Data Table 1: Add 0.1M HCl Drops pH Paper Color 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 Data Table 2: Add 0.1M NaOH Drops pH Paper Color 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 Data Table 3: Add 6M HCl Drops pH Paper Color 0 1 2 3 4 Data Table 4: Add 6M NaOH Drops pH Paper Color 0 1 2 3 4 5 Data
Free PH Acid dissociation constant Buffer solution
alkali. Different buffer systems are effective over different pH ranges. The aim of this experiment is to investigate the ranges at which three different buffer systems: Acetic acid/NaOH‚ Tris/HCl and Gylcine/NaOH are effective. Materials and Methods Three titrations were carried out: Acetic acid/NaOH‚ Tris/HCl and Gylcine/NaOH. 25ml of the weak acid or weak base was put into a beaker and its pH measured. Then it was titrated with the strong acid or strong base respectively while measuring the pH
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Experiment 2 Title: preparation of a halogenoalkane Objective: To synthesis 2-cholo-2-methylpropane by using corresponding alcohol and HCl(aq). The reaction is via SN1 of tertiary alcohol. Techniques: i) Distillation of the reactant and the product ii) Purification by separating funnel Theory: In the experiment‚ SN1 reaction take place‚ HCl is added to initiate the reaction. The R-OH attack the H+ with the lone pair on O. Then the R-O+H2 bond breaks the release a water molecule and
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acid-base titration curves help to find the pKa‚ Ka‚ and pH at equivalent point. At the beginning pH for HCl is 1.90 which is lower than the 3.28 for acetic acid; thus‚ strong acid (HCl) means lower pH and weak acid (acetic acid) means higher pH. Then at the equivalent point for the titration HCl-NaOH the pH is 7‚ which mans that is neutral‚ in other words there are enough NaOH mmol to neutralize the HCl mmol present; also‚ the solution contains only water and NaCl the salt derived from the titration made
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alcohol and acid by the concentrations of ester and water. Methods/Procedure: First begin by mixing up and standardizing a 500mL solution of NaOH to titrate. For each of the six bottles‚ measure the directed amounts of ester‚ water‚ alcohol‚ and HCl. The bottles of different solutions will be left to come to equilibrium for two weeks. Once the NaOH is standardized‚ the solutions in the bottles have come to equilibrium‚ and a molarity is calculated‚ use the molarity of NaOH to discover how many
Free PH Acid dissociation constant Hydrochloric acid
NaOH according to this equation: HCl (aq)+ NaOH(aq) → NaCl(aq) + H2O(l) HCl is a strong acid‚ NaOH is also a strong base‚ therefore they will dissolve completely. By adding NaOH into HCl‚ the hydrogen ions neutralized with hydroxide ions‚ the theoretical endpoint and then the solution will be weak basic solution. The endpoint
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For the buffer 2 solution‚ the original pH was 5.82 with 10mL of buffer and 10mL of DI water. We added 1.5mL of NaOH this time‚ and the pH went up to 7.81. This is a difference of 2. 2. What is the difference between a’smart’ and a’smart’? For adding HCl‚ we started with buffer 1. The
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ACID BASE TITRATION OBJECTIVES 1. To demonstrate the basic laboratory technique of titration 2. To learn to calculate molarity based on titrations INTRODUCTION Molarity (M) or molar concentration is a common unit for expressing the concentration of solutions. It is defined as the number of moles of solute per liter of solution (or millimoles of solute per milliliter of solution). The concentration of a basic solution can be determined by titrating it with a volume of a standard acid solution (of
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