listing the reduction potentials of a series of metal ions in order of ease of reduction. The series of half-cells is constructed by placing a piece of metal into a 1.0 M solution of its ions for each metal in the series. The metals are Cu‚ Fe‚ Pb‚ Mg‚ Ag‚ and Zn. The half-cells are connected by a salt bridge constructed of a strip of filter paper soaked in a solution of KNO3. The zinc half-cell is used as the reference standard and assigned an E of 0 volts‚ and all reduction potentials are measured
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ACIDS‚ BASES AND SALTS 1. What are indicators? What are the different types of indicators? An indicator is a dye which changes colour when put into an acid or a base. The different kinds of indicators are- Natural indicators- Litmus is a natural indicator‚ litmus solution is a purple dye which is extracted from a plant called lichen. Litmus turns red in acidic solutions and blue in basic solutions. Other
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equilibrium reaction Cu(OH)2(s) ⇌ Cu2+(aq) + 2OH-(aq). 0.10 M Cu(NO3)2 and 0.10 M NaOH were reacted together in seven test tubes to form the solid Cu(OH)2‚ a blue precipitate. Distilled water was added to the first test tube. This served as the control. When 6.0 M H2C2O4 was added to the second test tube‚ the precipitate turned cloudy blue. The new equilibrium can be attributed to the formation of the solid CuC2H4 which is cloudy blue in color‚ and the ionization of H2C2O4. The addition of Zn dust in the
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activity of the metal pairs used with Cu to make a voltaic cell‚ on the voltage of the cell when room temperature‚ 18.0 ℃‚ room pressure‚ 1068 hPa‚ molarity and volume of electrolytes used‚ 1M – 50 mL‚ surface area of electrodes‚ 6cm x 3cm and type of salt bridge‚ KOH‚ is kept constant in each trial? Aim: The aim of this investigation is to determine the effect of activity of metal pairs by changing the electrodes used on a half cell and keeping the other constant‚ Cu‚ under same
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ions in a solution can be found by reaction with an excess of aqueous iodide ions to produce iodine. The amount of iodine formed can be found by titration with thiosulfate ions‚ S2O32–. For Examiner’s Use FB 1 is aqueous copper(II) sulfate‚ CuSO4. FB 2 is 0.100 mol dm–3 sodium thiosulfate‚ Na2S2O3. FB 3 is aqueous potassium iodide‚ KI. starch indicator Read through the instructions carefully before starting any practical work.
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dry tube. Add a piece of copper metal into this solution. Add 5ml of 0.1 M solution. Record your observations 2. Add 5ml of 0.1 M Cu(No3)2 to each tube. Place of strip of Zn and Pb in each tube. Record your observations 3. Repeat step 2 using 0.1 M Pb(NO3)2 and strips of Cu and Zn. Record your observations 4. Repeat the step again using 0.1 M Zn(NO3)2 and strips of Cu and Pb. Reaction of
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NaOH(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(OH)(s) Observations: The solution turned slightly cloudy. Reaction #6A: Na2SO4(aq) + BaCl2(aq) Na2Cl2(l) + BaSO4(s) Observations: The solution turned white and cloudy. Reaction #7A: Na2SO4(aq) + Cu(NO3)2(aq) CuSO4(aq) + 2NaNO3(aq) Observations: The solution was slightly tinted blue due to the copper‚ but it
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strip‚ nothing happened. Adding the Cu strip did not affect the solution or the strip. (Strip stayed orange. The solution was still clear.) When we added the‚ nothing happened. The solution stayed clear and the strip stayed grey. When we added the Ag strip‚ nothing happened. The strip remained light grey and the solution was clear. Zn(NO3)2 aq When we added the Mg strip‚ the strip became dark grey (opposed to the regular grey before) Adding the Cu strip did not affect the solution or
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ELECTROPLATING Electroplating is the application of electrolytic cells in which a thin layer of metal is deposited onto an electrically conductive surface. Electroplating is a plating process that uses electrical current to reduce cat ions of a desired material from a solution and coat a conductive object with a thin layer of the material‚ such as a metal. Electroplating is primarily used for depositing a layer of material to bestow a desired property (e.g.‚ abrasion and wear resistance‚ corrosion
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like small flakes of silver Turned bright red and obviously to a very high temp. Turned bright red and gave off gas Zn Much bigger and sturdier than magnesium‚ although very similar in look (besides size). Completely melted and then solidified into a new form. Continued to melt CuCO3 Green powder Turned dark black instantly as if it was completely burning Again turned dark black Cu(NO3)2 Looked like aqua and navy blue glitter mixed together Fizzled and looked like it was turning into a gaseous solution
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