The effect on the pH of Distilled water‚ Potato Solution and Commercial Buffer‚ when Hydrochloric acid (0.1 mol/L) and Sodium Hydroxide (0.1 mol/L) is added Mahima Mandava Mrs. Haist September 23rd‚ 2014 SBI4U1 Background Information: The pH is the measurement of how acidic or how basic a substance can be. The pH scale is used to measure how acidic or basic a living cell can be. The pH scale ranges from 0-14; 0-6 being acidic‚ 8-14 being basic and 7 being neutral. There are many factors
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of H+ ions which means that pH of the solution is raised. Thus‚ a 0.1 M acetic acid solution has a pH of 2.87 but a solution of 0.1 M acetic acid and 0.1 M sodium acetate has a pH of 4.74. Thus 4.74 is the pH of the buffer. On addition of 0.01 mole NaOH the pH changes from 4.74 to 4.83‚ while on the addition of 0.01 mole HCl the pH changes from 4.74 to 4.66. Obviously the buffer solution maintains fairly constant pH and the changes in pH could be described as marginal. Buffer Action: A buffer
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This is the reaction for determining the excess of HCl: 2HCl (aq) + CaCO3(s) -→ Ca2+ (aq) + CO2(g) + H2O(l) + 2Cl- (aq) Materials: eggshell burette‚ 50 cm³‚ and stand pipette + filler‚ 20 cm³ plastic foil phenolphthalein indicator 0.1 M NaOH solution‚ M hydrochloric acid‚ Distilled water forceps safety eye wear 2 beakers‚ 100 cm3 volumetric flask‚ 250 cm3 filter funnel Mortar and pestle Method The shell of an egg must be removed and washed with soap to remove any organic
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Finally‚ in the third and fourth test tubes we added HCL and in the other NaOH and observed the effects. Data Tables and Observations: Data Table 1: Solubility or Reaction Mg Color: Silver‚ metallic Odor: None Effect of Heat: Color changed white Cold H2O: No effect‚ settled at bottom Hot H2O: No effect Litmus Red: Turned purple Litmus Blue: Turned purple Dilute HCL: Started smoking and fizzing Dilute NaOH: No effect Cu Color: Gold‚ copper‚ metallic Odor: None Effect of
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copper penny. Variables: There were no variables at this experiment PROCEDURES: Materials: Zinc (SN) filling‚ 3M NaOH solution‚ Copper penny‚ tongs‚ Hot plate‚ 100 ml beaker‚ 250 ml beaker‚ Bunsen burner‚ Water‚ Spoon. Procedure: First‚ we turned on the hot plate. Then‚ we filled 250 ml beaker with 125 ml of water. We put half a spoon of zinc fillings. We add 20 ml of 3M NaOH solutions in it. We placed the beaker on the hot plate‚ which we had turned on before. We put the penny into the
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Dagondon‚ Vanessa Olga Date of experiment: July 1‚ 2013 Nablo‚ Janica Mae Date of submission: July 18‚ 2013 Palmitos‚ Isabel Experiment # 2 chemical changes I. INTRODUCTION Chemical changes occur when a substance combines with another to form a new substance whether by combination reaction‚ combustion reaction‚ decomposition reaction and etc. These changes can be observed by evolutions of gas‚ appearance or disappearance of a precipitate‚ evolution or absorption of heat or even change
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composition of the following mixture by double indicator method: 1. NaOH(aq) and Na2CO3(aq) 2. NaHCO3(aq) and Na2CO3(aq) Introduction Consider a mixture of NaOH(aq) and Na2CO3(aq). Reaction between HCl(aq) and Na2CO3(aq) takes place in two stages: HCl(aq) + Na2CO3(aq) ⎯→ NaHCO3(aq) + H2O(l) …………………. (1) HCl(aq) + NaHCO3(aq) ⎯→ NaCl(aq) + CO2(g) + H2O(l) …………. (2) While that between HCl(aq) and NaOH(aq) completes in only one step: HCl(aq) + NaOH(aq) ⎯→ NaCl(aq) + H2O(l) ……………….………. (3) Solution mixture of
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was the dissolution of solid sodium hydroxide in water with a ΔH°rxn of -47047 J/mol‚ Reaction 2 was the neutralization of liquid sodium hydroxide with HCl with a ΔH°rxn of -31289 J/mol and Reaction 3 was the dissolution and neutralization of solid NaOH with HCl with a ΔH°rxn of -91000 J/mol. Consequently‚ the sum of Reaction 1 and Reaction 2 was -78336 J/mol‚ similar to the ΔH°rxn for Reaction 3. Table 2 displays the percent error of the experiment in comparison to the theoretical values‚ representing
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Aid with an NaOH solution. The reason titrations are used is to determine the concentration of an unknown solution by reacting a strong acid with a strong base. Titrations are hard to accomplish‚ though‚ due to the fact that indicators used to show the endpoints are very sensitive and one drop could make the solution titrate past its endpoint. Blue stock solution: 3 mg/L Yellow stock solution: 35 mg/L Phenolphthalein is the indicator used (6 drops per titration) Molarity of NaOH used: .05056
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using an acid burette. Then‚ the antacid was dissolved in the acid. After that‚ the two drops of phenolphthalein indicator were added and was mixed thoroughly. Lastly‚ the antacid mixture was titrated with 0.1 M NaOH the solution turned to a faint pink color. Recorded the final volume of NaOH used. Here‚ two trials were done. After the procedures‚ the weight of HCl that reacted with 1 gram of antacid tablet was calculated and found the result of 0.31 HCl per gram of antacid tablet. With the recovered
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