Strong electrolytes are compounds that completely dissociatein water, forming many ions that can conduct electricity. Do you have responsibilities that may hinder you from turning in your assignment on time? Course Hero is not sponsored or endorsed by any college or university. A compound thatis a solid (s), liquid (l), or gas (g) does not dissociate. Weak electrolytes are compounds that only partially dissociate in water. Are you tired and can barely handle your assignment? Never weigh chemicals directly on a balance pan. There areonly a few ions in the solution, thus the solution conducts electricity poorly. Examine thereactants and products to determine their phases. If the compound is aqueous (aq) it is possiblethat it will dissociate into its ions. If 167 mL of 6.0 M HCl is diluted to a final volume of 500 mL, the concentration of the final solution will be 2.0 M. Part B: Solubility Rules Each of the solutions made in Part A involves dissolving an ionic solid in water. This type of reaction usually results inthe formation of a precipitate, a gas, or water.ZnCl2(aq) + 2 AgNO3(aq) à Zn(NO3)2(aq) + 2 AgCl(s) (4), A + B → ABAB → A + BAB + X → XB + AAB + XY ® AY + XB2In equation 4, zinc chloride reacts with silver nitrate and the resulting products are zinc nitrate andsilver chloride. The other indicators of reaction wehave discussed above (precipitation, gas formation, color change) are easier to detect; they willbe the predominant indicators used in this experiment.IONIC AND NET IONIC EQUATIONSOnce you have determined that a reaction has occurred, you will need to write a chemicalequation. Unit V: Solutions and Solubility LAB REPORT I. Our essay writers are graduates with diplomas, bachelor, masters, Ph.D., and doctorate degrees in various subjects. The silver nitrate, magnesium chloride, and magnesium nitrate are all strongelectrolytes and should be broken into ions; however, silver chloride is insoluble (it is in the solidstate), and should be left alone.2 Ag+(aq) + 2 NO3–(aq) + Mg2+(aq) + 2 Cl–(aq) à 2 AgCl(s) + Mg2+(aq) + 2 NO3–(aq)From this total ionic equation, we conclude the nitrate and magnesium ions are the spectatorions, present on the reactants side as well as the products side of the equation, and can becanceled. Consider the reaction ofhydrochloric acid, HCl, and sodium carbonate, Na2CO3. From your observations you should be able to write a balanced chemical reaction for each, Properly dispose of the solutions in your dropper pipets. The trimmed reaction is called the netionic equation (NIE), and represents the actual chemical change taking place. After 10 Use a damp paper towel to clean. The NaOH solution provided in the lab was initially made as an ionic compound dissolved in water. If we exchange the ions we get the followingproducts:NH4Cl(aq) + NaOH(aq) à NH4OH(aq) + NaCl(aq) (13)↓NH4OH(aq) à NH3(g) + H2O(l) (14)The predicted product from this double displacement reaction is ammonium hydroxide, which, likecarbonic acid, is not a stable compound. Solubility refers to the ability of a given amount of a soluteto dissolve in a solvent. However, in some cases it may bedifficult to observe changes.Some reactions can be detected because they generate a gas or an odor. It will precipitate from solution as indicated in the reaction. However, some observations may be difficult to detect, sowrite detailed observations and keep an open mind when mixing the reactants. These cations will react with thechloride anions to form silver chloride, AgCl(s); silver chloride is not soluble in water, as indicatedby the solubility rules. Preview text. Any compound that is a weakor non-electrolyte should be left alone.Consider the following example. Notice that there is not a one to one mole ratio for the product zinc nitrate andthe reactant silver nitrate. Any compound that is a strong electrolyte should be broken into its constituent ions; forexample, Ba(OH)2(aq) would be broken into Ba2+(aq) and 2 OH–(aq). Hypothesis: If the temperature of the liquid is increased, then more sugar wil dissolve because warm solutions hold more solute than cold solutions. Solubility of NaCl as mass of NaCl per 100 mL of solvent. Air temperature and Altitude Relationship, Caution: many chemicals, in particular sodium hydroxide pellets and conc. Attempt to write the products of thisreaction on your own before continuing (don’t forget to balance equation 10 and identify thephase of the products).HCl(aq) + Na2CO3(aq) à ? Were there any cell(s) in which you did not observe a reaction but think a reaction did occur? However, it is possible that mixing twochemicals will cause no obvious changes. Examples of strong electrolytes aresoluble salts (NaBr and AlCl3), strong bases (NaOH and KOH), and strong acids (HCl, H2SO4,and HNO3). The cation from the second reactant (Pb2+) will combine with the anion from the firstreactant (Cl–) to form the second product, PbCl2. A student mixes silver nitrate with magnesium chloride andobserves a white precipitate. Calculations of the mass/volume percent, mass/mass percent, molarity, molality, and molar concentration of specified solutions will be completed. sulfuric acid, are. Solubility Lab Solution Equilibrium and - PhET 13. Again, you will have to memorize this phenomenon. Lab 5.docx - Unit V Solutions and Solubility LAB REPORT I Purpose The purpose of this laboratory experiment is to distinguish between the different, The purpose of this laboratory experiment is to distinguish, between the different parts of a solution and perform a series of dilutions from a, concentrated solution. Waste solutions from this experiment should be disposed of in the waste container. solubility product lab report answers pdf download. Module 6: Reactions and Solubility Laboratory. Lab Report: Solubility INTRODUCTION Purpose: Explore the relationship between temperature and solubility using a laboratory procedure. Beware this problem in thisparticular experiment, since it is run on such a small scale. Get Your Custom Essay on, Reactions and Solubility Experiment Lab Report. Therefore Mg2+ and NO3– will be present in the form of aqueousions. When a double displacement reaction occurs, the cations and anions switch partners, resultingin the formation of two new ionic compounds AY and XB. Never raise containers of solution, especially corrosive solutions, to eye level or above. Anotherexample (equation 2) is a decomposition reaction used in explosives and fireworks.2 KClO3(s) à 2 KCl(s) + 3 O2(g) (2)Single Displacement: A single displacement reaction involves a more reactive element displacinga less reactive one. It is easiest to. Since this is a double displacement reaction, the zinc cations will switch partners andassociate with the nitrate anions, giving the first product zinc nitrate, Zn(NO3)2(aq), which issoluble in water. When an acid reacts with a base, theproducts are always a salt and water. For example, acid-base reactions are characteristically exothermic reactions,meaning they generate heat energy which can be observed as an increase in temperature usinga thermometer or by the warming of the flask in your hand. Are you scared that your paper will not make the grade? We have a team of professional academic writers who can handle all your assignments.