Diffusion of Hydrochloric Acid into Different Sizes of Agar Blocks Aim: Investigating the relationship between the diffusion and the surface area to volume ratio‚ with agar and hydrochloric acid. Research Question: How does the difference in surface area to volume ratio affect the diffusion? Hypothesis: As the area to volume ratio increases‚ the time taken for a complete diffusion will also increase. Background Information: Agar is a jelly like substance and in this experiment‚ agar
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An Experiment to find the Concentration of a Sample of Acid Rain Plan Aim When a metal is extracted from its ore often sulphur dioxide is produced. When sulphur dioxide is dissolved in water it forms a strong acid called sulphuric acid. Sulphuric acid is often sold as a useful by-product‚ but also gets into the water cycle and forms acid rain. In this experiment‚ I have been given a sample acid rain of concentration between 0.05 mol dm-3 and 0.15 mol dm-3 and my aim is to find out exactly what
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of Bromine to trans-Cinnamic Acid Introduction/Abstract: The purpose of this experiment was to carry out the bromination of trans-cinnamic acid‚ to determine the stereochemistry of the dibromide product of 2‚3-dibromo-3-phenylpropanoic acid‚ and find out whether the reaction proceeds by the usual bromonium ion mechanism or some other mechanism. In this experiment trans-cinnamic acid was mixed with glacial acetic acid and stirred in which then bromine/acetic acid solution was added to the mixture
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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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in acid-base titrations Objectives 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. Introduction Indicator is usually a weak organic acid or base that has distinctly different colours in its protonated and deprotonated forms. There are 4 types of acid-base titrations such as strong acid-weak base titration‚ weak acid-strong base titration‚ strong acid-strong
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Ka‚ Acid Dissociation Constant and Kb‚ Base Dissociation Constant (Lesson Recap) Ka‚ Acid Dissociation Constant Ka- is the Keq for the dissociation for a weak acid. e.g Acetic Acid‚ when dissolved in H2O CH3COOH (aq) + H2O (l) (ACID) (BASE) CH3COO (aq) + H3O(l) (CONJ BASE) (CONJ ACID) CH3COOH (aq) + H2O(l) ↔ CH3COO (aq) + H3O(l) *ONLY weak acid and back can be reversible Equation for Ka : Keq= [CH3COO(aq)] [H3O(l)][CH3COOH(aq)] [H2O(l)] Keq x [H2O
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Henry Su December 12‚ 2001 Chapter Notes Chemistry 221 Chapter 13 Dr. Rahni Titrating Polyfunctional Acids and Bases 13A—Polyfunctional Acids -Phosphoric Acid is a typical polyfunctional acid H3PO4 + H2O ( H2PO4- + H3O+ Ka1 = [H3O+] [H2PO4-] = 7.11e-3 [H3PO4 ] H2PO4- + H2O ( HPO4-2 + H3O+ Ka2 = [H3O+] [H2PO4-2] = 6.32e-8 [H2PO4- ] HPO4-2 + H2O ( PO4-3 + H3O+ Ka3 = [H3O+] [PO4-3] = 4.5e-13 [HPO4-2]
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exactly. Rate Equation Rate Expression A mathematical expression which relates the rate to the concentrations of substances involved in the reaction Rate Constant‚ k This is the multiplying constant in the rate equation‚ e.g.‚ Rate = k [A].[B]2 It has a constant numerical value as long as temperature does not change. Rate constants increase as temperature increases. Order of Reaction This is the numerical power to which the concentration of a substance is raised in the rate equation.
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The dissociation of protons from oxalic acid proceeds in a stepwise manner as for other polyprotic acids. Loss of a single proton results in the monovalent hydrogenoxalate anion HC2O4−. A salt with this anion is sometimes called an acid oxalate‚ monobasic oxalate‚ or hydrogen oxalate. The equilibrium constant (Ka) for loss of the first proton is 5.37×10−2 (pKa = 1.27). The loss of the second proton‚ which yields the oxalate ion has an equilibrium constant of 5.25×10−5 (pKa = 4.28). These values imply
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De Leon‚ Jo-Anna Maria N. 3ChEA Group No. 2 Experiment No. 5 Spectrophotometric Determination of pKa I. Introduction The equilibrium constant of the dissociation of an indicator in water will be determined experimentally using spectroscopic method.This experiment aims to demonstrate the principle of equilibrium and the interaction of matter with light. II. Methodology Figure . UV-VIS Spectrophotometer 10 solutions covering the entire pH range from 1 to 13 were prepared
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