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Properties of Acids and Bases

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GREEN CHEMISTRY LABORATORY MANUAL Lab 22 Properties of Acids and Bases TN Standard 4.2: The student will investigate the characteristics of acids and bases. Have you ever brushed your teeth and then drank a glass of orange juice? hat do you taste when you brush your teeth and drink orange juice afterwards. Yuck! It leaves a really bad taste in your mouth, but why? Orange juice and toothpaste by themselves taste good. But the terrible taste W results because an acid/base reaction is going on in your mouth. Orange juice is a weak acid and the toothpaste is a weak base. When they are placed together they neutralize each other and produce a product that is unpleasant to taste. How do you determine what is an acid and what is a base? In this lab we will discover how to distinguish between acids and bases. Introduction Two very important classes of compounds are acids and bases. But what exactly makes them different? There are differences in definition, physical differences, and reaction differences. According to the Arrhenius definition, acids ionize in water to + produce a hydronium ion (H3O ), and bases dissociate in water to produce hydroxide ion (OH -). Physical differences can be detected by the senses, including taste and touch. Acids have a sour or tart taste and can produce a stinging sensation to broken skin. For example, if you have ever tasted a lemon, it can often result in a sour face. Bases have a bitter taste and a slippery feel. Soap and many cleaning products are bases. Have you accidentally tasted soap or had it slip out of your hands? 1 GREEN CHEMISTRY LABORATORY MANUAL Reactions with acids and bases vary depending on the substances being reacted. Acids and bases react differently. For example, bases do not react with most metals, but an acid will react readily with certain metals to produce hydrogen gas and an ionic compound. An ionic compound is often referred to as a salt. An example of this type of reaction occurs when magnesium metal reacts with hydrochloric acid. In this reaction magnesium chloride (a salt) and hydrogen gas are formed. Mg(s) + 2HCl(aq) Æ MgCl2 (aq) + H2(g) metal + acid Æ a salt + hydrogen gas Acids may also react with a carbonate or bicarbonate to form carbon dioxide gas and water. The general reaction equation for a reaction between an acid and a carbonate can be represented in this manner: 2- + CO3 (aq) + 2H3O (aq) Æ CO2(g) + 3H2O(l) carbonate + acid Æ carbon dioxide + water The general reaction equation for a reaction between an acid and a bicarbonate is similar and can be represented in this manner: - + HCO3 (aq) + H3O (aq) Æ CO2(g) + 2H2O(l) bicarbonate + acid Æ carbon dioxide + water Acids and bases can also react with each other. When the two opposites react with each other they cancel each other out so that the product formed has neither the acid nor the base properties. This type of reaction is called a Neutralization reaction. The general reaction equation for the reaction between an acid and a base is represented in this manner: + - H3O + OH Æ 2H2O Acid + Base Æ Water An example of a neutralization reaction is when an aqueous solution of HCl, a strong acid, is mixed with an aqueous solution of NaOH, a strong base. HCl when it is + - + - in water forms H3O and Cl . NaOH in water forms Na and OH . When the two solutions are mixed together the products are water and common table salt. Neither water nor table salt has acid or base properties. Generally this reaction is written without the water solvent shown as a reactant. HCl + NaOH Æ H2O + NaCl 2 GREEN CHEMISTRY LABORATORY MANUAL An aqueous (water) solution that has a lot of hydronium ions but very few hydroxide ions is considered to be very acidic. If instead an aqueous solution has a lot of hydroxide ions but very few hydronium ions, it is considered to be very basic. Acids and bases are measured on a scale called pH. The pH is minus the log of the hydronium ion concentration. + pH = -log[H3O ] pH ranges from less than 1 to 14. It lets us quickly tell if something is very acidic, a little acidic, neutral (neither acidic nor basic), a little basic or very basic. A pH of 1 is highly acidic, a pH of 14 is highly basic, and a pH of 7 is neutral. pH indicators, litmus paper, and pH paper can be used to determine whether something is an acid or a base and the strength of its acidity or basicity. An indicator is a substance that turns a different color at a certain pH. Litmus paper is a form of an indicator. It is made by coating paper with the indicator litmus. Litmus is known to