Jillian Mulrooney & Emma Zika Test Questions Concept 1: Write the name of the acids and bases from given formula Q-1-1: Name the following base: NaOH Q-1-2: Name the following acid: HCN Concept 2: Write the formula form given name of acids and bases Q-2-1: Write the formula for the following acid: lithium hydroxide Q-2-2: Write the name for the following base: hydrobromic acid Concept 3: Distinguish between acid‚ base‚ neutral compounds based on their properties which can be tested in a
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Investigating the effect of pH on amylase activity This practical allows you to: * discover how pH affects the rate of an enzyme controlled reaction * evaluate the experimental procedure Procedure SAFETY: Follow your teacher’s instructions for handling the solutions. Wear eye protection when handling the iodine solution. Investigation * Place single drops of iodine solution in rows on the tile. * Label a test tube with the pH to be tested. * Use the syringe to place
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The purpose of this experiment was to test how effective certain homogenates were as buffers. Buffers are devices that keep pH within maintainable boundaries so something can function. When something is too basic (has too much OH-) the buffer adds H+ and vice versa in order to create water to keep the pH at an acceptable range. Each group (I was with William Yung for this experiment) was tasked with testing one homogenate. The homogenate tested by our group was liquid spinach. Each team added HCl
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1. Introduction 2 2. Graphs 2.1 HC2H3O2 titration curve 3 2.2 H3PO4 titration curve 4 2.3 H2A titration curve 5 3. Calculations 3.1 HC2H3O2 Calculations a. Exact molarity of the HC2H3O2 solution 6 b. Ka from the initial pH 6 c. Ka from the pH at halfway point 6 d. Ka from the pH at the end point 7 3.2 H3PO4 Calculations a. Exact molarity of the H3PO4 solution 7 b. Ka1 from
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E XPE RIME NT 4 . 5 Reactions of acids Aim To investigate and compare some reactions of a strong acid‚ hydrochloric acid‚ and a weak acid‚ ethanoic acid (common name‚ acetic acid) Equipment Dropper bottles containing: • 0.1 M hydrochloric acid‚ HCl • 0.1 M ethanoic acid (acetic acid)‚ CH3COOH • 0.1 M sodium hydroxide‚ NaOH • 1 M hydrochloric acid‚ HCl • 1 M ethanoic acid (acetic acid)‚ CH3COOH • universal indicator solution • limewater (calcium hydroxide‚ Ca(OH)2) Marble chips (calcium carbonate
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To identify an unknown sample‚ there were several steps that helped determine the molecular structure and the name of the sample. When Belle #9 (unknown) was given to me‚ it’s physical state and color was recorded on the data sheet. Since the sample was a pure liquid‚ there was no need for distillation. Next‚ a solubility test was given. When one drop of the unknown liquid was added to about 2 mL of water‚ the sample was tested to be soluble due to the dissolubility between the two compounds. By
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The full strength 1M HCl acid had a pH level of 3.12 (Table 3.1). Sample A2 to A4 remained in the pH 3 level‚ while sample A5 and A6 had a pH range of 4 (Table 3.1). The pH level for 1M HCl dilutions slightly increased between each sample (Table 3.1). The diluted solutions of 1 M NaOH showed a few unexpected results. The original solution of 1 M NaOH was at a pH level of 11.50 (Table 3.1). However‚ the pH of sample B2 increased to 12.81 (Table 3.1). The remaining samples had a decreasing pH pattern
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I. Introduction The purpose of this experiment is to determine the pH values of acids‚ bases‚ and buffers of distilled water and 10.0 buffer using measured concentrations of Sodium hydroxide (NaOH) and/or Hydrochloric acid (HCl). Acid is a compound typically having a bitter taste and capable of nullifying alkalis and releases hydrogen ion when added to a solution‚ or containing an atom that can accept a pair of electrons from a base (McKinley‚ Dean O’Loughlin‚ & Stouter Bidle‚ 2016). Bases are water-soluble
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In order to determine the acidity of certain substances‚ we used moist and dry pH paper (litmus tests)‚ and observed the results. First we used dry pH paper to test the acidity of household ammonia‚ and it turned yellow. According to the legend‚ this indicates a weak acid. This is‚ however‚ not accurate as the vapor of the household ammonia wasn’t able to react as strongly with the pH paper since it was dry. Then‚ we used moist DI water pH paper with the same substance‚ household ammonia‚ and it
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Purpose: The purpose of this experiment is to analyze four drinking water samples from different places using four of the standard drinking water tests required by the EPA. The experiment will be performed by a four person group‚ with each person providing a different water sample. The four tests to be performed are: pH‚ conductivity‚ phenolphthalein and total alkalinity‚ and total and non-carbonate hardness. Data from these four tests will be gathered and analyzed‚ drawing conclusions “about
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