The coefficient in a chemical formula indicates how many molecules of the formula unit‚ or chemical compound. The chemical formulas we use in this experiment are NaCl (sodium chloride/salt)‚ KCl (potassium chloride)‚ and CsCl (cesium chloride) and CaCl2 (calcium chloride). To form
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Analysis of Soda Ash and Carbonate-Bicarbonate Mixture Submitted: February 27‚ 2013 Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas España‚ Manila Abstract A standard acid solution like HCl can be used as titrant for the analysis of both soda ash and a carbonate-bicarbonate mixture. In the analysis of soda ash‚ the volume needed to neutralize the soda ash is used to compute for its alkalinity‚ in this experiment we obtained a 17.6 % alkalinity with an error
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reached‚ and as a result the volume of the HCl needed for the endpoint to be reached could be used in determining the moles and in turn the molar solubility and the solubility constant of the Ca(OH)2. For the second part of the experiment a common ion (CaCl2) was added to the calcium hydroxide and the process was repeated to analyze how the common ion would affect the molar solubility of the calcium hydroxide solution. The purpose of this experiment was to resolve for calcium hydroxide’s molar solubility
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shows the properties and reactions belonging to group IA‚ IIA‚ and IVA. Proper procedures and observations were done to determine the solubility‚ physical state‚ color‚ and appearance of the compounds namely Li2CO3‚ Na2CO3‚ K2CO3‚ CaCO3‚ and BaCO3. The results shows that Li2CO3‚ Na2CO3‚ K2CO3 were soluble in water‚ while MgCO3‚ CaCO3‚and BaCO3 were not soluble. All of these compounds were color white‚ they are in solid form‚ and their appearance were powder like. The sample from Group IVA Elements
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Experiment 7 Investigating Stoichiometry with Sodium Salts of Carbonic Acid Introduction: The student will perform the experiment in order to find the percent yield by using the theoretical value found using the balanced equation for sodium carbonate as well as sodium bicarbonate. The objective is to stabilize the substances by titrations and finding the percent yield when all the data is collected. The purpose of this procedure is so that the student will get better understanding of stoichiometry
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Isolation of Eugenol from Cloves Abstract The experiment conducted‚ isolation of eugenol from cloves‚ is the extraction of the essential oil. To perform this experiment cloves and water were mixed together and heated by a heating mantle in a round-bottom flask. A direct stem distillation took place‚ and the oil product was out aside for a week. After one week‚ the isolation of the eugenol actually takes place. Next the thin-layer chromatographic analysis takes place‚ but the experiment
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Turned green Red cabbage + CH3COOH Change to clear Turned pink NaHCO3 + NH3 Will mix Backing soda separated to the bottom NaHCO3 + CH3COOH Will create bubbles Bubbled over Na2CO3 + CH3COOH Bubble Small fizz‚ clouded the mixture MgSO4 + CH3COOH Fizz Nothing MgSO4 + NH3 Mix NH3 turned the MgSO4 white MgSO4 + Na2CO3 Fizz or cloud The two combined and thickened B. Follow-Up Questions 1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give
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Experiment No. ___________________ Date ___________________ NEUTRALIZATION TITRATIONS INTRODUCTION The neutralization of hydronium or hydroxide ion to form water is widely used as the basis for volumetric determinations of acids‚ bases and salts of weak acids. The reaction is characterized by a rapid change in pH near the equivalence point‚ a change that is readily detected by an acid-base indicator or that can be followed electrically by use of a pH meter. Neutralization titrations
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that I found the name of. H2SO4 is a strong base‚ and a PH test revealed that it had a very low PH of 1. Also already knowing that solution 6 was NaHCO3 and solution 8 was Na2CO3‚ I was also able to confirm solution 2 was NaOH by the following reactions: H2SO4(aq) + 2 NaHCO3(aq) ⇒ Na2SO4(aq) + 2 CO2(g) + 2 H2O(l) H2SO4(aq) + Na2CO3(aq) ⇒ Na2SO4(aq) + CO2(g) + H2O(l) These reactions show that the fizzing that occurred while performing precipitate reactions was the release of CO2 gas. All findings lead
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given off to leave a white powder. The aim is to find the equations for this reaction. Hypothesis: The experiment will prove which of the equations below is true. It will tell us whether Sodium Carbonate is produced or Sodium Oxide. 2NaHCO3 Na2CO3 + CO2 + H2O 2NaHCO3 Na2O + 2CO2 + H2O Variables: Independent: Original Mass of NaHCO3 Dependant: Final Mass of the Residue Controlled: Mass lost Apparatus: Method: First we measured and recorded the weight of
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