Sodium hydroxide reaction with hydrochloric acid

An example of a chemical reaction with a measurable energy change is the reaction of an acid and a base. In this activity, you will determine whether the reaction of hydrochloric acid (HCI) with sodium hydroxide (NaOH) absorbs or liberates heat. 

Salts are a common variety of ionic compound. A salt can form from the reaction between a base and an acid (both of which we cover in Chapter 16). For example, hydrochloric acid reacts with sodium hydroxide to form sodium chloride (a salt) and water ... 

One of the most common titrations of this type is the titration of hydrochloric acid, HC1, with sodium hydroxide, NaOH. If you remember from earlier, this is a neutralization reaction. However, you should also remember from earlier that in order for a complete neutralization to occur, the reaction must use appropriate stoichiometric ratios. When we first look at the process, we will do so with two solutions of known concentration, but you will see that this process can be used to determine the concentration of one of the solutions. 

If these two aqueous solutions are mixed, a chemical reaction takes place. The hydrogen ion from the hydrochloric acid combines with the hydroxide ion (OH-) from the sodium hydroxide to form water—the (1) following the formula for water shows that... 

Preparation of Antimony(V) Oxide. Treat 0.25 g of powdered metallic antimony with 2-3 ml of concentrated nitric acid in a porcelain howl while heating it in a water hath. Consider oxidation to he completed if a sample of the obtained white powder dissolved in an alkali will not reduce an ammonia solution of silver. When oxidation is completed, dilute the reaction mixture with water and separate the precipitate by decantation. Dry the precipitate in a water bath until it is dry, and then in a sand bath (275 °C). What is observed when it is treated with concentrated hydrochloric acid and a sodium hydroxide solution Write the equations of the reactions. How can antimony(lll) oxide be prepared ... 

Acid-base neutralization reactions are processes in which an acid reacts with a base to yield water plus an ionic compound called a salt. You might recall from Section 2.9 that we defined acids as compounds that produce H+ ions when dissolved in water and bases as compounds that produce OH- ions when dissolved in water. Thus, the driving force behind a neutralization reaction is the production of the stable covalent water molecule by removal of H + and OH- ions from solution. The reaction between hydrochloric acid and aqueous sodium hydroxide to yield water plus aqueous sodium chloride is a typical example ... 

Glucose (23.2 g., 0.12 mol), glycine (8.8 g, 0.12 mol), phosphate (Nal PO. l aq) (0 g or 16.1 g, 0.12 mol), and water were mixed to a total amount of 100 g. The pHs of the reaction-mixtures were adjusted, either with concentrated hydrochloric acid or concentrated sodium hydroxide solution to pH=3, 5.6, 7, or 9, compensating for the amount of solvent added. The reactions were carried out at 100°C in a 100 ml round-bottomed three-necked flask equipped with a reflux condenser. An oil bath equipped with a magnetic stirrer was applied as heating system. The start of the reaction (t=0) was defined as the... 

Manufacture (1) Chlorobenzene is nitrated with a mixture of sulphuric acid and nitric acid to produce dinitrochlorobenzene, which is synthesized to dinitro-sodium phenolate under reaction with sodium hydroxide. This is further changed to dinitrophenol with hydrochloric acid and then the dinitrophenol is nitrated by a mixture of sulphuric acid and nitric acid to trinitrophenol5 picric acid. (2) Phenol is mixed with cone, sulphuric acid and heated to obtain phenol-sulphonic acid. This is nitrated with a mixture of sulphuric acid and nitric acid to trinitrophenol. 

Neutralization reactions can also be looked at through conductivity tests. If a conductivity titration is performed with diluted hydrochloric acid and diluted sodium hydroxide solution (see E7.14), one would attain a certain minimum of electrical conductivity at the equivalence point, but it is not zero (see left diagram of Fig. 7.15) Na + (aq) ions and CF(aq) ions are left behind in the solution and are responsible for the minimal conductivity. The decrease in conductivity is often explained by the misconception that the absolute number of ions decreases and that by the usual ionic equation from an initial number of four ions, only two remain ... 

To a chemist, the term salt refers to the ionic product of a neutralization reaction, the positive ion coming from the base (K+ from KOH), and the negative ion coming from the acid (Cl from HCl). Potassium chloride, KCl, is the salt produced in the neutralization of hydrochloric acid and potassium hydroxide. Sodium nitrate, NaN03, is the salt produced in the neutralization of nitric acid, HN03, with sodium hydroxide, NaOH. The other product, water, is the covalent product of neutralization, formed by the combination of H+ from the acid, and OH , from, the base. Notice now the ions responsible for the properties of acids, H (aq), and the properties of bases, OH (aq), combine to form neutral water, HzO(I). This is how acids and bases destroy the properties of each other simultaneously. 

The tendency to form water is the second of the driving forces for reactions that we mentioned before. Any compound that produces OH ions in water reacts vigorousiy to form H2O with any compound that can furnish H" ions. For exampie, the reaction between hydrochloric acid and aqueous sodium hydroxide is represented by the following molecular equation ... 

Bassam Z. Shakhashiri, "Differences Between Acid Strength and Concentration," Chemical Demonstrations A Handbook for Teachers of Chemistry, Vol. 3 (The University of Wisconsin Press, Madison, 1989) pp. 136-139. The strength of three acids (acetic, hydrochloric, and sulfuric) are compared by reaction with sodium hydroxide. A companion procedure, involving base strength, is also included. 

