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A common way of removing Cr3+ from solution is by precipitation of Cr(OH)3(s). An environmental engineer tells you that adjusting the pH to 8.5 will decrease total soluble Cr(III) to below 1 mg/L (1.92 x 10-5 M). Is this true? In other words, is the solubility of Cr(III) in the presence of Cr(OH)3(s) at a pH of 8.5 ? 1 mg/L. The pKsp of Cr(OH)3(s) is 30.22. Cr3+ forms 4 complexes with hydroxide: log K1 = 10.00, log K2 = 8.38, log K3 = 6.87, log K4 = 2.98. Assume no other solids or ligands are present.
Calculate the theoretical yield of aspirin to be obtained, starting with 2.0 g of salicylic acid. 2. If 1.8 g of aspirin were obtained in this experiment, what would be the percent yield?
10.08g of potassium chlorate, KClO3 is heated to decomposition according to the following equation. How many grams of O2 gas will be produced?
Calculating the concentration of the acetate ion when dissociation of acetic acid occurs in water and over varying pH conditions? I am a process engineer in wood pulping operation in which we use steam to digest hardwood chips. This is non-chemica..
A total charge of 96.5 kC is passed through an elctrolytic cell. What mass of silver metal will be produced from a silver nitrate solution?
Complete and balance the equation for this reaction in acidic solution. Phases are optional
How much energy in kJ must be absorbed to heat up a volume of ocean water 2 m high by 20 km wide by 30 km deep by 3°C.
A solution is made up by dissolving 73 g of glucose in 966 g of water. Calculate the activity coefficient of glucose in this solution if the solution freezes at -.66 degrees C.
A solution is made by mixing 12.0g of NaOH and 70.0mL of 0.200m HNO3. Calculate the concentration of OH- ion remaining in the solution.
its ground state absorbs 2.50 times as much energy as the minimum required for it to escape from the atom. Calculate the deBroglie wavelength of the emitted electron
a 97 gram solution of silver nitrate contains 21 grams of AgNO3. what is the percent by mass of silver nitrate in this solution?
how much of this chemical would have been measured? Express in terms of measured concentration C (mg/litre) of the filtered sample?
Balanced thermochemical equation and enthalpy diagram, The decomposition of zinc carbonate, ZnCO3(s), into zinc oxide, ZnO(s), and CO2(g) at a constant pressure requires the addition of 71.5kJ of heat per mole of ZnCO3.
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