In BaCl2 + Na3PO4, you would combine the two equations and find the charges. Both LiCl and NaOH are soluble in water so it would not form a precipitate and it would stay in the solution. So, in this, you would find the products which are HCl and NaOH. For this, the charges would be Li 1+, OH 1-, Na 1+, and Cl 7. In LiOH + NaCl, you would combine the two equations and find the charges. In an article from OpenStax, it is stated that “the equilibrium constant for the equilibrium between a slightly soluble ionic solid and a solution of its ions is called the solubility product of the solid.” This statement from the article supports the equation of equilibrium. An equation for the occurence of equilibrium is YX(s) ←> Y+(aq) + X-(aq). In a case where an additional solution caused the precipitate to dissolve, equilibrium occured. In a precipitation reaction, an insoluble product is created when the solutions of ions are mixed together. ![]() Because the concentration of the solute affects the solubility, when the precipitate is diluted, the solubility increases. According to Jue Xi Lu, the “factors that affect solubility include the concentration of the solute, temperature, pressure (for gas), and the polarity of the solute and solvent” (Lu and Bhimji, NBCI). The solubility of this precipitate increases when the sample is diluted with deionized water. In this experiment when we diluted a sample, the precipitate became white and cloudy. According to Macritchie, in his article “Effects of Temperature on Dissolution and Precipitation of Proteins and Polyamino Acids,” he states that “with increasing temperature, the range where phase separation occurs.” This statement shows that due to the kinetic energy, the solute molecules are broken apart. In the MgSO4 solution, only When the temperature of the water increases, the solubility of the precipitate also increases. In some steps such as steps a, b, and d in the BaCl2 solution, the precipitate formed at the bottom of the test tube when the precipitate was re-dissolved. When the precipitate was re-dissolved, the majority of the time the precipitate became white and cloudy. Add dilute acid, such as HCl or H2SO4,įourth sample and record any observations Take another sample and try diluting itĬ. Table 2: Ways to re-dissolve the precipitate Observations for BaCl2 Observations for MgSOī. Perhaps if we left the solutions together longer, their reaction would have produced a color. However there were a few exceptions the reaction between BaCl2 and NaOH was slow as well as the reactions between some of the solutions that did not produce a color in their reaction. Solutions that did not produce a color and had a clear color after their reaction were BaCl2 and NaCl, MgSO4 and NaCl, MgSO4 and H2SO4, NaCl and NaCO3, NaCl and H2SO4, NaCl and NaOH, Na2CO3 and NaOH, and H2SO4 and NaOH. Solutions that produced a cloudy white color were BaCl2 and MgSO4, BaCl2 and Na2CO3, BaCl2 and H2SO4, BaCl2 and NaOH, MgSO4 and NaCO3, MgSO4 and NaOH, and Na2CO and H2SO4. Rate of change- slow In Part 1 of the experiment, some solutions changed colors in their reaction while others did not. ![]() Rate of change- slow X X H2SO4 Color- cloudy Quick X X X X NaCl No change Color- clear BaCl2 → heavy metal Observations: Table 1: Solution BaCl2 MgSO4 NaCl Na2CO3 H2SO BaCl2 X X X X X MgSO4 Color- cloudy white Identify the salt that includes a heavy metal.- i. H2SO4 → acidity regulator (added to maintain pH) c. MgSO4 → acidity regulator (strengthens the food structure) v. NaCl → for taste (maintains blood pressure) iii. Give an example of the ways each of these salts is used in the food industry i. Determine which of the salts used in the experiment are sometimes used in foods. During this experiment many salts will be used. Identify the common ions in each of the chemicals you will be using (Use your text to help recognize the polyatomic ions.
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