it with sodium hydroxide (NaOH) solution of accurately known concentration. Titration is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of an identified analyte.¹ Titrant means substance with known concentration existing in buret‚ analyte means substance with unknown concentration in erlenmayer and indicator means chemical which is used to observe acid-base reaction.² In this investigation‚ titrant is NaOH‚ analyte is HCl and indicator
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nCa(OH)2/nHCl = 1/2 ∴ nCa(OH)2 = 1/2 x nHCl = 1/2 x 0.00187 = 9.35 x 10-4 mol ∴ CCa(OH)2 = n/V = 9.35 x 10-4/0.02304 = 0.406 M (3 sf) c) Burette 2. a) CH3COOH + NaOH → NaCH3COO + H2O C = 0.100 M V = 40.25 mL = 0.04025 L V = 50.0 mL = 0.0500 L C = ? known unknown nCH3COOH
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Chem 17 ▪ General Chemistry Laboratory II Experiment 1 Calorimetry INTRODUCTION Chemical reactions are usually accompanied by the evolution (exothermic reaction) or absorption (endothermic reaction) of heat energy. When measured at constant pressure‚ the heat evolved (qp < 0) or absorbed (qp > 0) is equal to the enthalpy change‚ symbolized by ΔH. ΔH is positive for an endothermic process and negative for an exothermic one. If H f is the enthalpy of the final state and Hi of the initial state
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CHEM 113L EXP# 7: Buffer Preparation and pH Measurements Revised . AMB 7-2005 Introduction: Even in quite dilute aqueous solutions‚ acetic acid is very slightly ionized (it would approach 99% ionization only as the concentration approaches 0.0 M): HC2H3O2(aq) + H2O(l) Ka = 1.8 x 10-5. H3O+ + C2H3O2- In general‚ if the acid is not extremely weak‚ the pH of a solution of a weak acid is governed by the concentration of the acid and Ka. Under similar conditions‚ the pH of a solution of a weak base
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Introduction Enthalpy change‚ ΔH‚ is defined as the heat output of a system as it goes through a reaction under constant pressure. It is an important aspect of thermochemistry‚ which is the study of energy changes during a chemical or physical reaction . When we calculate enthalpy change‚ we always assume that the pressure is constant. We are able to calculate enthalpy change numerous ways‚ notably by the increase in heat‚ Q‚ given by an exothermic reaction or the heat absorbed by an endothermic
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have been dancing for 11 years now and competing for 7 years. damn i have to put a lot of stuff. im just gonna copy & paste some random stuff. okayyyyyyyyyyyyyyyyyyyyy????????? okayyyyyyyyyy...... Conclusion: 1. Determine the enthalpy change for NaOH (s) + HCl (aq) → NaCl (aq) + H2O (l) using Hess’s Law. a. Write the balanced chemical reaction and enthalpy change for Part I (1pt) b. Write the balanced chemical reaction and enthalpy change for Part II (1pt) c. Calculate the enthalpy change
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hence the absorption at 540 nm is directly proportional to the protein concentation. Procedures • Mix 1ml of egg white solution and 10 drops of NaOH in the test tube. • Add 1 drop of CuSO4 solution. Mix well and record your observation. • Dissolve one tablet of aspartame or ½ sachet of Equal in 2 ml of water. • Add to the resulting solution 10 drops of NaOH and CuSO4 solution. • Mix well and record your observation. Compare the two results. What Is the principle involved in the biuret test? The Biuret
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BACK TITRATION- DETERMINATION OF THE CARBONATE CONTENT IN GARDEN LIME NAME: OSEI BONSU ERIC ID: 3906409 EXPERIMENT: I.2.2.1.
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Week-2-Solubility Name: ___________________________________________________ Section: ______________ For Instructor Use Only POST-LAB REPORT FOR THE SOLUBILITY EXPERIMENT I) Conclusion: Write the conclusions regarding your observations and results obtained from each part 2A‚ 2B‚ 2C
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blue) (e) Part V [Cu(H2O)6]2+ (aq‚ blue) + Zn(s‚ gray) → Cu(s‚ brown) + Zn2+ (aq‚ colorless) + 6H2O (l) Zn(s‚ gray) + 2H3O+ (aq) → Zn2+ (aq‚ colorless) + H2(g) + 2H2O (l) 4 a. What test will you perform to determinate when you have added sufficient NaOH solution in Part II? We will use red litmus paper‚ an acid base indicator that is red in acidic solution and
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