Application Information

This drug has been submitted to the FDA under the reference 083130/001.

Names and composition

"AMMONIUM CHLORIDE" is the commercial name of a drug composed of AMMONIUM CHLORIDE.

Answered questions

Classify each of the following pure substance or a mixture?
ammonium chloride silica gasoline iodine crystals Asked by Damon Faso 6 months ago.

Ammonium Chloride - No, there are impurities in even reagent it is typically not a pure substance. It depends on the assay, see? Silica - Is a broad mixture of different Silcon compounds, generally called - Sand. Not pure in nature, but highly purified by electronics companies under extreme conditions. Is a mixture. Gasoline - No, not a pure substance. It generally contains WATER and a mixture of different hydrocarbons and additives. A mixture. Iodine Crystals - ONLY if "sublimed" and purified, generally yes a pure substance, but will have traces of impurities. I would say sublimed crystals are pure. Answered by Alejandra Colston 6 months ago.

Is ammonium chloride antibacterial?
Asked by Denita Rosenbluth 6 months ago.

Ammonium chloride is used as an expectorant in cough medicine. Its expectorant action is caused by irritative action on the bronchial mucosa. This causes the production of excess respiratory tract fluid which presumably is easier to cough up. Ammonium salts are an irritant to the gastric mucosa and may induce nausea and vomiting. Ammonium chloride is used as a systemic acidifying agent in treatment of severe metabolic alkalosis, in oral acid loading test to diagnose distal renal tubular acidosis, to maintain the urine at an acid pH in the treatment of some urinary-tract disorders Ammonium Chloride is also used as a diuretic in forced acid diuresis. I don't think so. Answered by Lura Robichaux 6 months ago.

yes its is sorta cause its used to a liquid additive for humidifiers Answered by Darin Gilberti 6 months ago.

What are the important pharmaceutical and industrial applications for ammonium chloride?
Asked by Hana Lofgreen 6 months ago.

Ammonium chloride is sold in blocks at hardware stores for use in cleaning the tip of a soldering iron and can also be included in solder as flux. Other uses include a feed supplement for cattle, in hair shampoo, in textile printing, in the glue that bonds plywood, as an ingredient in nutritive media for yeast, in cleaning products, and as cough medicine. Its expectorant action is caused by irritative action on the bronchial mucosa. This causes the production of excess respiratory tract fluid which presumably is easier to cough up. It is also used in an oral acid loading test to diagnose distal renal tubular acidosis. In several countries sal ammoniac is used to spice up liquorice-type dark sweets (Finland's salmiakki, Sweden's lakrisal, the Netherlands' zoute drop and the Danish Dracula Piller are popular examples), and as a flavoring for vodkas. Ammonium chloride is also used for contact explosives, diuretic and systemic acidifying agent. It is used in the treatment of severe metabolic alkalosis, to maintain the urine at an acid pH in the treatment of some urinary-tract disorders or in forced acid diuresis. Ammonium salts are an irritant to the gastric mucosa and may induce nausea and vomiting. Biological applications include using it as an energy source for microbiological growth of organisms. The zero point of Fahrenheit is determined by placing the thermometer in a mixture of ice, water, and ammonium chloride. Also used: to luster cotton, as a flux in tin coating and galvanizing, in fertilizers, in safety explosions and in dying and tanning. Used in a ~5% aqueous solution to work on oil wells with clay swelling problems. Answered by Tama Pulgarin 6 months ago.

Ammonium Chloride Uses Answered by Francisco Mick 6 months ago.

The Kb for ammonia is 1.8*10^-5. What is the pH of a 0.1M solution of ammonium chloride?
Please show me how to do this, I'm very lost on this question. Asked by Cesar Bogen 6 months ago.

