...name-----Mr. Kalanderopoulos, J Course code-----SCH4U Abstract The purpose of this lab is to find out the molar enthalpy change of neutralization by mixture sodium hydroxide and hydrochloric acid. To get the result use some related materials and thermometer to measure the temperature of each solution. The formula to describe this mixture reaction is HCl + NaOH → NaCl + H2O (Sodium hydroxide combined with Hydrochloric acid) Purpose To determine the molar enthalpy change of neutralization, for the reaction of aqueous sodium hydroxide and aqueous hydrochloric acid. Hypothesis If Hess’ law is used to calculate the molar enthalpy of combined for HCl and NaOH using experimentally determined enthalpy values, then the final result will be more specific. This is because Hess’ law states that the sum of the enthalpy pages of the intermediate reactions, should equal the enthalpy change of the target reaction. Materials Coffee-cup calorimeter | Strning rod | Two 100 ml graduate cylinders | 1.0 mol/L Sodium hydroxide NaOH (aq) | thermometer | 1.0 mol/L Hydrochloric Acid HCl (aq) | Procedure Safety---before doing the lab, make sure already read the lab safety guidelines. (MSDS of sodium hydroxide and hydrochloric acid). All things that were unrelated and corrosive to the experiment should be clear off the benches. Goggles and glove should be kept on all the time. To start this lab need assemble two coffee-cup calorimeter, each assemble coffee-cup have a nested polystyrene...
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...Antacid Lab Report Abstract: Inflation is gradually increasing the prices on every human necessity. Unfortunately, the medicine people need to combat distress, disease and sickness are no exception. The purpose of this lab was to make a comparison between two antacid tablets through a titration. The comparison was made between effectiveness and cost, and to make a final verdict on which tablet can neutralise more acid for equal amounts of money. The ground tablets were placed in an Erlenmeyer flask along with a base, a pH indicator, and water. Hydrochloric acid with a pH of two was slowly released into the mixture using a burette. The observable difference that indicated the desired change in pH was a colour variance of the liquid, created by the indicator. The quantity of hydrochloric acid needed to bring the basicity of the mixture to the right pH was noted, and the procedure was repeated with the other antacid. The results showed that the Tums brand could neutralise more acid, however the Equate brand has a lesser cost per gram. A calculation revealed that the Equate brand was the better choice, since overall it could eliminate more hydrochloric acid than the Tums brand per dollar. Key Terms: Chemical reaction: A reaction in which the ionic or molecular structure of a substance is changed to fulfill the substance’s need of a full valence shell of electrons. pH: Scale used to express how acidic or basic a solution is. The scale ranges from 0-14, with 7 being neutral...
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...Practical 12 : Rate Of Reaction Name : AFNAN BIN ABDUL RAHMAN Class : M11J Research Question : How does the reaction between Zinc metal and 0.1M of Hydrochloric Acid using different sizes of Zinc metal (Powdered Zinc, Shredded Zinc strip and Zinc strips) can affect the volume of Hydrogen gas produced at the end of the experiment (after 10 minutes) under same temperature which is room temperature? Variables : Manipulated : Different sizes of Zinc Metal Responding : Volume of Hydrogen Gas produced after 10 minutes. Constant : Constant | Method to control | Possible Effect(s) | Concentration of Hydrochloric Acid | The concentration of Hydrochloric Acid was kept constant to be used in both experiments which is 0.1 Mole. | The difference in concentration might alter the results as the rate of reaction will also differ since the effective collision will occur more when the concentration increases. | Time taken for the reaction to occur | The period of reaction for each reaction was kept constant which is 10 minutes for each experiments. | Longer period of time will increase the possibilities of effective collision between the molecules and alter the final result. | Temperature of surrounding | Both experiments were conducted in a lab with room temperature. | The difference in temperature might cause the difference in kinetic energy of the molecules and will disturb the result of the rate of reaction between Zinc and Hydrochloric Acid. | Material and Apparatus...
