Chapter I Introduction A.) Background of the Study: The Acids‚ bases and salts in the pH range are among the most important chemical compounds used by chemists. For instance‚ hydrochloric‚ phosphoric and citric are acids used to make mineral stain removers‚ toilet bowl cleaners‚ metal cleaners and rust removers. A variety of maintenance chemicals contain these compounds. Alkali maintenance chemicals like degreasers‚ oven cleaners and drain openers contain bases such as Sodium Hydroxide (NaOH)
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Experiment 20: pH Titration: Phosphoric Acid in Cola Drinks Post-lab Assignment or Report The post-lab report for this experiment is due at the beginning of the following lab period. Student notes for the lab will be available on the lab T-Square site. Learning Objectives Students will be able to... • Use a known mass of solid acid to determine an unknown concentration of a basic solution (this process is called “standardization”). • Execute a titration using good‚ reliable technique.
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contains four sections‚ SECTION A to SECTION D. Instructions: Answer all questions in SECTION A - SECTION D. Make sure that the section heading is included and your answers are correctly numbered. The assignment must have a completed cover sheet. It must be placed in the drop-box on or before the deadline. st SECTION A ELECTRONIC STRUCTURE & IONIZATION ENERGY 1. 2. Write the electronic structure in s‚p‚d notation of the following: O‚ Na‚ Na+‚ Al‚ Cl- and Co
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CHAPTER 8: ACID – BASE EQUILIBRIUM 4 U CHEMISTRY P 526 – SEE KEY IDEAS - examples f acids and bases. 8.1: The Nature of Acid – Base Equilibria: - Arrhenius acids – H ions in water‚ bases – hydroxide ions in water - acids – sour‚ turn blue litmus to red (pink)‚ conduct electricity - bases – bitter‚ soapy taste‚ slippery‚ conduct electricity‚ turn red litmus to blue Bronsted – Lowry Theory: - acids – donate proton‚ bases accept proton - ex: HCl donates proton to water
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buffers are effective and provide opportunity for the use of the Henderson-Hasselbalch equation to prepare a buffer of a specific pH. Three different buffer systems were initially investigated; volumes of weak acid and weak bases of specified concentration were prepared and titrated against strong acid or strong base solutions with pH readings taken at frequent intervals to determine pH ranges over which the systems are most effective. The Henderson-Hasselbalch equation was used to calculate an appropriate
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in pH with consecutive 1mL additions of either a strong acid (HCl) or base (NaOH). The experiment entailed preparing a combination 10 buffered and non-buffered solutions and then monitoring the pH changes as a strong acid or base was added to the solution. By performing this experiment‚ it was found that with increasing amounts of buffer in the prepared solutions there was better resistance against pH changes. This was because the strong acid or base was converted to it’s weak conjugate. The solution
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Check your bubbling carefully – bubbling errors will not be negotiated. Turn in your scantron and retain your exam (with your answers circled). Potentially useful info : Kw = 1 x 10‒14 at 25°C pH = −log [H3O+] pH = pKa + log ([base] / [acid]) R = 0.0821 atm•lit/mol•K or 8.314 J/mol•K Kp = Kc(RT)∆n(gas) ΔG = ΔH – TΔS ΔG° = ΔH° – TΔS° ΔG° = −RTlnK ΔG = ΔG° + RTlnQ ΔG°rxn = ∑mΔG°f(prod) − ∑mΔG°f(react) (likewise for ΔH°rxn and ΔS°rxn) ln(K1/K2) = (ΔH°rxn / R){(1/T2) – (1/T1)} The
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Problem What effect does the different concentration of hydrochloric acid have to the rate of diffusion of agar that is dissolved with sodium carbonate and phenolphthalein? Introduction Diffusion is a process where the molecules intermingle as a result of their kinetic energy of random motion and is the net movement of like molecules down their concentration gradient‚ which is the energy inherent in their constant molecular motion makes them collide and careen outward from the region of higher
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of indicators and instrumental detection of equivalence points in acid-base titration. Objective 1. To understand the importance of choosing suitable indicators for detecting the end points of acid-base titrations. 2. To obtain titration curves for some acid-base titrations. Materials and Method (Please refer to the General Chemistry BPH2012 practical manual pg 4-5) Results Part I: Suitability of Indicators A.Strong acid-weak base titration 1 2 Initial Burette Reading (mL) 19.50
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Chemical Evolution‚ Water‚ Non-covalent bonds‚ Acid/base‚ pH 1. i) Convert using scientific notation to liters: 4 nanoliters‚ 4 x 10-9 L‚ 20 microliters‚ 2x10-5 L‚ 35 milliliters‚ 3.5 x 10-2 L‚ 10 deciliters‚ 1 L‚ 7 kiloliters 7 x 103 L ii) Convert using scientific notation to grams: 6 mg‚ 6 x 10-3 g‚ 21 µg‚ 2.1 x 10-5 g‚ 503 ng‚ 5.03 x 10-7 g‚ 10 kg‚ 1 x 104 g 2. Which of the following properties of water explains its ability to dissolve acetic acid? (there may be more than one correct answer) a
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