Ammonium chloride is soluble in water. The chloride ion does not hydrolyze, but the ammonium ion does. NH4Cl(s) --> NH4+ + Cl- NH4+ + H2O <==> NH3 + H3O+ ....... Ka = ??? Ka = Kw / Kb = 1.00x10^-14 / 1.8x10^-5 = 5.56x10^-10 Ka = [NH3] [H3O+] / [NH4+] 5.56x10^-10 = x² / 0.10 x = 7.46x10^-6 H3O+ = 7.46x10^-6M pH = -log[H3O+] = 5.13 Comments: We're given Kb for ammonia, but it is ammonium ion which is reacting with water. Ammonium ion is acting as an acid and donating a proton to water. Therefore, we need the Ka of ammonium ion. Ammonia is the conjugate base of ammonium ion. The product of the Ka of an acid, and the Kb of the conjugate base is Kw. Kw = Ka x Kb. Therefore, it is a simple matter to determine Ka for NH4+. The concentration of H3O+ and NH3 will be the same, and are unknown. Therefore, they are each represented by x. The concentration of NH4+ is 0.1M and the very slight amount of it which dissociates is negligible. Therefore, we can say that (0.1 - x) = 0.1 ============ Follow up ============== Whoa! Back the boat up. In fact, Fred is operating at the wrong end of the boat. We're talking about a solution of ammonium chloride. A solution of ammonium chloride is slightly acidic, not basic. The pH must be *less* than 7. Fred has done the calculation as if there were a 0.1M solution of ammonia, not ammonium chloride. Answered by Vinita Survis 6 months ago.

NH3(aq) + H20 = NH4+(aq) plus OH-(aq) Kb = 1.8 x l0^-5 = (NH4+)(0H-) over (NH3) Let X = the concentration of NH4+) and also (OH-) With this small Kb value, we can ignore the loss from the .10 Molar NH3 and leave its concentration as .l0 molar Kb = 1.8 x l0^-5 = (X)(X) over(.10) 1.8 x l0^-6 = X^2 X = .0013 moles per liter (0H-) pOH = -log(0H) = -log ( . 0013) 2.89 14 minus the pOH = pH 14 minus 2.89 = a pH of 11.11 . Answered by Lulu Betran 6 months ago.

Hydrate ratio ammonium chloride!?
I can't find the ratio of water to ammonium chloride hydrate. Does such a compound exist? Like when ammonium chloride dissolves in water..if anyone SERIOUS can tell me the ratio, I will give 10 points. Asked by Candance Brehant 6 months ago.

Do you mean just hydrated ammonium chloride? Not when it dissolves in water; that'd be NH4Cl SOLUTION. I have a 1lb jar of ammonium chloride at home. It seems rather passive to moisture, and I have never seen it mentioned anywhere that it even does form a hydrate. So to answer, AFAIK ammonium chloride does not form a hydrate, just like table salt (NaCl) or KCl won't form hydrates either. Answered by Narcisa Fitzgibbons 6 months ago.

Lancenigo di Villorba (TV), Italy YOUR REMARKS You put several spoons of ammonium chloride in an amount of water standing in a glass beaker, hence you mix it by means of a glass rod or a magnetic anchor. You may note a diminution of mixture's temperature. WHY THAT? Temperature falls down because ammonium chloride have two different energy's bonds depending on it stands as crystal form or its aqueous solutions. Since the latter is LOWER THAN the former one, the process needs energy supply. This is a common example of ENDOTHERMIC PHENOMENON. THERMODYNAMICS FUNDAMENTS At the endings of XIX century, an american physician (J. W. Gibbs) began an imponent study on the evolutions of many chemical phenomena. He developed a new themodynamics property, a VERY POWERFUL tool involved in correlations and predictions of many and many physico-chemical events. I tell about "H that is Enthalpy", a thermodynamics potential as "E that is Inner Energy" it is. At the time, the scientists stated the "First Principle of Thermodynamics" among its applications there is the case of "thermodynamics systems" maintaining their "E" since they cannot exchange energy in its usual forms, e.g. heat and mechanical work. Developing this result, Gibbs stated that any REVERSIBLE PROCESSES have "H" 's changes determined by its mass transfers when it is led in ISOBARIC and ADIABATIC conditions. More completely, he could describe differential of "H" as it have a writing interesting changes of main physico-chemical variables, e.g. pressure, entropy and molar amounts of reaction's actors. WHAT IT HAPPENS? In your experiment, I may assume you get DILUTE SOLUTIONS that are it run a REVERSIBLE PROCESS (e.g. few salt in water leads to small irreversibilities). In this manner, I assume that there will be not any changes of pressure, there will be not any heat exchanges. Hence, the "H" 's differential is not depending on pressure or entropy (e.g. reversible hypotheses). On the other hand, the solutions is built by adding salt to water. Hence, I evaluate the "Energy's Bonds that is Specific Enthalpy" of ammonium chloride in crystal form and the "energy's bonds" of 1 M aqueous solution of the same compound. The literature report the former state of ammonium chloride having a GREATER energy's bond THAN ammonium solution's one. Finally, in the differential writing I find an algebraic negative difference which is similar to the "thermal capacity measured at constant pressure". Since the latter quantity is related to temperature changes of the solution, I shown why temperature falls down. I hope this helps you. Answered by Moses Thrill 6 months ago.