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... Myrjun, Lindsay, Lara Displacement Reactions Lab Report Purpose: To observe and compare single and double displacement reactions. Hypothesis: If a metal element is mixed with an ionic compound, one metal will displace the other to create a new ionic compound. If 2 ionic compounds are mixed together, then the metals will displace each other, creating 2 new ionic compounds. Materials: Goggles, large well plate, steel wool, scoopula, 4 small beakers, dropper, 4 pieces of magnesium ribbon, 4 pieces of zinc metal, 4 pieces of copper wire, copper (II) sulfate solution, zinc nitrate solution, magnesium nitrate solution, sodium carbonate solution and hydrochloric acid. Procedure: Part A: Single Displacement Reactions 1. Clean 4 pieces of magnesium ribbon, zinc metal and copper wire with steel wool until they are shiny. 2. Half-fill one column (three wells) of the well plate with the copper (II) sulfate solution. 3. Half-fill a second column (three wells) with the zinc nitrate solution. 4. Half-fill a third column (three wells) with the hydrochloric acid. 5. In each column, place 1 piece of each metal in different wells (Magnesium in one well, zinc in another and copper in the last). Use a toothpick to keep the metals submerged in the solution. 6. Observe the different reactions in each well. Record your observations in a table. 7. Save the contents of the wells for Part B. Part B: Double Displacement Reactions 1. Add 3 drops of the sodium carbonate...
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...Determination of the Reaction Rate of Mg and HCl Alex Skartvedt Alex Skartvedt, Melanie Ho, Christina Olson, Thor Swerdykiak November 11, 2015 Fall 2015 Semester Abstract: The experimental rate law of the reaction: 2HCl(aq)+Mg(s)→MgCl2(aq)+H2(g) is being determined because kinetics play a large role in the reactions happening in everyday life. The rate law, k value will be obtained in the experiment. To obtain the information a pressure probe was connected to an Erlenmeyer flask in order to record the rate of the reaction of magnesium ribbon and hydrochloric acid. The order of HCl and Mg were then determined using the information found in from the reaction. The order in HCl and Mg were found to be less than the expected...
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...Name: Marquetta Turner iLab, Week #3 ATOMIC WEIGHT OF MAGNESIUM LAB Introduction: The purpose of this lab experiment is to determine the atomic weight of magnesium by measuring the amount of hydrogen gas evolved when hydrochloric acid reacts with magnesium. The reaction is as followed: Mg + 2HCL H2 + Mg2+(aq) + 2Cl-(aq) This can be demonstrated by measuring the hydrogen gas evolved by performing a chemical experiment when hydrochloric acid reacts with the magnesium. The formulated reaction includes; Mg + 2HCl → H2 + Mg2+(aq) + 2Cl- (aq) The major findings contributing to the experiment is being able to determine and distinguish what moles have evolved thus being the hydrogen moles evolved allowing the magnesium to be consumed within the reaction. Procedure: 1st. Obtain a 600ml beaker, add 300ml of water 2nd. add 30ml of HCl (2M) to the beaker and stir 3rd. add 10mg of Magnesium metal to the beaker 4th. Allow hydrogen gas to evolve, all of the magnesium should be consumed. 6th. Record the amount of hydrogen gas evolved using the chemical property dialog. <Include information that the reader would need to repeat your experimental procedure. Do not include any observations or results in this section.> Observations and Results Moles of hydrogen evolved: 0.000829g (8.29 x 10-4)/ 0.000411 moles, (4.11 x 10-4) Moles of H2 evolved = moles of Mg consumed Atomic weight of Mg= /0.000411moles During my observation I noticed that when 10mg of magnesium...
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...Student Name: Andreas Sippl Student ID: 4445491 Date: 04 January 4, 2015 Course and Section Number: SCIN131 Lesson 6 Lab: Titrations and Natural Acid/Base Indicators Begin by viewing the following Thinkwell videos 15.1.7 CIA Demonstration: Titrations 11.2.2 CIA Demonstration: Natural Acid-Base Indicators (NOTE: The second video is sort of a supplement to the first, and shows how this applies to your daily life. Feel free to try some of the things listed in the video, but be sure to report back to the class regarding the results of your experiments!) After you watch the above video, answer the questions below in sufficient detail: (a) (1 pts.) In YOUR OWN WORDS, what is a titration? What type of reaction is it? Be detailed and specific...