Using these erythro aminoalcohols we succeeded in the stereoselective synthesis of trans thiazolidinones. In Scheme 3, the convenient method to give trans thiazolidinones in an excellent yield is shown (IQ). We found that the erythro dithiocarbamates which were obtained by the reaction with erythro aminoalcohols, carbondisulfide and benzylbromide were easily cyclized to trans thiazolidinones stereoselectively by the reaction with thionylchloride involving the elimination of the chlorosulfonyl group with inversion. The cyclized intermediates were treated with hydrochloric acid followed by sodium hydroxide to give trans thiazolidinones, retaining the stereochemistry. Furthermore, the treatment of the dithiocarbamates with concentrated hydrochloric acid in ethanol at reflux temperature provided a short-cut pass to give trans thiazolidinones. We applied this method for the synthesis of the carbon-14-labeled hexythiazox at the 5-position of the thiazolidinone nucleus. 

Neutralization reactions are described by double-replacement equations, although it might not seem that way at first glance. The water molecule forms when the hydrogen ion from the acid combines with the hydroxide ion from the base. The doublereplacement character of the equation becomes clear if you write the formula of water as HOH rather than H2O. For the neutralization of hydrochloric acid by solid sodium hydroxide, the equation is... 

The whole mixture is determined after reaction with sodium hydroxide in excess for 30 minutes. In these conditions, all the derivatives are quantitatively transformed into the lactate ion. It does not exhibit a sufficiently basic character to be protonated by hydrochloric acid (pK value of lactic acid 3.86), the titrant that permits us to determine the sodium hydroxide excess. 

By analogy, ammonium salts should behave as acids in liquid ammonia, since they produce the cation NH4 (the solvo-cation ), and soluble inorganic amides (for example KNHj, ionic) should act as bases. This idea is borne out by experiment ammonium salts in liquid ammonia react with certain metals and hydrogen is given off. The neutralisation of an ionic amide solution by a solution of an ammonium salt in liquid ammonia can be carried out and followed by an indicator or by the change in the potential of an electrode, just like the reaction of sodium hydroxide with hydrochloric acid in water. The only notable difference is that the salt formed in liquid ammonia is usually insoluble and therefore precipitates. 

Sodium hydroxide solution cannot be used at this stage since it may produce benzoic acid by the Cannizzaro reaction (Section IV,123) from any unchanged benzaldehyde. If, however, the reaction mixture is diluted with 3-4 volumes of water, steam distilled to remove the unreacted benzaldehyde, the residue may then be rendered alkaline with sodium hydroxide solution. A few grams of decolourising carbon are added, the mixture boiled for several minutes, and filtered through a fluted filter paper. Upon acidifying carefully with concentrated hydrochloric acid, cinnamic acid is precipitated. This is collected, washed and purified as above. 

The cleavage products of several sulfonates are utilized on an industrial scale (Fig. 3). The fusion of aromatic sulfonates with sodium hydroxide [1310-73-2J and other caustic alkalies produces phenohc salts (see Alkylphenols Phenol). Chlorinated aromatics are produced by treatment of an aromatic sulfonate with hydrochloric acid and sodium chlorate [7775-09-9J. Nitriles (qv) (see Supplement) can be produced by reaction of a sulfonate with a cyanide salt. Arenesulfonates can be converted to amines with the use of ammonia. This transformation is also rather facile using mono- and dialkylamines. 

Into a stirred, cooled (10°-15°C) solution of 26.2 grams (0.1 mol) of 2-amino-5-chlorobenzo-phenone (3-oxime in 150 ml of dioxane were introduced in small portions 12.4 grams (0.11 mol) of chloracetyl chloride and an equivalent amount of 3 N sodium hydroxide. The chlor acetyl chloride and sodium hydroxide were introduced alternately at such a rate so as to keep the temperature below 15°C and the mixture neutral or slightly alkaline. The reaction was completed after 30 minutes. The mixture was slightly acidified with hydrochloric acid, diluted with water and extracted with ether. The ether extract was dried and concentrated in vacuo. Upon the addition of ether to the oily residue, the product, 2-chloroacetamido-5-chlorobenzophenone (3-oxime, crystallized in colorless prisms melting at 161°-162°C. 

Thebaine is dissolved in aqueous formic acid and treated with 30% HjO neutralization with aqueous ammonia gives 14-hydroxycodeinone. It is hydrogenated to give oxycodone. 90 ml of concentrated hydrobromic acid are heated to 90°C. 9 grams of 14-hydroxydi-hydrocodeinone (oxycodone) are then added under stirring and the mixture is quickly heated to 116°C and kept at this temperature under reflux condenser for 20 minutes, with continued stirring. The resulting brown solution Is diluted with about 90 ml of water and chilled with ice. Aqueous 10% sodium hydroxide solution is now added to alkaline reaction and the liquid is extracted 3 times with 100 cc portions of chloroform. The layers are separated and the aqueous phase is fiitered and acidified by the addition of concentrated aqueous hydrochloric acid, treated with charcoal and filtered. 

A solution of 100 g (1.7 mols) of isopropylamine in 60 cc of water was stirred into a solution of 4-hydroxyphenoxypropylene oxide. After the exothermic reaction has subsided, the reaction mixture was heated for two hours at 60Thereafter, the aqueous ethanol was distilled off, and the solid residue was dissolved in aqueous hydrochloric acid comprising more than the theoretical stoichiometric molar equivalent of hydrochloric acid. The aqueous acid solution was extracted with ether and was then made alkaline with sodium hydroxide, whereby a solid crystalline precipitate was formed which was filtered off and dried over phosphorus pentoxide. The product was 1,1 -(4 -hvdroxvphenoxv)-2-hvdroxv-3-isopropylamino-pro-pane. Its hydrochloride had a melting point of 166°Cto 169°C. 

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