aqueous solution‚ when acetic acid reacts with a strong base like sodium hydroxide (NaOH)‚ the hydroxide ion from the base reacts with the hydrogen ion from the acid to produce water. The remaining sodium ion (Na+) and the polyatomic (CH3COO-) acetate ion form the soluble salt sodium acetate‚ NaCH3COO(aq)‚ which remains dissociated in solution. This acid-base reaction is called a neutralization reaction and has the general form: Acid + base a salt + water For the reaction of acetic acid with
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Lab Report # 11 By: Andrew Hoitt CHEM 105 Lab 11/29/2012 Lab # 11 – Acid - Base Titration Introduction: The purpose of this lab is to determine the molarity (M) of an unknown HCl solution. A NaOH solution will be made and its molarity calculated. A sample of the NaOH solution will be titrated against the unknown HCl solution to calculated the volume needed to neutralize it. With these volumes the unknown molarity can be calculated. Theory: Solutions
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strong base and when it is titrated with a strong acid the equivalence point will be expected to be a pH of 7 (wyzant.com‚ Feb. 12). NaOH is also known as caustic soda‚ it is soluble in water‚ ethanol‚ and glycerol but is insoluble in acetone and ether (nap.edu‚ Feb. 12). When Phenolphthalein a weak acid and when hydroxide ions (NaOH) is added the indicator is turned pink (Chemguide.co.uk‚ Feb.12). The objective was to titrate a solution of Citric acid and Phenolphthalein‚ with a base‚ (NaOH)
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Observe & add 1 drop of hydrochloric acid. 6. Potassium iodide + Lead Nitrate. A precipitate should form. 7. Sodium hydroxide + phenolphthalein. a. Phenolphthalein is an acid-base indicator. 8. Hydrochloric acid + phenolphthalein. a. What color would be expected when combining phenolphthalein with an acid or with a base? 9. Sodium bicarbonate + Silver nitrate 10. Silver nitrate + Ammonia a. Using a paper towel‚ absorb the mixture onto a paper towel and hold in front of a strong light bulb
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concentration. HC2H3O2 (aq) + NaOH (aq) H2O (l) + NaC2H3O2 (aq) The above equation is used to neutralize the acetic acid. The acid reacts with a base to produce water and a salt. Because there’s a 1:1 ratio‚ the moles of the acid must equal the moles of the base in order to reach the equivalence point. As far as the indicators go‚ an acid-base indicator will be used to show when we are close to the end point. For example‚ when HIn is dissociated In - is produced and it is pink. (See equation
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Title Laboratory Techniques and Measurements Purpose The purpose of this experiment is to determine mass‚ length‚ temperature‚ volume‚ and density of objects and liquids using common measuring devices and algebraic formulas. The metric system‚ the most common set of measurements used in science‚ which includes meters‚ liters‚ Celsius‚ and grams will be used. Procedure The following items were used within the experiment: (1) Metric ruler with centimeter (cm) and millimeter (mm)‚ (1)
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results in a yellowish tint. This means the byproduct of the two is a base. C NH 3 and BTB When two drops of Ammonia and one drop of Bromothymal blue are combined the result remains blue. This means they are base. D HCI and blue dye When Hydrochloric acid and blue dye are combined the result is a base. E Blue dye and NaOCI When Blue dye and Sodium Hypochlorite react are combined the result is green. This means it is a base. F NaOCI and KI When Sodium Hypochlorite and Potassium Iodide
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experiment 7) Repeat the entire process using a new 100 drops of milk and ammonia this time Liquid Wide Range pH Narrow Range pH Water Lemon Juice Milk Ammonia Analysis: In this lab‚ one observed that acids and bases affect the pH of milk differently from one another. For example‚ the lemon juice gave the milk a lower pH because of the acidity of the lemon juice. That’s why the milk curdled. Another example‚ when ammonia was added to milk in part II of the lab
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Leader’s Book Notes - Boots June 20‚ 2008 By SMA Kenneth Preston Leaders Book Note - Boots Leaders‚ In this edition of my leader book notes I would like to inform leaders of the authorized and unauthorized Commercial-Of-The-Shelf (COTS) and Army issued boots for wear with the ACUs. There has been misunderstanding with the ALARACT Message 140/2007 with leaders in interpreting which COTS boots are authorized and which are not. My intent is to add clarity to the ALARACT message giving
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occurs. Increasing the concentration of the buffer can increase the buffer capacity of a solution. At the half equivalence point‚ the moles of base added to the acid is equivalent to half the moles of acid originally present. Thus‚ the amount of the weak acid and its conjugate base are equal. According to the Henderson-Hasselbach equation‚ when [Conjugate Base]/[Acid] is equal to 1‚ then
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