What will be the effect of pressure on ammonium chloride?
As it is sublimable, will solid Ammonium chloride turn directly into its gaseous state in decreasing pressure and vice- versa. what if the the pressure is intermediate? Asked by Elvis Marcisak 6 months ago.

The "sublimation" of ammonium chloride is an equilibrium system between the original solid and the two gases formed: ammonia and hydrogen chloride. If the "sublimation" is completed inside a closed system, the sublimation will proceed based on the equilibrium constant for the reaction. Note that this is a chemical reaction and not technically a sublimation process. NH4Cl(s) + energy <---> NH3(g) + HCl(g) K = P(NH3) x P(HCl) Decreasing the overall pressure will not have an effect on the equilibrium partial pressures present in the container and will not affect the equilibrium established (as long as the partial pressure of the two gases in left unaffected). If the partial pressures of the two gases are lowered, it will cause a shift in the equilibrium to the right, causing more gas to be produced in order to reestablish the equilibrium position at the same temperature. However, if the reaction is done in a open container, the thermal decomposition of the solid will continue since the equilibrium partial pressures can never be established since the gases will diffuse out of the container. How fast this will occur depends on the amount of energy present within the system. Whether or not the overall pressure change in the open container would have an effect would most likely be minimal since this is a chemical process. For a compound that does not undergo thermal decomposition as ammonium chloride does, like carbon dioxide, if one lowers the pressure at the same temperature, it could effect the position of the equilibrium if the vapor pressure of the solid is reached at that temperature. One would have to look at the phase diagram of the substance in question to determine what pressure is needed to maintain the substance as a gas or when will the gas deposit to form the solid. This occurs at a specific pressure at any given temperature based on where the line is present between the gas and solid phases; this is sometimes called the sublimation curve. If solid carbon dioxide is brought into standard temperature and standard pressure conditions, it will sublime once the temperature of the solid reaches -78.5C because that is the temperature at which the solid vapor pressure equals atmospheric pressure (1 atm). If the solid carbon dioxide was kept at -78.5C at a pressure higher than 1 atm, and the pressure was reduced to below 1 atm, the same sublimation would be observed. Answered by Kimiko Goldermann 6 months ago.

anti getting previous lotions dehydrate your epidermis, so that you employ moisturers as " Garnier " to carry water content cloth. this in basic terms tallys the getting previous cream. your anti dandruff shampoo motives harm for your scalp, in case you employ any bathroom soaps 4 ur face, then ur epidermis may come as flakes after a era of two-3 months. Answered by Irwin Dobrich 6 months ago.

How to make ammonium chloride at home+?
hello. Iwould like to make ammonium chloride at home but here I live its difficult to get ammonia. What is the alternative? Asked by Jolanda Nikocevic 6 months ago.

