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The crude copper that is subjected to electrorefining contains tellurium as an impurity. The standard reduction potential between tellurium and its lowest common oxidation state, Te^4+, is Te^4+(aq)+4e-=> Te(s) E°red= 0.57V
Given this information, describe the probable fate of tellurium impurities during electrorefining.
A student makes 215 mL of a 3.15M solution of Na2SO4. he then forgets to seal it and some water evaporates overnight. When he comes back int he morning, the volume of the solution is only 205 mL. What is the molarity of the solution after the wate..
The molar enthalpy of fusion of solid silicon is 46.4 kJ mol-1, and the molar entropy of fusion is 27.6 J K-1 mol-1.
The freezing point of t-butanol is 25.50°C and Kf is 9.1°C·kg/mol. Usually t-butanol absorbs water on exposure to air. If the freezing point of a 12.0 g sample of t-butanol is 24.59°C, how many grams of water are present in the sample?
The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O2 from the air is 2.67 × 10-4 M at sea level and 25°C.
write a net ionic equation for the reaction of each antacid with aqueous HCl. include the state of each species. a)MgCO3 b)CaCO3 c)Mg(OH)2
ampere current have to be applied to plate out 8.00 grams of copper metal from te aqueous copper(II) sulfate solution?
What volume of 0.200M Iron(II)sulfate solution would be required to react with 20.0mml of 0.250M potassium permangante(in sulfuric acid solution)?
Pour the water into a 24.0 gram beaker and boil off all the water, so only the salt remains. The beaker with salt in it weighs 41.0 grams. What is the % of salt and % of water
The standard (1 bar) boiling point of acetone is 56.1 C, and its enthalpy of vaporization is 29.1 kJ/mol. Calculate the vapor pressure of acetone at 55.1 C.
Using the Henderson-Hasselbalch equation determine the pKa for illinic acid from the following values: At pH 9.02, the concentration of illinic acid and its conjugate base
A solution is initially 0.050M in acetate, CH3COO- (Kb = 5.6 x 10^-10). 10.0mL of 0.10 M HCl is added. The Ka for the conjugate weak acid of CH3CHOO- is 1.8 x 10^-5. Calculate the pH for this solution at equilibrium.
How would the observed molarity of your experiment be affected by the following circumstances. (i.e. would it be higher than the true value, lwer than the ture vaule or remain unchaged?)
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