CM1191 Experiment 1: Study of Solubility Equilibrium 1. Abstract The aim of this experiment is to determine the relationship between the solubility of potassium hydrogen tartrate (KHC4H4O6) and temperature. Titrate a known concentration of NaOH against a saturated solution of KHC4H4O6 at different temperatures to obtain the concentrations of KHC4H4O6‚ and hence the solubility product constant of KHC4H4O6 at various temperatures. It was found that the solubility product constant of KHC4H4O6
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Acid-Base Titrations February 21‚ 2013 Abstract: With the given volume measurement of KHP and NaOH‚ the students experimented to calculate the mass of unknown acid and its equivalence point using a method called titration and titration curve. The known volume of an acid solution would be titrated by slowly adding drops of solution into NaOH‚ and the volume of base needed to react with the acid is measured throughout. By using those data‚ the students are able to find what they
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hydroxide (NaOH) was determined by using a known amount of Potassium Hydrogen phthalate (KHP). The balanced chemical equation for the reaction is: KHC8H4O4(aq) + NaOH(aq) => H2O(l) + KNaC8H4O4(aq) (1) KHP was chosen as a good acid to standardize NaOH because it has high molecular weight and stable on drying. The standardized NaOH solution was then used to determined the percent composition of KHP in an unknown substance #47. Experimental Information Part 1: Standardization of NaOH NaOH solution
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The unknown acid for this experiment was #14. The experiment began with the preparation and standardization of NaOH solution. It was calculated that 2.00 grams of NaOH pellets were needed to prepare 0.5 L of 0.1 M NaOH solution. The solution was then standardized by conducting three titration trials. It was calculated that 0.7148 grams of KHP were necessary to neutralize 35 mL of the 0.1 M NaOH. Three samples of KHP were weighed approximating this number (Table 1). Each sample was mixed
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diprotic‚ or triprotic‚ and how to calculate the molarity of a soft drink. At the same time‚ other skills were practiced. Skills such as calculating molarity‚ molar mass and percent error were exercised. The molarity was calculated for part B‚ the standardization of sodium hydroxide. After all of the molarities were calculated‚ five of them were accepted and the average came out to be 0.0935‚ which was the number that would be used throughout the lab to help calculate the molar masses of the unknown acids
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strong acid and strong base solutions. The technique of titration is used to observe the acid content of the fluid in a car battery. 3. Procedure: Calculate the volume of 6.00 M NaoH that is needed to prepare 250mL of an approximately 0.100 M NaOH solution. Transfer the calculated volume of the 6.00 M NaOH solution to a volumetric flask using a graduated cylinder. Obtain a 25mL buret‚ and rinse and fill it with the prepared base solution. Make sure there are no air bubbles trap within the
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Overview • • • • after calibration of the pH electrode and determination of the flow rate for the automatic titration‚ a NaOH solution is standardized against HCl. a pH titration curve for acetic acid is obtained and its pKa is determined. an unknown sample of Lysol is analyzed for its HCl content using the standardized NaOH. an unknown sample of Liquid Plumr is analyzed for its NaOH and NaOCl content using HCl of known molarity. 7 Name ______________________________ Section _______ Date ____________________
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a strong base. The titrant reacts with and consumes the acid via a neutralization reaction. The point at which stoichiometric amounts of the acid and base have combined is the equivalence point. An example of this is shown in the equation: HCl(aq)+NaOH(aq)NaCl(aq)+H2O(l). The number of moles is given by knowing the exact concentration and volume added of the titrant. The latter‚ in turn‚ is related by stoichiometry to the number of moles of acid initially present in the unknown. To detect the equivalence
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concentration of acetic acid of vinegar‚ in terms of (m/m). Introduction Neutralization is a reaction of an acid with a bases to produce a salt and water. For example‚ the reaction of the strong acid HCl with the strong base NaOH produces the salt sodium chloride and water HCl(aq) NaOH(aq) ( NaCl(aq) H2O(l) Since the acid‚ base‚ and salt in this reaction are all strong electrolytes‚ the net ionic equation for this reaction is H(aq) OH-(aq) ( H2O(l) This same result occurs in the reaction of strong
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which a 4.2 mL concentrated HCl was added to a 500.0 mL of distilled water. It was stirred and transferred to an Arrhenius storage bottle. After preparing‚ it was then standardized in which the prepared solution was used as a titrant and a standard NaOH as the analyte. An indicator methyl orange was added by adding 3 drops to the analyte then it was titrated until the orange-colored
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