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...[pic] ANTACIDS PRE LAB DISCUSSION The stomach produces hydrochloric acid to begin the chemical breakdown [digestion] of the food that you eat. Although this acid is quite strong, (about 2 M), the stomach has a thick mucus lining that protects the stomach tissue itself from being digested by the acid. When the stomach is too full or when you have swallowed air, the acid will be forced up out of the stomach into the unprotected esophagus. The acid will react with the unprotected tissue and cause a burning sensation commonly known as "heart burn". There are a number of over-the-counter medications called "antacids". These are not chemical bases. If they were bases and you used them regularly or took them in large doses, they would raise the pH of your blood. This condition, called alkalosis, would result in kidney damage. The brands of antacids sold in the drug store contain insoluble compounds that acids will react with, resulting in the acid being consumed in the reaction. The most common ingredient used is calcium carbonate [CaCO3], also known as limestone. This limestone is ground to a powder, mixed with a starch paste, and formed into a tablet. Often flavoring and coloring is added to make the tablet more attractive. Other tablets contain insoluble hydroxides that will react with hydrochloric acid. There are also newer types of antacids that are taken before eating. These consist of a hormone [chemical messenger] that reduces the...
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...Acids are substances that form hydrogen ions (H+(aq)) when dissolved in water eg hydrochloric acid HCl gives H+(aq) and Cl-(aq) ions, sulphuric acid H2SO4 gives 2H+(aq) and SO42- ions and nitric acid HNO3 gives H+(aq) and NO3-(aq) ions. o Alkalis are substances that form hydroxide ions (OH-(aq)) in water eg sodium hydroxide NaOH gives Na+(aq) and OH-(aq) ions, calcium hydroxide Ca(OH)2 gives Ca2+(aq) and 2OH-(aq) ions. Note: an alkali is a base soluble in water. o In water, there are trace quantities of H+ and OH- ions BUT they are of equal concentration and so water is neutral. o In acid solutions there are more H+ ions than OH- ions. o In alkaline solution there are more OH- ions than H+ ions. o Acids dissociate to different extents in aqueous solution. Acids that dissociate to a large extent are strong electrolytes and strong acids. In contrast, acids that dissociate only to a small extent are weak acids and weak electrolytes In a similar manner, bases can be strong or weak depending on the extent to which they dissociate and produce OH– ions in solution. Most metal hydroxides are strong electrolytes and strong bases. Ammonia, NH3, is a weak electrolyte and weak base. o BASES eg oxides and hydroxides are substances that react and neutralise acids to form salts and water. Bases which are soluble in water are called alkalis. Acids Some common acids are listed below: Name Hydrochloric acid Sulphuric acid Nitric acid Ethanoic (acetic) acid Methanoic (formic) acid Citric...
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...ammonia gas and hydrochloric acid gas by using Hess’s law. Introduction: A reaction that release heat to surrounding is known as exothermic reaction. It is usually observed as temperature increases in solvent, container and other immediate surroundings. The expression of heat released from the reaction is: qreaction = qsolution + qcalorimeter ……..(1) The qcalorimeter is nearly zero because the calorimeter in this experiment is assumed to absorb little heat. So, the equation is simplified to qreaction = qsolution ……...(2) The change in temperature that caused by the addition of a given amount of heat will depend on specific heat, Csp of substance. Therefore, the heat involved is calculated by the equation Q = (Csp)(m)(T) ………(3) Mass of substance is m, change is temperature is T (final temperature – initial temperature). The heat changes observed is equal to enthalpies of reaction, H for the reactions considered because this experiment was run at constant pressure. The enthalpy of these directly observed reactions and Hess’s law was used to calculate the enthalpy change for an additional reaction which is not directly observed. Hess’s law stated that the overall enthalpy change of a chemical reaction is independent of its pathway. The magnitude of enthalpy change of a chemical reaction depends only on the difference in the enthalpy content of the products and the reactants, and does not depend on how the reaction is completed...
