end point of the reaction by change of colour. For example phenolphthalein and methyl orange are indicators used in acid alkali titrations. Potassium permanganate itself acts as an indicator in potassium permanganate titrations. Acidimetry and Alkalimetry Titration: Acidimentry refers to the titration of alkali with a standard acid and alkalimetry refers to the titration of an acid with a standard alkali. 123 Permanganimetry Titration: The titration involving KMnO4 is called permanganimetry
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cm3 of a solution of hydrochloric acid. What is the molarity of the acid? 2. 25.0 cm3 of a 0.10 moldm-3 solution of sodium hydroxide was titrated against a solution of hydrochloric acid of unknown concentration. 27.3 cm3 of the acid was required. What was the concentration of the acid? 3. 10 cm3 of a solution of NaCl react with 15 cm3 of a 0.02 moldm-3 solution of AgNO3. What is the concentration of the NaCl solution in gdm-3? 4. 25 cm3 of a 0.1 moldm-3 solution of an acid HxA reacts with 75 cm3
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Calcium Hydroxide Titrated with Hydrochloric Acid By: Juliana Kadiasi Signature__________________________________________ (Experimental team: Ashley Tsao‚ Sophie Alvarez‚ Catherine Hering) IB Chemistry HL B3 For: Mr. Ahmed. Belmir 15 September 2014 Criteria Aspect IA IA Total Design 1. Identified Problem & relevant variables 2. Procedure controls variables 3. Procedure & relevant sufficient data Data Collection & Processing 1. Precise & accurate
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Magnesium Iron Copper 1M hydrochloric acid‚ HCl 1M sulphuric acid‚ H2SO4 1M acetic acid‚ HC2H3O2 1M phosphoric acid‚ H3PO4 Procedure: Please refer to Health Chemistry‚ Laboratory Experiments‚ page(s) 75-76. Data and Observations: Table 1: Comparison of Metal Activities Zinc Magnesium Copper Iron Hydrochloric acid Small bubbles Many bubbles N.R. color change (black) Sulfuric acid Small bubbles Many bubbles N.R. N.R. Phosphoric acid Small bubbles Few Bubbles
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zinc‚ an element‚ and hydrochloric acid‚ a compound‚ but combining a compound and an element is not synthesis‚ it is single replacement. We are taking zinc and hydrochloric acid and making zinc chloride and hydrogen‚ a single replacement‚ but what occurred during that replacement? The lab starts with a given amount of zinc and 10 milliliters of hydrochloric acid being placed in a test tube surrounded by cold water. The zinc then replaces the hydrogen in the hydrochloric acid‚ leaving the excess hydrogen
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accepted heat of reaction for the neutralization of hydrochloric acid with sodium hydroxide is −56.0 kilojoules per mole‚ determine the percent error of the experimental value that you calculated in Part II. Show your work. (experimental - actual value) / actual value × 100 % 4. Using the accepted values of the processes you’ve examined‚ would your estimation of the enthalpy change for the reaction of solid sodium hydroxide in aqueous hydrochloric acid change from the prediction you made in question
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eLearning 2009 Publication No. 91860 Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid Rate Laws Introduction The purpose of this demonstration is to investigate the effect of sodium thiosulfate concentration on the rate of reaction of sodium thiosulfate with hydrochloric acid. The reaction‚ which produces solid sulfur‚ will be followed by measuring the time needed for the reaction mixture to become opaque. The results will be analyzed graphically to determine the order of
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Butanol Purpose: To test the reactions of primary‚ secondary‚ and tertiary alcohols with acid and with an oxidizing agent. Equipment and Materials: Chemical safety goggles Lab apron Protective gloves 3 test tubes Test-tube rack Eyedropper Dropper bottles containing the following Butan-1-ol Butan-2-ol 2-methylpropan-2-ol Potassium permanganate solution‚ KMnO4(aq) (0.01 mol/L) Concentrated hydrochloric acid‚ HCl(aq) (12 mol/L) *Alcohols are flammable and should be kept away for heat sources
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THE MOLE CONCEPT References : Mohammed and Lambert ( Old Edition) Chapter 11 pg. 107 Mohammed and Lambert ( New edition) Chapter 8 pg 123 Anne Tindale Chapter 10 pg 46 The following topics will be covered : 1. Definition of Relative Atomic and Relative Molecular Masses. 2. Calculation of Relative Molecular Masses 3. Converting Moles to Grams / Grams to Moles 4. Calculation from equations Masses of substances /Volumes of gases / Concentration
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Hot water 7. Room temperature water 8. 1M hydrochloric acid (HCl) 9. 3 M HCl 10. Iron (III) chloride (FeCl3) 11. Sodium chloride (NaCl) 12. Calcium chloride (CaCl2 ) 13. Potassium nitrate (KNO3) 14. 0.3% hydrogen peroxide (H2O2) solution 15. 8 test tubes 16. Test tube rack 17. 3 250mL beakers 18. Alka Seltzer tablet 19. 3 pieces of zinc metal Procedure: Particle size 1. Have two test tubes in the test tube rack. Put 1M hydrochloric acid into both of these test tubes. 2. Take a scoop
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