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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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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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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This left us with the silver and chlorine which yield us silver chloride which is a solid. We did note on our observation that we had a change in color and a solid precipitate. 3. Na2CO3(aq)+ HCl(aq) → NaCl(aq) + HCO3(aq) Na2CO3 + 2HCl → 2NaCl + H2O + CO2(aq) 2Na+ + CO32- + 2H+ + 2Cl- → 2Na+ + 2Cl- + H2O + CO2 CO32- + 2H+ → H2O(l) + CO2(g) With this reaction the carbonate and the diatomic hydrogen combined together to make the bubbling effect that
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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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When determining the molar mass‚ add the mass of 2 water molecules to the mass of the CaCl2. 2. From the balanced equation calculate the number of moles of Na2CO3 required to react completely with the CaCl2·2H2O and record in the table. (See lab‚ page 79 for example) Prepare a table. 3. Calculate the number of grams of Na2CO3 to weigh out from the number of moles in step 2. Prepare a table. 4. Calculate the number of grams of CaCO3 that are expected to be produced. This
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Hard Water Analysis Guided Inquiry Lab CaCl2 + Na2CO3 → CaCO3 + 2 Na + 2 Cl Purpose: Determine the amount of ions‚ specifically calicum‚ that are present in multiple samples of water by adding another chemical to create a reaction to percipitate the calcium out of the water into a measureable solid Materials: balance (.001g)‚ 100ml beakers‚ graduated cylinder‚ drying oven‚ Na2CO3 (sodium carbonate)‚ stir rod‚ scoopula‚ DI water‚ watch glasses‚ filter paper‚ ring stand‚ funnel‚ water samples with
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