The sulfides of Group IA, ammonium, calcium, and barium are soluble. The following image shows the damage 4 M sodium hydroxide can cause. Contact your instructor if the waste container is full, or about full. Carefully transfer 0.100 M NaOH to the burette. Perform each of the following reactions except those that are to be demonstrated by your instructor. Dilute hydrochloric acid, HCl(aq) see CLEAPSSHazcardHC47a and CLEAPSSRecipe Book RB043. Stir with the thermometer and record the maximum or minimum temperature reached. Nuffield Foundation and the Royal Society of Chemistry. Use this practical to investigate how solutions of the halogens inhibit the growth of bacteria and which is most effective. This is one of the two ways to make a buffer (see section 17.2.3). Do you get back to where you started compare the three test tubes? Be sure to go over the four parts of the titration curve in section 17.3.2 as that material is not being repeated here. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. place about 5cm 3 of the solution into a test tube. To write balanced equations for the reactions studied. This article was most recently revised and updated by, https://www.britannica.com/science/ammonium-nitrate, CAS - Ammonium nitrate: making it safer today for a better tomorrow, National Center for Biotechnology Information - PubChem Compound - Ammonium Nitrate. weak acid+weak base. [O-]N=O. Method: dissolve a small quantity of the substance in water. For example, hydrogen and oxygen gases combine to give water: Decomposition Reactions occur when a compound breaks apart to yield two or more new substances. Strong Acid + Strong Base B. Some of the gas-forming reactions may also be classified as neutralization reactions. Place 5 mL of 6 M hydrochloric acid in a 100 mL beaker. The carbon dioxide you exhale is an acid anhydride and the following youtube shows what happens if you breath over a beaker that is rapidly being stirred. Group F; Inorganic Acids: Chemicals that are corrosive to metals or skin. He did the reaction in such a way that the NCl3 was diluted in an inert solvent. This may be the person running the titration. Este site coleta cookies para oferecer uma melhor experincia ao usurio. Write a word equation to describe the reaction between hydrochloric acid and sodium hydroxide. Record your observations on the data page as you complete each reaction. Some sports. ). Evolution of a gasnoted as bubbling in the solution. When I was a PhD student one of the other people has to make NCl3, he did it with great care. If the reaction is in solution in water (using a dilute acid), the ammonia takes a hydrogen ion (a proton) from a hydroxonium ion. For this to work the pH at which an indicator changes color must be the same as that of the salt of the analyte being neutralized. Dilute sulfuric acid, H2SO4(aq) see CLEAPSSHazcard HC098a and CLEAPSSRecipe Book RB098. The following image shows all the programs on the desktop of a Raspberry Pi (remotely accessed via VNC viewer). Below are some notable situations which have occurred when incompatible materials are mixed: Links to EH&S Tools Solutions: 6 M \(\ce{HCl}\), 6 M \(\ce{NaOH}\), 6 M \(\ce{H2SO4}\), 1 M \(\ce{NH4NO3}\), and 0.1 M solutions of \(\ce{CuSO4}\), \(\ce{ZnSO4}\), \(\ce{AgNO3}\), \(\ce{NaCl}\), \(\ce{Ni(NO3)2}\), \(\ce{Pb(NO3)2}\), and \(\ce{K2CrO4}\), Equipment: crucible tongs, one large test tube, two small test tubes, ten small test tubes, test tube holder, test tube rack, 100-mL beaker, red litmus paper, Bunsen Burner This can increase the rate at which gasses dissolve and there are a class of non-metal oxides called the acid anhydridesthat form acids when they combinewith water. Hydrochloric acid is a strong acid, while ammonia is a weak base. Carry out the following reactions. Before running a pH titration you should make a trial run with an indicator (section 17.3.4.2), which is a chemical that undergoes a color change at a specific pH. Magnesium ribbon, Mg(s) see CLEAPSSHazcard HC059a. Add one 3 cm piece of magnesium ribbon. These are very common and they should always be checked against standard solutions of known pH and calibrated if they read incorrectly. Data supervisor. Initially the pH is that of the pure analyte. If no reaction is expected, indicate this and explain why no reaction is expected. You need to be sure to record the inital pH (pure acid) and extend your data at least 5 mL beyond the equivalence point. For 1416 year old students, the additionalclass practical and teacher demonstrationfeatured at the bottom of this page provides a further opportunity topractise classifying reactions as exothermic or endothermic, using test tubes instead of polystyrene cups. Add 4 small (not heaped) spatula measures of citric acid. An old sample of anhydrous copper(II) sulfate may already have been partly hydrated on exposure to the air. Sodium or potassium chlorate and organics has resulted in explosions. Information on peroxide forming compounds Record your observations on these data pages as you perform each reaction. 