and dark has other things added to it C. Write a balanced equation for the neutralization of acetic acid with NaOH. CH3COOH + NAOH =.CH3COONA +H2O D. How would your results have differed if the tip of the burette was not filled with sodium hydroxide before the initial volume reading was recorded? You would think there was more NaOH than there actually was E. How would your results have differed if you had over-titrated‚ i.e. added NaOH beyond
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into solution. For example‚ hydrochloric acid (HCl) dissolves in water as follows: HCl | H2O | H+(aq) | + | Cl-(aq) | Arrhenius defined bases as substances that dissolve in water to release hydroxide ions (OH-) into solution. For example‚ a typical base according to the Arrhenius definition is sodium hydroxide (NaOH): NaOH | H2O | Na+(aq) | + | OH-(aq) | The Arrhenius definition of acids and bases explains a number of things. Arrhenius’s theory explains why all acids have similar properties
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“chlorine” after the Greek word “chloros” meaning “pale green”. Chlorine appears naturally in both the earth’s crust as well as in sea water. Though chlorine does not exist naturally as a gas‚ chlorine is obtained through a chemical reaction involving a sodium chloride and water mixture known as brine. When an electrical current is passed through the brine it reacts and breaks up the solution into chlorine‚ caustic soda and hydrogen gas. The reaction looks like this: 2NaCl + 2H2 ----- Cl2 + 2NaOH + H2.
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NO | ANSWER | MARK | 1 :( i )( ii ) ( iii ) ( iv )2 :( i )( ii )( iii )3 )4 )5 ) ( i )( ii )( iii )( iv )6 )7 ) i )ii ) iii )8 )9 )10 )i ) ii )iii)11 ) | A reagent is highly serves as a reference material in all volumetric & mass titrimetric method.A reagent solution of accurately known concentration. * End point-point at which the reaction is observed to be complete and there is permenant colour change at the end of titration. * Equivalent point-point at which an equivalent amount of
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4-26-13 This lab 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
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AP Chem Exam - ‘98 1. Solve the following problem related to the solubility equilibria of some metal hydroxides in aqueous solution. (a) The solubility of Cu(OH)2(s) is 1.72 x10–6 g/100. mL of solution at 25° C. (i) Write the balanced chemical equation for the dissociation of Cu(OH)2(s) in aqueous solution. Cu(OH)2 Cu 2+ + 2 OH – (ii) Calculate the solubility (in mol/L) of Cu(OH)2 at 25 °C. (1.72 x10–6 g/0.100 L)(1 mol/97.5 g) = 1.76 x10–7 mol/L (iii) Calculate
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The effect of size on the effectiveness of diffusion Aim: To use agar blocks infused with 0.1 Molar sodium hydroxide (NaOH) and phenolphthalein to investigate the relationship between shape and surface area: volume ratio on the effectiveness of diffusion. Hypothesis: That for a cube of agar‚ the time taken for complete colourisation due to diffusion of HCl is directly proportional to the cubes volume. Materials: |A block of agar (10cm x 5cm x 3cm) with 0.1M NaOH and |1x 250mL
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304 Kinetics of Alkaline Phosphatase Objective To study the kinetics of alkaline phosphatase. Procedure 1. Sodium carbonate - sodium bicarbonate buffer: Dissolve 20 ml of 0.2 M solution of sodium carbonate (2.12 gm in 100 ml distilled water) and 230 ml of 0.2 M sodium bicarbonate (4.12 gm in 250 ml distilled water) to make up the volume 250 ml with pH 9 -9.2 2. 5 N sodium hydroxide solution (10 gm in 50 ml distilled water) 3. Substrate stock solution: Dissolve 0.1 gm of p-nitrophynyl phosphate
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Experiment 2 Preparation of Primary Standard solutions and Standardizing Acid and Base solutions Objectives: The objective of this experiment is: 1- To prepare two primary standard solutions‚ KHP and Na2CO3 2- To standardize a sodium hydroxide solution using the prepared primary standard KHP. 3- To standardize a hydrochloric acid solution using the prepared primary standard Na2CO3. 4- To calculate the concentration of an unknown acid or base. Introduction A primary standard is a standard that
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Standardization of hydrochloric acid by sodium carbonate Concentrated hydrochloric acid is roughly 11 M. Pour out into a measuring cylinder about 2 cm3 of concentrated hydrochloric acid. Transfer it to a 250 cm3 flask and make up to the mark with water. Shake well. Put some pure sodium hydrogen carbonate or anhydrous sodium carbonate into an evaporating dish and heat gently over a low flame for about fifteen minutes‚ stirring continuously. Take care not to heat the mass too strongly or fusion
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