Suppose a household product label says it contains sodium hydrogen carbonate (sodium bicarbonate). How would you test this material for the presence of sodium bicarbonate? To test for the presence of sodium bicarbonate you could collect a sample of the household product and add HCl to it and see if you observe any CO2 bubbles. B. You know what color phenolphthalein and bromothymol blue turn when testing an acid or a base. Use the empty pipet in the Auxiliary Supplies Bag to test several (at least 3) household items incl
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Sulfate ion in the reducing agent 10. In which set are the substances arranged in order of decreasing solubility in water? A. Al(OH)2 > Mg(OH)2 > NaOH B. BaSO4 > CaSO4 > MgSO4 C. CaCO3 > NaHCO3 >Na2CO3 D. AgCl > AgBr > AgI 11. What Volume of 10M HCl solution is required to prepare exactly 500 mL of a 0.60M HCl solution? A. 10mL B. 14mL C. 30mL D. 40mL 12. What is the molarity of a solution made by dissolving 9.56g of sodium acetate(82.03g/mol) in water and diluting to 650mL? A. 0.179M B. 1.206M
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and ethanol as the solvent. 9.2 Reactions with Bases 1. Prepare 3 test tubes with 3 drops of 5% NaOH. 2. Add 5 drops of 50 mg of acetic acid‚ benzoic acid and oxalic acid. 3. Shake and observe the changes. 4. Repeat the procedures using 5% NaHCO3. 9.3 Oxidation Reactions 9.3.1 Reaction with KMnO4 1. Prepare 4 test tubes with 2 ml of water and add 1 ml of conc. H2SO4 to each. 2. Place 4 drops (0.1 g) of formic acid‚ acetic acid‚ benzoic acid‚ and oxalic acid‚ each into a different test
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write the net ionic equation for the reaction: a. ZnSO4 (aq) + BaS (aq) → ? b. NaHCO3 (aq) + Ca(OH)2 (aq) → ? 3. Assign an oxidation number to each atom in: a. Al2O3 b. HAsO42c. NaMnO4 4. Identify the reducing agent and the oxidizing agent in the following reaction: MnO4- + 5 Fe2+ + 8 H+ → Mn2+ + 5 Fe3+ + 4 H2O 1. Balance the equation: FeS (s) + HCl (aq) → FeCl2 (aq) + H2S (g) Given 13.2 g FeS and 10.2 g HCl‚ determine: (a) how much H2S is formed‚ (b) how much excess reactant is left.
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skin. -Acids change litmus red. -Acids become less acidic when mixed with bases. 2) Write down the chemical formulae of five Acids. -Sulfuric acid: H2SO4 -Boric Acid: H3BO3 -Carbonic Acid: CH2O3 -Citric Acid: H3C6H5O7 -Hydrochloric acid: HCl 3) Write down the chemical equation that shows what happen to acids when they dissolve in water. 4) What determines that some acids are stronger than others. 5) Describe how using Universal Indicators solution‚ blue litmus paper and pH meter can
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In the experiment‚ 0.3 g of mixture was dissolved in 3 mL of t-butyl methyl ether in a centrifuge tube. Then‚ 2 mL of 0.5 M NaHCO3 was added‚ shaken for one minute‚ and allowed to sit for two minutes so the layers could separate. The lower water layer was removed with a Pasteur pipette and placed in a test tube labeled “Acid.” Next‚ 0.5 mL of distilled water was added to wash the ether layer in the centrifuge tube and then discarded. 2 mL of 0.5 M NaOH was added to the remaining layer‚ shaken for
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had 6M and carefully added 2 drops to well A1. Next‚ I stirred the water and the HCl in the well with a toothpick to ensure that the HCl was diluted as much as possible. Then‚ taking a pipet labeled Hydrochloric Acid‚ I sucked up the diluted HCl and placed the pipet upside down in a well plate for standby until needed for the experiment. For Ammonia and Sodium Hydroxide‚ I followed the same procedure that I did for HCl with the exception that the diluted solution for Ammonia was made in well A2 and
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Q1. Why should a four place analytical balance not be used in weighing a sample if the manual requests only one decimal place accuracy? Ans. We use the analytical balance where we need to weigh the small amount which needs a high degree of accuracy. Whereas‚ the manual requests only one decimal place accuracy which is not that much important and the time is consumed more to use the analytical balance with four decimal places. Q2. How is the pH meter calibrated? Ans. Firstly‚ The pH meter is calibrated
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are equal. Hypothesis/Prediction: Experiment 1: All of the kernels will pop due to the increase in temperature‚ presence of a catalyst and pressure. Experiment 2: The Ka value is going to be high. Experiment 3: If the concentration of HCl increases‚ then the dissolving of magnesium in the solution will occur faster. The decreasing of temperature will cause the magnesium to take longer to dissolve. When using pieces of magnesium as opposed to a strip‚ it will dissolve faster and lead
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filter paper (coffee filters work well) 1 liter beaker Six 250 mL beakers Professors/Instructors please specify which chemicals you wish to use. Some that we may have on hand are: household ammonia (NH3) baking soda (sodium bicarbonate‚ NaHCO3) washing soda (sodium
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