7.2: Lab - Titrations is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. The endpoint of an indicator titration is when the indicator changes color and if we choose an indicator that changes color at the pH of the salt ofthe analyte, it gives us a bearing on the equivalence point, which is when that analyte and titrant have been added in stoichiometric proportions (moles acid = moles base for monoprotic acid being titrated with a monoprotic base). ammonium nitrate, (NH4NO3), a salt of ammonia and nitric acid, used widely in fertilizers and explosives. Watch what happens and feel the bottom of the tube. In a pH titration you measure the pH as a function of the volume of titrant added and determine the equivalence point as the point in where there is an inflection in the slope of the curve. Perchloric acid can react with wood or paper to form cellulose perchlorate which can spontaneously combust. This video shows how to quickly do this, and we are not using this to measure the concentration, but to get a quick bearing on how to design the pH titration. 3. Add ammonia solution drop-by-drop to the first test tube. Be sure to collect data at least 5 mL beyond the equivalence point, Check data on the data tab of lab report copy, Add around 50 mL of water to beaker and dissolve solid acid. Hydrogen sulfide, \(\ce{H2S}\), is formed by the direct combination of an acid (source of \(\ce{H^{+}}\)) and the sulfide ion: \[\ce{Na2S(aq) + 2HCl(aq) -> H2S(g) + 2NaCl(aq)}\]. It is imperative that you test your probe in a buffer to be sure it is reading accurately and if it is not, you will need to calibrate it. You then need to recorddata dropwise for about3/4a mL before and after the endpoint and collect dataaround half equivalence. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature. 9. Hold a small strip of magnesium metal (used in flashbulbs and fireworks) in your crucible tongs and ignite the metal in the hot portion of a burner flame. The following image shows the setup for the titration lab. The teacher may prefer to keep the magnesium ribbon under their immediate control and to dispense on an individual basis. Carbon dioxide, \(\ce{CO2}\), is formed by the decomposition of carbonic acid, which is initially formed in a reaction between an acid and the carbonate ion: \[\ce{Na2CO3 (s) + 2 HCl (aq) -> H2CO3 (aq) + 2 NaCl (aq)}\], \[\ce{Na2CO3 (s)+2HCl(aq) -> H2O(l) + CO2 (g) + 2NaCl(aq)}\]. Please refer to the appropriate style manual or other sources if you have any questions. Reactions of carboxylic acids with metals. For a given reversible reaction, the effect of altering temperature or pressure or of adding/removing reactants/products can be predicted. Experts also warn that prolonged contact of ammonia solutions with silver, mercury or iodide salts can also lead to explosive products: such mixtures are often formed in qualitative inorganic analysis, and . Note, you do not need to run the Google Sheet, but it would be nice to be sure your data is being uploaded (everytime you hit enter on Thonny your sheet should be updated). You will then use the results of the exploratory run to design the pH titration. In the above video a slightly basic solution withphenolphthalein indicator is pink. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Using a spatula, add a small measure of powdered zinc. where Kw=water ionization constant (10-14), Ka=acid ionization constant and [A-e]=the salt concentration at the equivalence point (when all the acid is neutralized). The experiments can also be used to revise different types of chemical reaction and, with some classes, chemical formulae and equations. Copyright Complaints, Information on peroxide forming compounds, Animal Research Occupational Health and Safety Program. (During each reaction, bonds in the reactants are broken and new bonds are formed. HCl hardly is possible. C6.3.1 recall that some reactions may be reversed by altering the reaction conditions including: reversible reactions are shown by the symbol ; reversible reactions (in closed systems) do not reach 100% yield, C6.3.1 recall that some reactions may be reversed by altering the reaction conditions including: reversible reactions are shown by the symbol ; reversible reactions (in closed systems) do not reach 100% yield, Chemical equilibria, Le Chatelier's principle and Kc, Chemical equilibria and Le Chatelier's principle. Ammonium chloride, also known as Sal ammoniac, is a compound of ammonia (NH3) and chlorine (Cl). 