Hydrochloric-Acid Written By Kahlil Zione Date:02/02/05 Abstract: We observed the reaction between zinc and hydrochloric acid and recorded it in a table and learned wether the percentage of zinc is effected by the amounts of both substances added to the solution. Introduction The purpose of this experiment is to determine if the amount of zinc and hydrochloric acid will effect the percentage of the zinc in the out coming solution. We are reacting zinc metal with hydrochloric acid to produce
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ACID CONSUMPTION AND ACID RUNAWAY IN A SULFURIC ACID ALKYLATION UNIT Presented By Sarah Hoelzle Process Engineer DuPont™ STRATCO® Clean Fuel Technologies 11350 Tomahawk Creek Parkway Suite 200 Leawood‚ KS 66211 September 2007 Copyright 2007 DuPont™ STRATCO® Clean Fuel Technologies Table of Contents Page Number I. ACID CONSUMPTION FUNDAMENTALS.....................................................................1 Figure 1 - Diluent Production vs. Acid Strength- 40/60 C3=/C4= .....
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acid + metal -------->salt + hydrogen acid + metal oxide--->salt + water acid + metal carbonate---->salt + water + carbon dioxide Element | Symbol | Valency | Hydrogen | H | 1 | Oxygen | O | -2 | Carbon | C | 4 | Calcium | Ca | 2 | Iron | Fe | 2 | Aluminium | Al | 3 | Sodium | Na | 1 | Potassium | K | 1 | Magnesium | Mg | 2 | Zinc | Zn | 2 | Copper | Cu | 2 | Silver | Ag | 1 | Lead | Pb | 2 | Chloride | Cl | -1 | Sulphate | SO4 | -2 | Hydroxide | OH
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reactions to remember: Acid reactions: acid + base salt + water acid + metal salt + hydrogen gas acid + carbonate carbon dioxide gas + salt + water Formation of hydronium: H+ + H2O H3O+ Reactions of various oxides with water: Non-metal (acidic) oxides: CO2 (g) + H2O (l) H2CO3 (aq) (carbonic acid) SO2 (g) + H2O (l) H2SO3 (aq) (sulfurous acid) 2NO2 (g) + H2O (l) HNO3 (aq) + HNO2 (aq) (nitric and nitrous acid) P2O5 (g) + H2O (l) 2H3PO4 (aq) (phosphoric acid) Metal (basic) oxides:
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properties of acids with the general properties of bases. Acids: Aqueous solutions of acids have a sour taste. Acids change the color of acid-base indicators. Some acids react with active metals and release hydrogen gas‚H2. Acids react with bases to produce salts and water. Acids conduct electric current. Bases: Aqueous solutions of bases taste bitter. Bases change the color of acid-base indicators. Dilute aqueous solutions of bases feel slippery. Bases react with acids to produce salts
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Abstract The objective of this experiment was to observe multi-step purification of benzoic acid after performing the extraction from a mixture containing benzoic acid‚ cellulose‚ and methyl orange. Recrystallization was done to remove impurities from the sample. The amount of BA recovered during recrystallization is much less than the extracted amount of BA. The difference between the pure and impure samples was observed by comparison of melting points. It was found that impure samples will have
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was conducted in order to determine the chemical composition of an unknown organic acid. A known mass of acid was dissolved into 30mL of either water or methanol (depending on solubility) and titrated with standardized sodium hydroxide. Data from this allowed the molar mass of the acid to be calculated if it was either monoprotic or diprotic. Titration Table: |Trail |Acid Used (mg) |Concentration of base |Volume of base (mL)
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An acid is a substance with particular chemical properties including turning litmus paper red‚ neutralizing alkalis‚ and dissolving some metals. It can be corrosive or it can be sour liquid of this kind. Acids are also all around us in everyday life‚ for example‚ carbon dioxide gas dissolves in rain to form carbonic acid (a weak acid). We find acids in many foods‚ such as ethanoic acid in vinegar. These acids are not hazardous. Some acids‚ which are found in the laboratory a car battery are too dangerous
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of the amount of unknown acid X measured in grams (±0.001g) Table 2: Table of reading of the burette initially filled with 25mL of 0.201moldm-3 sodium hydroxide (NaOH) to titrate 25mL (±0.03mL) of unknown acid X in mL (±0.05mL) after each titre. Reading on the burette initially filled with 25mL of 0.201moldm-3 NaOH (±0.05mL) First titre 21.3 Second titre 18.2 Third titre 15.2 Fourth titre 12.0 Qualitative data Observations: When dissolving the acid X in the water‚ most of it
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to neutralise the acid‚ the number of moles of HCl neutralized by the ant-acid would be greater. For example; by using mole ratio‚ the number of moles of HCl reacted with the NaOH is 0.00216 moles (1 tablet of Quick-eze). The number of moles of HCl that were neutralized by Quick-eze was 0.00284 moles. Nevertheless‚ 0.00173 moles of HCl neutralized by Gaviscon. This explains that the excess amount (no of moles) of HCl was greater‚ which reacted with the NaOH. Quick-eze (ant-acid)
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