Du Pont de Nemours and Co
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Priority to US65326A priority Critical patent/US2160391A/en
Priority to DEP74701D priority patent/DE706831C/de
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    • C—CHEMISTRY; METALLURGY
    • C11—ANIMAL OR VEGETABLE OILS, FATS, FATTY SUBSTANCES OR WAXES; FATTY ACIDS THEREFROM; DETERGENTS; CANDLES
    • C11D—DETERGENT COMPOSITIONS; USE OF SINGLE SUBSTANCES AS DETERGENTS; SOAP OR SOAP-MAKING; RESIN SOAPS; RECOVERY OF GLYCEROL
    • C11D3/00—Other compounding ingredients of detergent compositions covered in group C11D1/00
    • C11D3/39—Organic or inorganic per-compounds
    • C11D3/3947—Liquid compositions
    • D—TEXTILES; PAPER
    • D06—TREATMENT OF TEXTILES OR THE LIKE; LAUNDERING; FLEXIBLE MATERIALS NOT OTHERWISE PROVIDED FOR
    • D06L—DRY-CLEANING, WASHING OR BLEACHING FIBRES, FILAMENTS, THREADS, YARNS, FABRICS, FEATHERS OR MADE-UP FIBROUS GOODS; BLEACHING LEATHER OR FURS
    • D06L4/00—Bleaching fibres, filaments, threads, yarns, fabrics, feathers or made-up fibrous goods; Bleaching leather or furs
    • D06L4/10—Bleaching fibres, filaments, threads, yarns, fabrics, feathers or made-up fibrous goods; Bleaching leather or furs using agents which develop oxygen
    • D06L4/12—Bleaching fibres, filaments, threads, yarns, fabrics, feathers or made-up fibrous goods; Bleaching leather or furs using agents which develop oxygen combined with specific additives

