ions of SO42-‚ CO32-‚ Cl-‚ and I-‚identify them separately‚ and use the observation to identify the unknown. Procedure Part I - Qualitative Analysis of Group 2 Elements Mix 0.02M K2CrO4 with each Mg(NO3)2‚ Ca(NO3)2‚ Sr(NO3)2 and Ba(NO3)2 together. Secondly‚ mix 0.1M (NH4)2C2O4 instead of 0.02M K2CrO4 together with the same reactants used before. Thirdly‚ mix 0.1M Na2SO4 with those reactants. Then‚ mix 0.1M NaOH with the same reactants used before again. Some precipitates should forms
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Determination of the mole ratio of a chemical reaction The method of continuous variations is a means of determining the stoichiometric mole ratio of the reactants in a chemical reaction. The stoichiometric ratio‚ as given by the coefficients in the balanced chemical equation‚ represents the ratio at which chemicals must be combined to produce all product with no excess reactant. Since there is no “wasted” reactant‚ the maximum amount of product is made for the given amount of both reactants
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(Ksp for Ag2CrO4 is 910-12 ) Procedure: A. Standardization of 0.1 M AgNO3 solution 0.2500 g portions of NaCl was weighed into Erlenmeyer flasks and about 100 mL of distilled water was dissolved in. Small quantities of NaHCO3 was added in order to adjust the pH of the solutions until effervescence ceased. About 2 mL of K2Cr04 was added and the solution was titrated with 0.1 M AgNO3 solution to the first permanent appearance of red Ag2Cr2O4. B. Determination of Cl- in solid
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Ammonium sulphate (NH4)2SO4. FW = 132.14‚ Eq. = 66g/l. 250ml 0.05M = 1.325g = 0.1N | Adipic acid HO2C(CH2)4CO2H‚ FW = 146.4‚ Eq. = 73.03g/l 250ml 0.05M = 1.83g = 0.1N | Barium hydroxide Ba(OH)2.8H2O‚ FW = 315.48‚ Eq. = 157.5g/l 250ml 0.05M = 3.94g = 0.1N | Benzoic acid C6H5COOH‚ FW = 122.12‚ Eq. = 61g/l 250ml 0.05M = 1.52g = 0.1N | Calcium carbonate CaCO3‚ FW = 100.00‚ Eq. = 50g/l 250ml 0.05M = 1.25g = 0.1N | Furroic acid FW = 112.08‚ Eq. = 112g/l 250ml 0.1M = 2.8g = 0.1N |
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------------------------------------------------- ------------------------------------------------- RESULTS AND DISCUSSION A. Iron-Silver Equilibrium In studying equilibrium between iron and silver‚ 0.10 M FeSO4 and 0.10 M AgNO3 were used. The balanced equation for the reaction is: FeSO4 (aq) + 2 AgNO3 (aq) ↔ Fe(NO3)2 (aq) + Ag2SO4 (s) It has a net equation of: Fe2+(aq) + Ag+(aq) ↔ Fe3+(aq) + Ag(s) This part of the experiment required centrifugation of the solution
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quadrat 8. Transect line 9. Plastic bags and vials 10. Compass 11. Drinks or distilled water 12. pH papers 13. A light string 14. Hydrometer instrument for measuring salinity 15. Long ruler 16. Long plastic water pipe 17. Deionized water 18. K2CrO4 solution 19. AgNO3 solution‚ 0.05M BRIEF INTRODUCTION OF ROCKY SHORE HABITAT Rocky Shores are the regions with strong waves all the time which erode the rocks surface and thus leave the rocks exposed. Due to the different period of submergence along the
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Name: Charity Flosser Date: 12.17.2012 Unit: Lesson: Unit 4 Lesson 11 Classifying Reactions Objectives: Identify the four most common types of reactions: synthesis‚ decomposition‚ single replacement‚ double replacement Predict the products of reactions Balance chemical equations Part I: Reaction between zinc and iodine Watch the Video. http://www.youtube.com/watch?v=xT9V7Y1iKYc Observations: Describe what happened when the water was added. A reaction
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solutions for you to investigate. (Note Table 1 on the Data Sheet.) Some of these combinations will produce precipitates; others will not. Step-by-step instructions for experimenting with the first combination (AgNO3 and NaCl) are listed below. For the first solution‚ select AgNO3. For the second solution‚ select NaCl. The Erlenmeyer flasks that appear are filled with the two aqueous solutions. Note the color of each solution. This information has already been recorded for you in Table
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solution containing chloride ions: Ag+(aq) + Cl-(aq) -> AgCl(s) By adding silver ions until silver chloride is no longer precipitated‚ the amount of chloride in a solution can be found. Potassium chromate (VI)‚ K2CrO4‚ can be used to indicate the end-point of the titration‚ the point at which all chloride ions have been precipitated. Silver ions combine with chromate (VI) ions to form a red precipitate of silver chromate (VI): 2Ag+(aq) + CrO2-4(aq)
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C2O42(oxalate): Salt + conc H2SO4 1. No reaction: Group II anion not present. Continue to group III. 2. Chloride: Colourless white pungent fumes (HCl); intensify when glass rod dipped in NH4OH is brought near mouth of test tube 1. Silver nitrate test: WE + AgNO3 = white ppt soluble in NH4OH 2. Chromyl chloride test: Salt + solid K2Cr2O7 + 2-3 drops conc H2SO4 = orange / red fumes of chromyl chloride 6 1. Vapours + NaOH (aq) = yellow solution 2. Yellow solution + acetic acid + lead acetate sol = yellow ppt
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