|4|~2.5| Questions 1. Compare and contrast acids and bases in terms of their H+ ion and OH- ion concentrations. Vinegar – Acidic with a low pH of around 3. Sodium – Basic – with a higher pH scale around 7.5 Milk – I thought would be basic but it’s actually more acidic‚ around 6.5 Orange Juice – Acidic actually around 3.5 Hand soap – Basic around 9 pH Lemon juice - most acidic thing I tested around 2.5 2. Name two acids and two bases you often use. Acids: I drink Orange Juce everyday along
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Writing Practical Reports Aim: To observe what happens during and after a chemical reaction. Equipment: Concentrated nitric acid in a glass dropping bottle Small pieces of Copper 250ml Beaker 2 M Lead nitrate in a dropping bottle 2 M Potassium iodide in a dropping bottle 2 M Copper sulfate in a dropping bottle 2 M Sodium hydroxide in a dropping bottle 2 M Hydrochloric acid in a dropping bottle 4 Pyrex test tubes Test tube rack Spatula Bunsen burner‚ gauze
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it is also equally possible that the solution was not shaken properly in order to avoid the over-addition of sodium bicarbonate. The failure to perform these steps correctly could have resulted in this loss of product due to the fact that too much base could have reacted with the product‚ resulting in a product that could have been washed by water‚ but
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that our data in the experiment was “good data”. We had the expected positive results occur from the identification experiments. We made sure to measure everything correctly. We correctly identified the precipitate Zn(OH)2 by performing the acid and base test on our precipitate. We received a positive result for each test performed for the presence of the zinc hydroxide compound. It was interesting to note the appearance of the zinc hydroxide from only the mixture of zinc‚ iodine and deionized water
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10th & 17th Introduction： The purpose of this lab is to observe the titration between acid and base‚ and calculate the morality of unknown solution base on the volume required to reach equivalence point and stoicheiometry. There are two groups of experiments. The first one is the reaction between nitric acid and sodium hydroxide which is a reaction between strong acid and strong base‚ so‚ theoretically‚ the pH value of the the mixture of these two solution at the equivalence point in the
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Mg(OH)2 and swirled by hand This was continued until it turned from pink in colour back to a colourless solution The amount of HCL was then recorded in a data table This titration was carried out four times‚ the first being use for a base line Theory Hydrochloric Acid | + | Magnesium | | Magnesium Chloride | + | water | 2HCl (aq) + Mg(OH)2 (aq) ⇒ MgCl (aq) + 2H2O (l) Neutralization Reaction Hydrochloric acid reacts with Mg(OH)2 the products
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1%) concentration which permits detection of the utilization of this substrate only. The acid base indicator phenol red- also incorporated to detect carbohydrate fermentation that is indicated by a change in color of the medium from orange-red to yellow in the presence of acids. a. Method to inoculate slant: stab and streak procedure which requires insertion of sterile straight needle from the base of the slant into the butt. Upon withdrawal‚ the slanted surface of the medium is streaked. Determining
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sodium hydroxide solution‚ NaOH Actual concentration of sodium hydroxide solution used can be calculated by using the formula : MaVa = A MbVb B Where : M = Molarity; V = volume; a=acid; b = base; A = Number of moles of acid B = Number of moles of base Balanced chemical equation C8H5KO4(aq) + NaOH (aq) C8H4KO4Na (aq) + H2O From equation‚ 1 mol of C8H5KO4 react with 1 mol of NaOH 1.When Ma = 0.5 mol/dm³‚ ((0.5 mol/dm³) ( 0.023 dm³ ))/(Mb ( 0.066 dm^3))= 1/1
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being used increasingly as resolving bases for racemization since phenylethylamine is synthesizable and can readily be resolved into its antipodes. In contrast to naturally occurring alkaloids theoptically active forms of 1-phenylethylamine can be provided in any desired amount for technical purposes. In the racemization of synthetically prepared resolving bases‚ two antipodes are necessarily produced in equal amounts. However‚ it is largely only one resolving base that is needed for the racemization
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Figure 1: Titration curve of 0.160 grams of an unknown diprotic acid that was dissociated in distilled water. Shown is the pH versus the volume in milliliters of 0.1 M NaOH‚ a strong base‚ added to the solution. The initial pH reading of the solution was a pH of 2.60. Although the pH of the ½ equivalence point was unknown‚ it could be estimated by halving the volume of NaOH used at the first equivalence point. At the first equivalence point‚ 13.63 milliliters of NaOH had been added to the unknown
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