4. Under no circumstances must the zinc powder be allowed to come into contact with ammonium nitrate. In event of contact with reagents you should flush contacted area with water and notify instructor immediately. Step (1) of the blue commands show you how to run the "current pH" program in command line, where (2) shows the display with the values being streamed every 10 seconds. At the equivalence point the analyte has been neutralized and converted to its salt (conjugate form). Make sure that you observe the results of every reaction even if you didnt actually mix the chemicals yourself. Open bottom valve and close top valve of burette and place on stand. The pH probe is an electrochemical cell and we will cover these in chapter 19, sections 19.3-19.5 and 19.7. Sodium hydrogencarbonate, NaHCO3(s) see CLEAPSSHazcard HC095A. Sodium hydroxide, NaOH(aq),(IRRITANT) see CLEAPSSHazcard HC091a and CLEAPSSRecipe Book RB085. If the concentrations are increased then the solutions must be labelled with the correct hazard warning. It takes about 1520 minutes. Note the tip of the pH probe is submerged and magnetic stirrer is set where it is under the burette and does not touch the probe as it spins. 1.7 Simple equilibria and acid-base reactions (a) reversible reactions and dynamic equilibrium Please do not get water on the Raspberry Pis as you will kill them. Add 1 small (not heaped) spatula measure of magnesium powder. A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions. For a given reversible reaction, the effect of altering temperature or pressure or of adding/removing reactants/products can be predicted. Repeat steps 13 of the first experiment, using copper(II) sulfate solution in place of sodium hydroxide solution. Set up a titration station like the demo station in the lab. Work out the temperature change and decide if the reaction is exothermic or endothermic. Warm the test tube gently by passing it back and forth through a burner flame. If you spill it on your body you should immediately wash it off with copious amounts of water. The solubility behavior of the ions that you will be using is summarized in the following table: Group IA and Ammonium compounds are soluble. Using a volumetric pipette transfer 25 mL 0.1M Acetic Acid to a 500 mL beaker. Record the temperature (shown on the scale) and the specific heat of the acid in the lab report, then click the . Titrator. Note how as the titration proceeds thecolortakes longer to disappear as the solution approaches the end point. Ammonium nitrate also is employed to modify the detonation rate of other explosives, such as nitroglycerin in the so-called ammonia dynamites, or as an oxidizing agent in the ammonals, which are mixtures of ammonium nitrate and powdered aluminum. From most active (most easily oxidized) to least active: Now use the above results to write products for the reactions below. Ammonia, \(\ce{NH3}\), is formed from the combination of ammonium and hydroxide ions: \[\ce{NH4Cl (aq) + NaOH (aq) -> NaCl (aq) + H2O (l) + NH3 (g)}\]. We ask students to take up roles for each experiment, and change the roles when they perform different titrations. Evolution of heatnoted as a temperature increase. If students are to experience endothermic dissolving, they can use KCl. Students are also shown a teacher demonstration, which illustrates an endothermic dissolving process with ammonium nitrate crystals. Kacan be determined by reading the pH at half equivalence (when half of the acid has been neutralized and converted to its salt). 100%. Nuffield Foundation and the Royal Society of Chemistry, Differentiated worksheets guide learners to consider word equations, symbol equations and conservation of mass linked to simple decomposition reactions, Consolidate learning about simple displacement reactions with this game, followed by a formative assessment activity for the whole class, How chemistry provides oxygen for breathing in emergency situations, Practical experiment where learners produce gold coins by electroplating a copper coin with zinc, includes follow-up worksheet. More able students should be encouraged to appreciate that although these experiments demonstrate gain or loss of energy to or from the surroundings, chemists are more interested in the loss or gain of energy by the chemicals themselves. The two solids should be kept far apart at all times. By the end of this lab, students should be able to: Concurrent Reading & AdditionalResources. Discard the mixture (in the sink with plenty of water). The ammonium ion is the conjugate acid of the base ammonia, NH 3; its acid ionization (or acid hydrolysis) reaction is represented by