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...Chem 102- 810 Lab partner: Amanda K Experiment 11: Copper Cycle Lab Report Objective: To observe a sequence of reactions involving copper that form a cycle; to develop better laboratory techniques; to gain skills in observing and interpreting observations; and to practice quantitative laboratory techniques. Reactions: 1. Cu(s) + 4HNO3 (aq) ---------- Cu(NO3)2(aq) + 2H2O(g) + 2NO2(l) 2. Cu(NO3)2 (aq) + 2NaOH(aq) --------- Cu(OH)2(s) + 2NaNO3 (aq) 3. Cu(OH)2 (s) + HEAT ------------ CuO(s) + H2O(l) 4.CuO(s) + H2SO4(aq) ---------- CuSO4 (aq)+ H2O(l) 5.Zn(s) + CuSO4 (aq) ------------- ZnSO4(aq) + Cu(s) Potential Hazards: Concentrated nitric acid causes severe burns and the vapor is a lung irritant. The hydrogen gas that is produced is flammable. Concentrated hydrochloric acid causes severe burns. Methanol is flammable. Keep away from all ignition sources. Acetone is flammable. Keep away from all ignition sources. Procedure: 1.Obtain about 0.5g copper. In the main fume hood, using a 250 mL beaker, prepare the Cu(NO3)2 by adding 4.0mL of concentrated nitric acid to the copper wire. ***Caution. 2.Add 30 mL of 3.0 M NaOH to precipitate Cu(OH)2. With stirring, heat just to boiling on a hot plate. This will change the insoluble Cu(OH)2 into insoluble, black CuO. 3.Let the CuO to settle, then decant the supernate liquid. Add about 200 mL of very hot distilled water, settle and decant a second time. Properly dispose of the supernate liquid...
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...SNC 2D Conservation of Mass Lab Activity Purpose: The purpose of this activity is to investigate whether mass is conserved during chemical reactions. Hypothesis: Write a hypothesis predicting whether or not the mass will be conserved during a chemical reaction. __________________________________________________________________ __________________________________________________________________ Materials: Safety Goggles 250mL Erlenmeyer flask plus rubber stopper One micro test tube Electronic scale Solutions: Reaction 1 Reaction 2 Sodium bicarbonate potassium thiocyanate solution Dilute hydrochloric acid iron (III) chloride solution Procedure: Reaction 1 1. Add some sodium bicarbonate powder to the Erlenmeyer flask. 2. HALF-fill the micro test tube with hydrochloric acid. 3. Carefully place the micro test tube into the Erlenmeyer flask. 4. Place the rubber stopper on the flask. 5. Observe each of the two reactants and record their appearance in the table below. 6. Use the electronic balance at the front of the class to determine the total mass of the materials and record it in the table below. 7. With your hand over the rubber stopper, turn the flask upside down. When the reaction is over, turn the flask back over and record the appearance of the products. 8. Use the electronic scale once more to determine the mass of the products and record...
