We must indicate these phases in the balanced chemical equation (equation 9).MgCl2(aq) + Pb(NO3)2(aq) à Mg(NO3)2(aq) + PbCl2(s) (9)When the two solutions in the above example are mixed, it is instantly apparent that a chemicalreaction has occurred; a cloudy white precipitate forms. This preview shows page 1 - 3 out of 10 pages. The reactioncan be balanced after the correct chemical formulas for the products have been written.The reaction between HCl and NaOH (equation 5) is an acid-base reaction. Strong electrolytes dissociatecompletely. Obtain one set of unknown solutions and record the letter in your lab notebook. Non-electrolytes are compounds that do notdissociate in water. Obtain one set of unknown solutions and record the letter in your lab notebook. Therefore Mg2+ and NO3– will be present in the form of aqueousions. In equation 3, zinc is much more reactive than copper; therefore, it replacesthe copper(II) ion in cupric chloride.CuCl2(aq) + Zn(s) à Cu(s) + ZnCl2(aq) (3)Double Displacement: A double displacement reaction involves the exchange of the anions andcations of two compounds. Solubility of NaCl as mass of NaCl per 100 mL of solvent. In a previous experiment, you carried out thedecomposition of copper(II) sulfate pentahydrate through a process called dehydration. It is useful to classify reactions in this waybecause it can assist you in the prediction of products. The reaction of an acid with a base is simply a specialcase of a double displacement reaction, but is more commonly referred to as a neutralizationreaction.HCl(aq) + NaOH(aq) à NaCl(aq) + H2O(l) (5)Combustion: A combustion reaction is where a hydrocarbon (e.g., methane or octane) orhydrocarbon derivative (e.g., glucose) is burned in the presence of oxygen. Examples of strong electrolytes aresoluble salts (NaBr and AlCl3), strong bases (NaOH and KOH), and strong acids (HCl, H2SO4,and HNO3). We have a team of professional academic writers who can handle all your assignments. In essence, predict the outcome of the reactions from the solubility rules.6SAFETY/HYGIENE/WASTE DISPOSAL, 123456Name: _____________ Lab Day: M T W R F Instructor: ______Room: 103 109 117 125 Lab Time: ___10POST-LAB QUESTIONS. Preview text. Solubility refers to the ability of a given amount of a soluteto dissolve in a solvent. As in the previousexample, the cations on the reactants side (H+ and Na+) exchange with the anions (Cl– and OH–,respectively) to give the products NaCl and HOH (H2O). Prepare a similar data sheet in your lab notebook. CriticalHomework offers writing services for our clients research purposes and helping them to gain better understanding of the subject. A classicexample is photosynthesis, the conversion of carbon dioxide and water into sugar by plants(equation 16).6 CO2 + 6 H2O + energy à C6H12O6 (16)Temperature changes are generally harder to detect when small amounts of reactants are used,since the energy produced or consumed is an extensive property. But you are required to know how to, Each pair of students will need to obtain a transparency cover from their instructor. For example, you may see a white precipitate form whenthe two solutions are mixed, or you may detect a temperature change. Examples of weakelectrolytes are slightly soluble or insoluble salts and bases (BaSO4, PbI2, and Zn(OH)2) andweak acids (H2CO3, CH3COOH, and HCN). © 2020 Critical Homework. (10)This is a double displacement reaction, so after we have exchanged the ions and balanced theircharges, the predicted products are NaCl and H2CO3. Again, you will have to memorize this phenomenon. The following net ionic equation remains:2 Ag+(aq) + 2 Cl–(aq) à 2 AgCl(s) (spectator ions; Mg2+(aq) and NO3–(aq))The observation that the student made when these two solutions were mixed was the formationof the silver chloride precipitate. In this experiment you willneed to make detailed observations as you mix the known solutions to help you determine if areaction has occurred.3OBSERVATIONSYou can tell that a reaction has occurred if you observe a “change” when the chemicals aremixed. The following experiments were carried out in order to detect which two solutions would create a distinguishable change when mixed.