forms when sodium benzoate is placed in a simulated stomach acid. Theory Benzoic acid can be found in a wide variety of plants. It is used as a natural preservative in many foods. Sodium benzoate‚ the salt of benzoic acid‚ has become a more popular choice as a food preservative because it is more soluble in water than benzoic acid. Many food items found today are preserved with sodium benzoate. Reaction Reaction: sodium benzoate + hydrochloric acid benzoic acid + sodium chloride Amounts:
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Calcium Chloride Grainy‚ White Sodium Bicarbonate White‚ flour texture Phenol Red Solution The color of Hawaiian punch‚ thin consistency‚ semi- transparent What happens when the substances are mixed together? Observations Calcium Chloride- Foams and heats up when mixed with the phenol red. Turned orange Sodium Bicarbonate- Turned orange‚ dissolved What individual interactions are responsible for the observed changes? Questions How come the sodium bicarbonate dissolved? Why did
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were told that sodium hydrogencarbonate decomposes on heating to give sodium carbonate‚ water and carbon dioxide as shown in the equation below:- 2NaHCO3(s)--------> Na2CO3 (s) + H2O (l) + CO2 (g) = DeltaH1 This was given as deltaH1 and we had to calculate as part of the experiment. This however cannot be measured directly‚ but can be found using the enthalpy changes from two other reactions. These being that of sodium hydrogencarbonate and hydrochloric acid and also sodium carbonate and hydrochloric
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Alkali Metals Introduction Alkali metals refer to six elements belonging to the Group IA of the long form of the Modern Periodic Table‚ viz. Lithium (Li)‚ Sodium (Na)‚ Potassium (K)‚ Rubidium (Rb)‚ Cesium (Cs) and Francium (Fr). Fr is a radioactive element. These elements are called so because they form strongly alkaline oxides and hydroxides. Electronic Configuration of Alkali Metals Each of the alkali metals has one electron in their outermost (valence) shell‚ which is just outside an inert
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following functions: 1. Plays a major role in regulating blood volume because it controls the amount of water to be excreted and the amount of water to be reabsorbed. 2. Regulates electrolytes in the blood by controlling the secretion and reabsorption of sodium and potassium ions. 3. Regulates the pH of the blood by controlling the secretion and reabsorption of hydrogen ions. When more hydrogen ions are excreted from the blood‚ it renders the blood less acidic (more alkaline). But if more hydrogen ions are
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conditions of bleach’s stored at different temperatures. Introduction: Chlorine bleaches are made by dissolving chlorine in sodium hydroxide solution. They have a number of uses as they are used to remove colors‚ whiten or disinfectant via oxidation. Many bleaches have strong bactericidal properties‚ and are used for disinfecting and sterilizing as they contain chlorate ions. Sodium Thiosulphate is used in the pH testing of bleach substances as it neutralizes the color-removing effect of the bleach and
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tumor had disappeared and showed no scar tissue. Emily was scheduled to undergo one more chemotherapy session on February 26th to rid of any last traces her tumor may have left behind. (Jerry‚ C.) At 4:30 P.M.‚ a nurse administered a solution of sodium chloride through her IV while Emily was napping. She was awoken feeling very tired and weak struggling to sit up. She was holding her head complaining of pain. She became suddenly thirsty and within minutes‚ she was
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Purpose: The purpose of the practical that we completed was to determine the molar mass of carbon dioxide (CO2) by experimental means and to observe the reaction of hydrochloric acid and sodium carbonate. Using the balanced equation: Na2CO3 + 2HCl → 2NaCl + H2O + CO2 Materials / Apparatus: 1) 8.00g of sodium carbonate‚ 2) 30mL of hydrochloric acid (6molL-1) 3) 100mL of hydrochloric acid (6molL-1) 4) 100mL conical flask‚ 5) 150mL glass beaker 6) 50mL glass beaker 7) Glass funnel‚ 8) Digital scales
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BUFFER SOLUTION (ACID) An acidic buffer solution is simply one which has a pH less than 7. Acidic buffer solutions are commonly made from a weak acid and one of its salts - often a sodium salt. Objectives: 1. Measure the pH of the unknown solution first with indicators and then with pH paper. 2. compare the buffer solution with both a strong acid and a weak acid materials: 2 30 mL beakers 2 100mL volumetric flask 1 10mL pipet 2 aspirator 1 50mL graduated cylinder 1 10mL graduated
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hydrate sodium thiosulfate. The experiment’s purpose was to observe the reaction of the hydrate sodium thiosulfate in different situations‚ such as being shook over a period of time‚ or place another hydrate sodium thiosulfate pellet in its liquid form. This allows the students to observe the process of crystallization. Throughout the experiment‚ the students are asked to melt the hydrate sodium thiosulfate into liquid form‚ having no definite shape but a definite volume. Hydrate sodium thiosulfate
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