Definitions

  • This invention relates to a process of bleachbaths in use prior to our discovery have usually ing and to bleach baths containing certain staoperated'with precipitated magnesium silicate bilizers. More particularly, it relates to the therein. preparation and use of bleach baths which con- It is one of the objects of this invention to tain magnesium compounds as stabilizers. overcome the objectionable defect of insolubility Magnesium compounds have been used as stawhen magnesium silicate is utilized as the stabibilizers for bleach baths consisting essentially lizing agent for bleach baths comprising dilute of dilute solutions of hydrogen peroxide or similar hydrogen peroxide solutions.
  • bleach baths method known to us of practicing the improved comprising dilute solutions of hydrogen peroxide process and preparing the improved compositions. 25 which are alkaline in reaction are employed.
  • curve A represents the Due to the limited solubility of magnesium silisolubility at room temperature of magnesium as cate which is formed in the solution when it conmagnesium silicate in dilute solutions of hydrogen tains a soluble silicate, these bleach baths have peroxide ranging in volume concentration from usually contained the stabilizing agent in the about 0.25 volume to 10 volume under various 30 form of an insoluble precipitate.
  • the volume remove solid particles but, nevertheless, the presconcentration of a dilute solution of hydrogen ence of insoluble particles in bleach baths has peroxide is, of course, the number of volumes of been regarded as distinctly unsatisfactory and oxygen gas, measured at 0 C. and 760 mm. of undesirable. mercury'pressure, which will be evolved from one Commercial bleaching solutions consisting esvolume of the solution at 25 C.
  • the solubility 45 usually have a pH falling between about 9.0 and of magnesium, as magnesium silicate, at room 13.0.
  • the pH of such temperature, in dilute solutions of hydrogen persolutions is about 10.0 or 10.5.
  • oxide having a pH of 2 or below is in excess of 0.4 we have found that the solubility of magnesium gram magnesium per liter.
  • the solubility of magnesium as 50 and, at room temperature does not exceed about magnesium silicate is only about 0.025 gram mag- 0.025 g. magnesium metal per liter. Ordinarily nesium per liter.
  • magnesium silicate has been indicated in terms of grams of magnesium, as magnesium silicate
  • magnesium silicate is ordinarily a salt of complex, variable and changing constitution and under these circumstances greater accuracy results from treating the solubility on the basis of the Mg content of the bath.
  • a stabilizing agent ordinarily a soluble salt of magnesium S'LlCho as magnesium chloride, magnesium nitrate, magnesium acetate, or magnesium carbonate, is caused to react in situ with a soluble silicate, usually sodium silicate, present in .the bath.
  • magnesium sulfate magnesium carbonate
  • magnesium nitrate magnesium citrate
  • magnesium silicate it is necessary to prepare a solution in which the silicate is completely dissolved. This may be done by preparing a bath containing hydrogen peroxide or other per-compound in the desired concentration, treating the solution in accordance with our solubilizing step and then dissolving magnesium silicate in the desired amount in this solution. Or, if desired, magnesium silicate may be brought into solution in a separate sample using our solubilizing step and this solution then added to the bleach bath containing the soluble silicate.
  • solubilizing step which will hereinafter be described more fully, be employed before the soluble silicate and magnesium salt are brought into contact under conditions wherein precipitation might occur. other words it is necessary to avoid any opportunity for the precipitation of magnesium silicate prior to the use of our solubilizing step.
  • the solubility of magnesium silicate cannot be increased by the use of our process. Accordingly the exact order of steps is important and we have found it essential in preparing our solutions first to add the magnesium salt to the bleach bath, then to adjust the pH in accordance with our solubilizing step, and finally add the sodium silicate or other soluble silicate, this final step serving at the same time to adjust the alkalinity to the desired pH value.
  • a commercial solution of hydrogen peroxide such as one of 100 volume concentration sold commercially under the trade-mark name Albone C may be first diluted with water until a solution of the desired volume concentration is obtained. For most bleaching applications this will be a concentration somewhere between 0.25 volume and 10 volumes. Next a soluble magnesium salt, which may be any one of the magnesium salts previously specified or may be magnesium silicate in solution, is added. The amount of magnesium salt should be sufiicient so that the amount of magnesium in the form of magnesium silicate in the bleach bath after the addition subsequently of. the soluble silicate, will be from 0.1 to 0.125 lb. of Mg per 100 gallons of solution.
  • the amounts which should be added are specified as amounts of Mg in the form of its salts. If the relatively inexpensive magnesium salt, magnesium sulfate, MgSO-a'TI-IzO, is used, it is necessary for a magnesium content of from 0.1 to 0.125 lb. per 100 gallons to add approximately 1 to 1.25 lbs. of magnesium sulfate. When other magnesium salts are utilized the amount of salt necessary can be calculated from its magnesium content.
  • This step which is an essential element of our invention, involves the addition of an inorganic acid such as hydrochloric, nitric or sulfuric acids to the solution in amount sufficient to render it distinctly acid in reaction.
  • an inorganic acid such as hydrochloric, nitric or sulfuric acids
  • the solubility of magnesium as magnesium silicate in bleach v baths is changed as indicated by curves A and B on the drawing.
  • distinctly acid in reaction is meant that the pH of the solution should be about 2.5 or below. This pH' value is given merely as illustrative, however, as in practice enough acid would be added to make the solution distinctly or even strongly acid. While a pH of 2.5 cannot be termed strongly acid it may be regarded as distinctly acid.
  • NaHSQaHzO NaHSQaHzO is suitable.
  • Other inorganic salts may also be used, and as they are exactly equivalent to the acids they should be added in suflicient amount to render the hydrogen peroxide solution containing magnesium distinctly acid in reaction.
  • the pH should be adjusted to about 2.5 or below by the addition of the salt.
  • the alkalinity of the solution is next adjusted by the addition of an alkaline material.
  • an alkaline material ordinarily we prefer to add sodium silicate atthis stage, as this soluble silicate serves at the same time to reduce the acidity, since it is alkaline in reaction, and to add the requisite amount of silicate to the bleach bath.
  • other soluble silicates could be used in place of the sodium silicate, or if desired, the pH may be first adjusted by the use of some other alkaline materials such as caustic soda or soda ash.
  • the alkalinity is adjusted so that it falls somewhere within the range desired in bleaching which, for most bleaching purposes, is somewhere between 9 and 13, and for the great majority of bleaching applications within the range 10.0 and 11.5.
  • Curve B represents the solubility of magnesium in the form of magnesium silicate in the bleach bath.
  • magnesium may be present in amounts as high as 0.125 lb. magnesium as magnesium silicate per 100 gallons of solution without precipitation occurring. This is attributable to the novel solubilizing step;
  • the order of addition of the material to the hydrogen peroxide solution is also important and it is necessary to add the magnesium prior to the addition of the solubilizing agent and finally add the desired amount of soluble silicate to the solution. If the order of steps is changed precipitation will occur and it will be impossible to increase the solubility as desired.
  • Example 1 To 100 gallons of water sufiicient 100 volume hydrogen peroxide solution was added to yield a bath having a concentration of 25 volumes, and to this bath 9. lb. of magnesium sulfate, MgSO4.7H2O, was added. Approximately pound of concentrated sulfuric acid (95.5 to 96.5% H2804) were next added. The solution was thoroughly mixed and its pH determined. The pH value was approximately.2.5 as observed by the colorimetric method.
  • a process for preparing solutions of hydrogen peroxide containing large amounts of dissolved magnesium silicate which comprises the steps of adding a soluble magnesium compound to a solution of hydrogen peroxide, adjusting the pH of the solution to 2.5 or below, adding a soluble silicate thereto, and adjusting the pH so that said solution is alkaline in reaction.
  • a process for preparing solutions of hydrogen peroxide containing large amounts of magnesium silicate in solution which comprises adding a soluble magnesium compound to a solution of hydrogen peroxide, adding a mineral acid in amount sumcient to adjust the pH of said solution to 2.5 or below, subsequently adding a soluble silicate thereto, and adjusting the pH of said solution so that it is alkaline in reaction.
  • a process for preparing solutions of hydrogen peroxide which when they are rendered alkaline in reaction will retain amounts of magnesium silicate up to those equivalent to 0.14 gram of magnesium as magnesium silicate per liter without precipitation developing therein which comprises the steps of adding a magnesium salt to a solution of hydrogen peroxide, adjusting the pH of said solution to a value of 2.5 or below, and adding thereto a soluble silicate.
  • a process for preparing bleach baths comprising oxygen-evolving compounds which will retain in solution amounts of magnesium silicate up to those equivalent to 0.14 gram of magnesium as magnesium silicate per liter without precipitation developing therein when said solutions are rendered alkaline in reaction which comprises the steps of adding a magnesium compound to a bleach bath containing an oxygen-evolving compound, adjusting the pH of said solution to a value of 2.5 or below, and subsequently adding thereto a soluble silicate.
  • a process for preparing bleach baths comprising active oxygen yielding compounds which will retain in solution amounts of magnesium silicate up to those equivalent to 0.1-4 gram of magnesium as magnesium silicate per liter without precipitation developing therein when said baths are rendered alkaline and used for bleaching which comprises the steps of adding a soluble magnesium salt to a bleach bath, adjusting the pH of said bath to a value of 2.5 or below, and then adding thereto a soluble silicate.
  • a clear solution of hydrogen peroxide containing substantially no undissolved stabilizing agents said solution having a volume concentration from 0.25 volume to 10 volume, having a pH within the range 9 to 14, and containing dissolved therein magnesium silicate in amounts equivalent to from 0.025 gram magnesium as magnesium silicate to 0.14 gram of magnesium as magnesium silicate, both of these amounts being per liter of solution.
  • a clear solution of hydrogen peroxide containing substantially no undissolved stabilizing agents having a pH within the limits 9 to 14 and containing dissolved therein magnesium silicate in amounts ranging from that equivalent to 0.025 gram of magnesium as magnesium silicate per liter of solution to 0.14 gram magnesium as magnesium silicate per liter of solution.
  • a process for preparing solutions of hydrogen peroxide having a pH ranging from 9 to 14 and containing amounts of magnesium silicate up to and including 0.14 gram of magnesium as magnesium silicate per liter of solution which comprises the steps of adding a magnesium compound to said solution, adding to said solution an acidic material selected from the group which consists of mineral acids and sodium acid sulfate in amount sufficient to impart to said solution a pH of 2.5 or below thereby rendering magnesium silicate more soluble therein, adding a soluble silicate thereto, and then adjusting the pH of said solution to any desired value, within the range 9 to 14.