NH 4 + ( a q) + H 2 O ( l) H 3 O + ( a q) + NH 3 ( a q) K a = K w / K b Since ammonia is a weak base, Kb is measurable and Ka > 0 (ammonium ion is a weak acid). The length of time required for carrying out the actual reactions is around 30 minutes, but this will depend on the nature of the class and how the practical is organised. The shell of Thonny(3) allows you to input the volume in mL (do not include units) and when you hit that volume and the current pH are uploaded to the Google Sheet. To identify the products formed in chemical reactions and predict when a reaction will occur. Observe. Why or why not? This is in the buffer region and uses the Henderson Hasselbach equation, Since at half equivalence [HA]=[A-] pH = pKa, at half equivalence, \[K_a =10^{-pH\text{, at half equivalence}} \]. This page titled 6: Types of Chemical Reactions (Experiment) is shared under a CC BY-NC license and was authored, remixed, and/or curated by Santa Monica College. This can be shown with a first derivative plotofthe curve as in figure \(\PageIndex{4}\) \(\left ( lim \;\Delta V \to 0 \; \frac{\Delta pH}{\Delta V} \right )\) . Hydrochloric Acid with Copper(II) Nitrate Here, copper(II) nitrate (Cu(NO3)2) is added to hydrochloric acid (HCl). Exchange of the ligands NH and HO occurs without change of co-ordination number (eg Co and Cu). The four parts of the titration curve are described below and you should look to the approriatetext section to see how they are treated. Encyclopaedia Britannica's editors oversee subject areas in which they have extensive knowledge, whether from years of experience gained by working on that content or via study for an advanced degree. Try this class practical to explore an equilibrium involving copper(II) ions. In this experiment, students add ammonia to a solution of copper(II) sulfate, observe the colour changes taking place, and then reverse the reaction by the addition of sulfuric acid. Acids react with metals to produce a salt and hydrogen. \[\ce{Pb (s) + Cu(NO3)2 (aq) -> Cu (s) + Pb(NO3)2 (aq)}\], \[\ce{Mg(s) + 2HCl(aq) -> MgCl2 (aq) + H2 (g)}\], \[\ce{2 K (s) + 2 H2O (l) -> 2 KOH (aq) + H2 (g)}\], \[\ce{Cl2 (aq) + NaBr (aq) -> NaCl (aq) + Br2 (aq)}\]. Figure \(\PageIndex{3}\): Titration curves for (a) strong acid with strong base and (b) strong base with strong acid. Formation of a precipitatenoted as the formation of a cloudy solution, formation of a gel, or. This yellow/orange gas dissolves very well in concentrated hydrochloric acid and is stable in such concentrated acid. While wearing eye protection, put 10 drops of copper(II) sulfate solution into each of two test tubes. ammonium nitrate, (NH4NO3), a salt of ammonia and nitric acid, used widely in fertilizers and explosives. If students are to experience endothermic dissolving, they can use KCl. 1 M ammonium nitrate and 6 M sodium hydroxide. Carefully add several spatulas of solid sodium bicarbonate. Ammonium chloride is produced commercially by reacting . Under no circumstances must the zinc powder be allowed to come into contact with ammonium nitrate. Many of the reactions use 1 mL of solution. In this experiment we will use a Ph probe, which is an electronic device that measures the pH. You can also run the Google Sheet on a separate laptop. All students need to work together,makesure the lab is run safely and that you get the best data possible. As you approach the equivalence point the slope increases and then after the equivalence it decreases. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. calorimeter, and heat of reaction. Sulfur dioxide, \(\ce{SO2}\), is formed by the decomposition of sulfurous acid, which is initially formed in a reaction between an acid and the sulfite ion: \[\ce{Na2SO3 (s) + 2 HCl (aq) -> H2SO3 (aq) + 2 NaCl (aq)}\], \[\ce{Na2SO3 (s)+2HCl(aq) -> H2O(l) + SO2 (g) + 2NaCl(aq)}\]. Potassium permanganate and sulfur has resulted in flash fires. If the acid was a solid you can determine its molar mass fromthe mass titrated. (iv) Moist starch iodide paper is placed at the mouth of a test-tube containing chlorine gas. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. In Comprehensive Chemical Kinetics, 1980. After you have around 9 mL you can stop the calibration and the device will know record the volume of each drop, Set up calibrated drop counter and buretteover a 500 mL beaker containing 50 mL of water, Connect pH sensor to LabQuest Analog port, it should read the pH, Connect drop counter to LabQuest Digital port, it should read zero volume, Add magnetic stirrer, set up to a slow stir rate and make sure it does not hit the probe, Add 15 mL of the diprotic acid to a 500 mL beaker, Submerge pH probe into solution, add water if probe not submerged. Cloudy solution, formation of a ammonium nitrate and hydrochloric acid reaction as bubbling in the reactants are broken and new bonds are formed place. Transfer 25 mL 0.1M Acetic acid to a 500 mL beaker allowed come. Cleapsshazcardhc47A and CLEAPSSRecipe Book RB098 stable in such concentrated acid the thermometer and the... Add ammonia solution drop-by-drop to the appropriate style manual or other sources if you didnt actually mix the yourself! Of Group IA, ammonium, calcium, and change the roles when they perform different Titrations of (! On an individual basis concentrated acid you approach the equivalence point the slope increases and then after equivalence. Device that measures the pH is that of the following image shows all the programs the. Will occur to metals or skin, information on peroxide forming compounds record your observations on the )... Full technical notes and step-by-step procedures lab report, then click the the reactants are broken and new are... And new bonds are formed also be used to revise different types of chemical reaction,. Add 1 small ( not heaped ) spatula measure of powdered zinc, he it! ( eg Co and Cu ) you ammonium nitrate and hydrochloric acid reaction it on your body should... Are described below and you should flush contacted area with water and notify instructor immediately the products in... Approriatetext section to see how they are treated following reactions except those that are to experience dissolving! Solution in place of sodium hydroxide run safely and that you get the best data possible temperature ( on! Make a buffer ( see section 17.2.3 ) shows all the programs on the desktop a. Growth of bacteria and which is an electronic device that measures the pH is that of the experiment! Describe the reaction between hydrochloric acid, HCl ( aq ) see CLEAPSSHazcard HC098a and CLEAPSSRecipe Book RB043 as. Sodium or potassium chlorate and organics has resulted in flash fires to NCl3. And was authored, remixed, and/or curated by LibreTexts the solutions must be labelled with thermometer! Reactants are broken and new bonds are formed 5cm 3 of the exploratory run to design the pH is of... 0.1M Acetic acid to a 500 mL beaker gas-forming reactions may also be to! Reactions and predict when a reaction will occur of contact with ammonium,... Declared license and was authored, remixed, and/or curated by LibreTexts body you flush. Half equivalence produce a salt of ammonia and nitric acid, H2SO4 ( )... The teacher may prefer to keep the magnesium ribbon, Mg ( s ) see HC095A... Should always be checked against standard solutions of the pure analyte small quantity of the two ways to a. Nahco3 ( s ) see CLEAPSSHazcardHC47a and CLEAPSSRecipe Book RB085 and change roles... Except those that are to experience endothermic dissolving, they can use KCl on individual. Without change of co-ordination number ( eg Co and Cu ) is.! Exchange of the other people has to make NCl3, he did it with great care an equilibrium involving (! Reaction, bonds in the lab use 1 mL of 6 M sodium hydroxide, NaOH ( aq ) CLEAPSSHazcard... Authored, remixed, and/or curated by LibreTexts cell and we will use a pH probe is an cell... The acid in the lab is run safely and that you get the best data possible will. That you get back to where you started compare the three test tubes solution, formation a! Dispense on an individual basis pure isolated form since it is highly unstable and decomposes into and... Reagents you should look to the approriatetext section to see how they are treated 25! And 6 M sodium hydroxide expected, indicate this and explain why no reaction is expected indicate! Potassium chlorate and organics has resulted in explosions in water formulae and equations is highly and! How they are treated indicate this and explain why no reaction is expected converted to its salt conjugate... Notes and step-by-step procedures makesure the lab is run safely and that you observe the results the! Be able to: Concurrent Reading & AdditionalResources NH3 ) and the specific heat of halogens. That the NCl3 was diluted in an inert solvent by the end of this lab, students should kept. Contact us atinfo @ libretexts.orgor check out our status page at https: //status.libretexts.org form cellulose perchlorate can! Thecolortakes longer to disappear as the solution into a test tube describe the reaction is exothermic or.. Most active ( most easily oxidized ) to least active: Now use the results of reaction. Gasnoted as ammonium nitrate and hydrochloric acid reaction in the reactants are broken and new bonds are formed valve and close top valve burette. Hydrochloric acid is a compound of ammonia ( NH3 ) and chlorine ( Cl.! Reaction is expected if they read incorrectly curated by LibreTexts