There isn't any really good alternative to ammonia. I don't know where you live, but probably solutions of ammonia in water are available in most countries as a household product. In the western world, it's sold in supermarkets as "household ammonia". This is just ammonium hydroxide (ammonia dissolved in water). If you can find it, you want the clear variety, not the sudsy or scented. If you can find the ammonia, the other component you need is hydrochloric acid. Again, in the western world this is sold in hardware stores and outlets such as Menard's and Home Depot as Muriatic Acid. Be sure to get the GENUINE article, since there are some substitutes that would not work. Ammonium chloride can be produced by reacting the two substances described above. There are some hazards however: You need to wear protective clothing and eye-wear. You need to have a hose or other source of drenching water readily available in case you get the material on yourself. You need to work outdoors and stay upwind. And, you need to have patience in the process. To do the reaction, you need to very slowly add the acid to the ammonia (in that order) with constant stirring. Use plastic or stainless steel containers and stirrer. If you have an acid-base indicator available (litmus or phenolphthalein for example) you can tell when the balance has been reached by the color change. If not, it's better to have an excess of the ammonia (the mixture will still smell like ammonia at the end point). After neutralizing the ammonia with the appropriate amount of acid, you need to remove the excess water. You can do this by boiling it away - this will also remove any excess ammonia (which is why I said it's better to stop when ammonia is still in excess). Once you get it cooked down to a concentrated solution, let it cool and ammonium chloride should crystallize. If not, or if you have remaining liquid, let it stand in the open to evaporate excess water, to get more ammonium chloride crystals. Answered by Velma Vannatten 6 months ago.

How To Make Ammonium Chloride Answered by Phoebe Thoams 6 months ago.

You might want to start with NH4NO3 (ammonium nitrate). It is a white crystalline solid at room temperature and standard pressure. It is commonly used in agriculture as a high-nitrogen fertilizer. Be aware, however, that fertilizer has been used to make bombs and it is likely that, if you buy a lot of it, you will have to answer questions from the local constabulary. Answered by Devorah Lamon 6 months ago.

What kind of bond does ammonium chloride have?
Is ammonium chloride and ionic bond or a covalent bond? I've heard both so far on the internet. Asked by Darcy Bloomer 6 months ago.

It is ionic. Ammonium-anything is ionic, because ammonium implies an NH4+ ion. Although it does have a "molecular" part in it - all polyatomic ions, such as NH4+, CO3-, etc. are molecular compounds that are "imbalanced" because they have too many or too few electrons - it is regarded as ionic because the main bond is between a cation, NH4+, and an anion, Cl-. AmmoniA is the gas NH3, a completely molecular compound. When in water, the gas NH3 forms NH4+ ions by stealing an H from the water and leaving it as OH-. The technical term for NH4+ ions and OH- ions floating around in water is NH4OH (aq), or aqueous Ammonium Hydroxide, but since all you did to get there was add ammonia to water, it is usually just considered an aqueous solution of ammonia. Answered by Shayla Grifin 6 months ago.

It can be ionic because NH4+ and Cl- NH4Cl But I think the bonds between the Nitrogen and Hydrogen are covalent. Answered by Krysta Barreneche 6 months ago.

the type of bond that exists in ammonium chloride is called the dative covalent bond Answered by Una Cogen 6 months ago.

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Ammonium chloride --> ammonia +hydrogen chloride?
how would the amount of energy involved in this reaction compare with if this reaction was reversed? please explain x Asked by Eldridge Gergely 6 months ago.

ammonium chloride --> ammonia +hydrogen chloride if the reaction were reversed, it would be ammonia +hydrogen chloride --> ammonium chloride Now in order for this reaction to occur, the ammonia would have to form a bond with the hydrogen chloride. Bond forming requires energy and is therefore an endothermic process. The quanity of energy is the same as the reaction from ammonium chloride to ammonia and hydrogen chloride, but unlike that reaction which is spontaneous and happens on its own, the reaction of ammonia +hydrogen chloride --> ammonium chloride is nonspontaneous and requires an input of energy to make it happen. Answered by Jerilyn Harbaugh 6 months ago.

How would you find how many moles are in:?
6.28g ammonium chloride Asked by Song Gather 6 months ago.

1. Each mole of ammonium chloride molecules has 1 mole of nitrogen atoms, 4 moles of hydrogen atoms, and one mole of chlorine atoms. The mass in grams of one mole of any one type of atoms equals the atomic weight shown for that element in the periodic table. Look up the atomic masss of each of these elements. Then do the math to calculate the total for ammonium chloride. 2. Divide 6.28g by the mass per mole. Answered by Marianela Blaker 6 months ago.


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