Editing Student-Directed Comparison Of Strong And Weak Acids And Bases
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This lab will consists of two parts as follows:<br> a) Each group will make one of the solutions below and place around 20.ml into a 100.ml beaker and label it with Molarity and solution's chemical formula. <br> b) Each group will determine the pH with a) pH paper (record pH to the tenth place) and b) <nowiki>LabQuest2</nowiki> pH probe of each of the 4 solutions. <br> c) Each group will also determine the color change on the red and blue litmus paper.<br> c) Each group will then calculate (in their lab book) the theoretical pH of each solution. Show all work as if calculations are part of a test.<br> <br> <br> The solutions to be made are (any leftover solution will be put into plastic containers with label of molarity and chemical formula):<br> a) 1.0M HCl solution, 500ml of this solution (from a concentrated, (concen), 12.0M solution) <br> b) 1.0M HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> solution, 500.ml of this solution (from a concen 12.0M solution)<br> c) 1.0M <nowiki>NaOH</nowiki> solution, 500.ml of this solution (from a solid <nowiki>NaOH</nowiki>). <br> d) 1.0M NH<sub>4</sub>OH solution (it is called ammonium hydroxide but the other name is ammonia water solution), 500..ml of this solution (from concen 14.5M solution)<br> e) 2.0M HCl solution, 500mL of this solution from concen 12.0M solution<br> <br> Please show your calculations on making "your" solution. Show all work as if it was a problem on a test. Share with other groups so everybody have the calculations needed to make the 4 solutions (these calculations will be part of your lab write-up.)<br> <br> *[[Question for Student-Directed Comparison of Strong and Weak Acids and Bases]]<br> <br> ----<br> 2017-2018 AP Chem Extension <br> <br> a) To the 1.0 M HCl solution, add a few grains of <nowiki>NaCl</nowiki>, stir/dissolve salt and record new pH.<br> <br> b) To the 1.0M HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> solution, add a few grains of Sodium acetate ( <nowiki>NaC</nowiki><sub>2</sub>H<sub>3</sub>O<sub>2</sub>), stir/dissolve and record new pH.<br> c) To the 1.0M <nowiki>NaOH</nowiki> solution, add a few grains of <nowiki>NaCl</nowiki>, stir/dissolve salt and record new pH.<br> d) To the 1.0M NH<sub>4</sub>OH solution, add a few grains of Ammonium chloride ( NH<sub>4</sub>Cl ), stir/dissolve and record pH. <br> Question for 2018-2018 AP Chem Extension. (Will answer these questions on different sheet of paper)<br> <br> 1. What would <nowiki>LeChatlier's </nowiki> Principle about adding <nowiki>NaC</nowiki><sub>2</sub>H<sub>3</sub>O<sub>2</sub>) to a HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> solution? What would the new Equilibrium "bucket" look like and do any concentrations change? Do those changes the pH of the new solution compared to the original solution?<br> <br> <br> 2. Similarly, how would the same thing happen when you added NH<sub>4</sub>Cl to the NH<sub>3</sub> ( i.e. NH<sub>4</sub>OH solution).<br> <Br> <br> 3. Does the same thing happen when added the <nowiki>NaCl</nowiki> to either the HCl solution and/or <nowiki>NaOH</nowiki> solution? Explain?<br> <br>
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