change color at a pH of about 7. Either red or blue litmus paper can be purchased. Blue litmus paper remains blue when dipped in a base, but it turns red when an acid touches it. Red litmus paper stays red when dipped in an acid, but turns blue when a base touches it. Another way to more specifically determine an acid or base is through the use of pH paper. pH paper allows us to determine to what degree a substance is acidic or basic. When a substance is placed on pH paper a color appears. The color is compared to a color chart showing the color the pH paper will turn at different pH values. In this experiment, we will observe the neutralization of acids and bases using grape juice as an indicator, and an acid-base reaction of a bicarbonate. We will also test common household products for their acidity or basicity. Objectives • To understand the properties and reactions of acids and bases. • To relate these properties to common household products. 3 GREEN CHEMISTRY LABORATORY MANUAL 4 GREEN CHEMISTRY LABORATORY MANUAL Date:________ Name:_______________________ Period:_________ Pre-lab Questions 1. What is a neutralization reaction? __________________________________________________ __________________________________________________ __________________________________________________ 2. Hydrochloric acid (HCl) is a strong acid. About what pH would you expect it to be? __________________________________________________ 3. Sodium hydroxide (NaOH) is a strong base. About what pH would you expect it to be? __________________________________________________ 5 GREEN CHEMISTRY LABORATORY MANUAL 6 GREEN CHEMISTRY LABORATORY MANUAL Procedure Part 1: Acid-Base Neutralization SAFETY 1. Label 3 medium sized test tubes 1, 2, and Standard. FEATURES , Safety Gloves 2. Pour 10 mL of the dilute grape juice solution into each test Safety Goggles tube. 3. Note the color of the juice in the test tube labeled standard in MATERIALS Table 1. NEEDED 4. Add 10 drops of 1M HCl into test tube 1. Record your Welch’s Grape Juice observations concerning the color change in Table 1 of the 3 Medium size test data section. Use the juice in the test tube labeled standard for tubes comparison. 1 M HCl 5. Add 10 drops of 1M NaOH into test tube 2. Record your 1 M NaOH observations concerning the color change in Table 1 of the 2 droppers data section. Use the juice in the test tube labeled standard for Stirring rod comparison. 25 mL graduated 6. Use pH paper to determine the pH of the solution in each of cylinder the 3 test tubes. Record the pH values in Table 1. 100 mL Beaker Balance 7. Add drops of 1M NaOH to test tube 1 until it returns to its pH paper original color. Record your observations in Table 2. Red and blue litmus 8. Add drops of 1M HCl to test tube 2 until it returns to its paper original color. Record your observations in Table 2. Sodium bicarbonate (baking soda) 9. Use pH paper to test the pH of the 3 solutions. Record the pH values in Table 2. Distilled water Universal indicator Part 2: Acid / Bicarbonate Reaction Vinegar Tomato juice 1. Weigh out 0.5 grams of sodium bicarbonate into a 100 mL beaker. 2. Add 3 mL of distilled water to the beaker and stir until most of the sodium bicarbonate is dissolved. 3. Add ~3 drops of universal indicator to the beaker. Compare the color of the solution to the pH paper indicator chart. Record the color and corresponding pH in Table 3. 7 GREEN CHEMISTRY LABORATORY MANUAL 4. Measure 10 mL of vinegar into a graduated cylinder. 5. Add ~3 drops of the universal indicator to the vinegar. Compare the color of the solution to the pH paper indicator chart. Record the color and corresponding pH in Table 3. 6. Use a dropper to add 3 mL of the vinegar in the 10 mL graduated cylinder into the sodium bicarbonate solution. Note the color change and pH in data Table 3 under mixture. 7. Add 3 mL increments of the vinegar into the sodium bicarbonate and vinegar mixture until the solution’s color changes and becomes neutral. Note the color and pH in Table 3 under “additional vinegar”. Part 3: Testing acidity and basicity of common household products 1. Use the droppers provided to place into different wells of your spot plate a couple of drops of each of the following items: tomato juice, household ammonia, milk, vinegar, lemon juice, and dilute dishwashing liquid. Be sure to label or write down where each item is located in the spot plate. CAUTION: Do not contaminate the items being tested. Be sure to use only the designated dropper for each item. 2. Guess the pH of each of the items before you find the experimental value and record your guess in Table 4.
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