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  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Inorganic Chemistry (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Oil, Petroleum & Natural Gas (AREA)
  • Wood Science & Technology (AREA)
  • Organic Chemistry (AREA)
  • Textile Engineering (AREA)
  • Detergent Compositions (AREA)
US65326A 1936-02-24 1936-02-24 Bleaching process and composition Expired - Lifetime US2160391A (en)

Priority Applications (2)

Application Number Priority Date Filing Date Title
US65326A US2160391A (en) 1936-02-24 1936-02-24 Bleaching process and composition
DEP74701D DE706831C (de) 1936-02-24 1937-02-19 Verfahren zur Herstellung von alkalischen, Perverbindungen und Magnesiumsilicat enthaltenden Bleichflotten

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Cited By (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US2612898A (en) * 1952-10-07 Cleaning of manufactured jewelry
US2838459A (en) * 1955-02-01 1958-06-10 Pennsalt Chemicals Corp Stabilization of solutions containing peroxygen compounds
US3287083A (en) * 1961-06-30 1966-11-22 Bancroft & Sons Co J Formaldehyde modification of cellulose catalyzed by a lewis acid salt and formic acid generated in situ by a peroxide
RU2500613C2 (ru) * 2011-12-16 2013-12-10 Открытое акционерное общество "Корпорация "Росхимзащита" (ОАО "Корпорация "Росхимзащита") Способ стабилизации щелочного раствора пероксида водорода

Cited By (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US2612898A (en) * 1952-10-07 Cleaning of manufactured jewelry
US2838459A (en) * 1955-02-01 1958-06-10 Pennsalt Chemicals Corp Stabilization of solutions containing peroxygen compounds
US3287083A (en) * 1961-06-30 1966-11-22 Bancroft & Sons Co J Formaldehyde modification of cellulose catalyzed by a lewis acid salt and formic acid generated in situ by a peroxide
RU2500613C2 (ru) * 2011-12-16 2013-12-10 Открытое акционерное общество "Корпорация "Росхимзащита" (ОАО "Корпорация "Росхимзащита") Способ стабилизации щелочного раствора пероксида водорода

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Publication number Publication date
DE706831C (de) 1941-06-06

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