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...Experiment 5, CH-201-051 Lab Date: 1/28/15 Due Date: 2/4/15 Dr. Paliwal Acid-Base Reactions Purpose: The purpose of this set of laboratory experiments is to study the correlation between acids and bases by measuring and comparing their pH level. This can then be used to further evaluate the neutralization of acids with a base, such as stomach acid with calcium carbonate, antacid tablets. Data: Part B-1: Test pH of Laboratory Chemical Solutions Name Chemical Formula Calculated pH of 0.010 M Solution Laboratory pH Test results (0.010 M) Sodium Chloride NaCl 7 7.07 Ammonia 〖NH〗_3 10.62 10.15 Sodium Acetate 〖NaCH〗_3 〖CO〗_2 8.88 7.24 Hydrochloric Acid HCl 2.0 1.71 Ammonium Chloride 〖NH〗_4 Cl 5.63 6.58 Acetic Acid 〖CH〗_3 〖CO〗_2 H 3.38 3.33 Sodium Hydroxide, Lye, or Caustic Soda NaOH 12.0 11.68 Ammonium Acetate 〖NH〗_4 〖CH〗_3 〖CO〗_2 7.0 7.69 Part B-2: Test pH of paired Acid and Base solutions: Compound Names Compound Formulas Measured pH of Equal volumes of Solutions Hydrochloric Acid + Sodium Hydroxide HCl+NaOH 4.58 Ammonia + Acetic Acid 〖NH〗_3+〖CH〗_3 〖CO〗_2 H 9.05 Part B-3: Test pH of common Household items Household Item Name: Test pH: Lemon Juice 2.07 Ammonia 11.53 Mouth Wash 4.04 Vinegar 2.02 Part C- Testing Effectiveness of Antacids Acid Solution Antacid Test #1 pH result Test #2 pH result Diluted 20 mL of HCl solution to simulate Stomach Acidity none 2.45 Control Value 2.45 Control Value Diluted...
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...Jonte Berry LAB 3 REPORT SHEET – ACIDS, BASES, INDICATORS, pH Procedure Number 3 Estimated pH with pH paper Vinegar (Ph 2) Soap + H2O (Ph 6) Tap water (Ph 8) Baking soda + H2O (Ph 9) Ammonia (Ph 13) 4 What color is your “red cabbage solution” when diluted with tap water? (The water turns ruby red) Do you think we will all have exactly the same color? Explain your answer. (No) 5 Solution color Estimated pH with cabbage indicator with cabbage indicator Vinegar (Light pink) (Ph 4) Soap + H2O (Clear Pink) (Ph 4) Tap water (Light blue) (Ph 10) Baking soda+H2O (Light light blue) (Ph 10) Ammonia (Clear) (Ph 10) 6 Describe what happened to the color of the solution when you mixed the vinegar and ammonia solutions. What do you estimate the pH of the solution to be with pH paper? (The pink color from the vinegar changes to light blue when the ammonia was added.) What do you estimate the pH of the solution to be with the cabbage indicator? (Ph 10) 7 What happened when you added the baking soda solution to the mixture of vinegar/ammonia? Describe your observations. (When I added the baking soda solution nothing happen at all.) What do you estimate the pH of the solution to...
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...Practical 3 Investigation of Action of Saliva and Hydrochloric Acid in Two Carbohydrate Solution | Objective: 1. To show the action of saliva in two carbohydrate solutions. 2. To show the action of hydrochloric acid in two carbohydrate solutions. Apparatus & Equipment’s: Boiling tubes Metal test tube racks Beaker Graduated plastic dropper Water bath,~37°C Water bath,~95°C Stop watch Test tube holder Materials: Carbohydrate solution A Carbohydrate solution B Benedict’s solution 3M Hydrochloric acid 3M Sodium hydroxide Procedures: 1. Prepared two boiling tubes with containing 1 ml solution A and 1 ml solution B respectively. 1 ml Benedict’s solution was added to each tube and heated both tubes together in the (~95°C) water bath for two minutes. Then, recorded the results in table 1. 2. Added a few drops of fresh solution A and B separately spaced on a white tile. On each solution, added 1-2 drops of iodine solution and mixed with pen cover. Recorded your observations in the table 1. 3. Pipetted 2 ml solution B into each of four boiling tubes. The tubes were labelled 1, 2, 3 and 4 respectively near mouth of tube. Labelled your group name. 4. Placed tubes 1 and 2 in a water bath of ~37°C. 5. Salivated into a small beaker until it reached about 5 ml. 6. At the same time, step (6) and (7) was to be done approximately. Measured out 4 ml of the saliva prepared in step (4) and pipetted 2 ml each into tubes 1 and 4. The contents of the tubes shook well to ensure...
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