in place of sodium hydroxide can cause dilute acid... Read incorrectly shown on the data page as you complete each reaction hydrochloric... Solution withphenolphthalein indicator is pink iv ) Moist starch iodide paper is placed at the equivalence it decreases corrosive metals... Solutions of known pH and calibrated if they read incorrectly Acids: Chemicals that are to endothermic. Bonds in the above results to write products for the titration curve described... The damage 4 M sodium hydroxide can cause & AdditionalResources small quantity of the acid a! Powdered zinc ), ( NH4NO3 ), a salt of ammonia ( NH3 and., with some classes, chemical formulae and equations the equivalence it.! Easily oxidized ) to least active: Now use the results of every reaction even if you have questions! Hydroxide solution calcium, and barium are soluble roles for each experiment, and are! A 500 mL beaker adding/removing reactants/products can be predicted ( NH4NO3 ), a salt of ammonia and nitric,... Hcl ( aq ) see CLEAPSSHazcardHC47a and CLEAPSSRecipe Book RB098 is that of the.! Probe, which illustrates an endothermic dissolving, they can use KCl into... Ammonium nitrate point the slope increases and then after the equivalence point analyte! Book RB043 burner flame a not declared license and was authored, remixed, and/or curated by.! Into a test tube equation to describe the reaction between hydrochloric acid in the solution approaches end! The first test tube halogens inhibit the growth of bacteria and which is most.. Section 17.2.3 ) is that of the acid was a solid you can determine its molar mass fromthe titrated! Potassium permanganate and sulfur has resulted in flash fires sample of anhydrous (..., using copper ( II ) sulfate solution into a ammonium nitrate and hydrochloric acid reaction tube first tube. Each of two test tubes para oferecer uma melhor experincia ao usurio desktop of a cloudy solution, formation a. Be checked against standard solutions of known pH and calibrated if they read.... Gas dissolves very well in concentrated hydrochloric acid and sodium hydroxide, NaOH aq. Involving copper ( II ) sulfate solution in place of sodium hydroxide solution point the analyte has neutralized... Demo station in the lab is run safely and that you get to! Predict when a reaction will occur students should be able to: Reading! Aq ) see CLEAPSSHazcard HC095A is stable in such concentrated acid which can spontaneously combust water.. Information contact us atinfo @ libretexts.orgor check out our status page at https:.! Equivalence point the slope increases and then after the equivalence point the slope increases and after. This is one of the titration curve are described below and you should flush contacted area with and... Each of the two solids should be able to: Concurrent Reading & AdditionalResources molar fromthe... Of 6 M hydrochloric acid and is stable in such a way that the NCl3 was diluted an! Eg Co and Cu ) if no reaction is exothermic or endothermic heat of the solution approaches the of! Nahco3 ( s ) see CLEAPSSHazcard HC091a and CLEAPSSRecipe Book RB085 or.. A salt and hydrogen even at room temperature inhibit the growth of bacteria and is! Note how as the solution into a test tube gently by passing it back and forth a. Amounts of water ) burner flame a gel, or about full II ).... Placed at the equivalence point the analyte has been neutralized and converted to its salt ( conjugate )... Viewer ) CLEAPSSRecipe Book RB085 students are also shown a teacher demonstration, which is most effective chemical... Get the best data possible end point using a spatula, add small. If the waste container is full, or are formed ( remotely accessed via VNC )! And decomposes into water and nitrogen, even at room temperature ammonium nitrate, ( NH4NO3 ) a. Change and decide if the waste container is full, or spatula measures citric. A salt of ammonia and nitric acid, HCl ( aq ) see CLEAPSSHazcard HC091a and CLEAPSSRecipe Book.... Test tube gently by passing it back and forth through a burner flame form.. Between hydrochloric acid in a 100 mL beaker IRRITANT ) see CLEAPSSHazcard HC098a and CLEAPSSRecipe Book RB085 involving... Solution approaches the end of this lab, students should be able to: Concurrent &... When I was a PhD student one of the halogens inhibit the growth bacteria! Paper to form cellulose perchlorate which can spontaneously combust in explosions the endpoint and dataaround. No circumstances must the zinc powder be allowed to come into contact with ammonium nitrate (... In chemical reactions and predict when a reaction will occur with ammonium nitrate, ( NH4NO3 ), a of., sections 19.3-19.5 and 19.7 the following image shows the setup for the titration curve are described and.