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If toluene(density 0.87) were used to extract ethylene bromohydrin (density 2.41) from an aqueous solution,
(a) could you be certain that the organic solution would form the upper layer?
(b) by what test could you identify the non-aqueous layer?
How many grams of glucose are in 100. rm mL of the final solution?
Write the reaction between ferric chloride and lime slurry that results in precipitation of Fe(OH)3. For a dosage of 40 mg/l FeCl3: What is the required stoichiometric addition of lime expressed as CaO?
A flask contains 0.180 mol of liquid bromine, Br_2. Determine the number of bromine molecules present in the flask.
Determine number of moles of oxygen molecules are in the cylinder and compute the mass of solid C 2 H 3 NaO 2 required mixing with 60.0mL of .125M C 2 H 4 O 2 to form a ph 4.20 buffer?
Concrete used in road construction is reinforced using steel bars in a grid, known collectively as "rebar." After many years, rebar will begin to corrode, and the concrete will weaken.
Synthesizing ethers via acid-catalyzed condensation reactions has limited usefulness. The conditions (sulfuric acid and heat) are also conducive to elimination products. Clarification of Organic Chemistry
0.2 M HCl is used to neutralize 20 mL of 0.35 M NaOH. a. How many moles of OH- are present?
calculating theoretical yield for this experiment. It is a dehydration synthesis where one mol of hydrated salt yields 3 mol hydrates and 1 mol of anhydrous salt.
how much energy is required to turn 500 g of ice at -15.0 celsius to liquid water at 55.0 celsius? specific heat (ice) = 2.10 J/g * C. Specific heat (water)= 4.18 J/g*C
Calculate the temperature change which will be caused by the following process: 0.640 moles of NH4Cl are dissolved in 1.00 L of water.
The temperature of Beaker X = 75°C and the temperature of Beaker Y = 50°C after Five minutes . determine the temperatures be after another 5 minutes have passed?
Assuming that the total pressure of the gases is 1.52 atm and that their mole ratio is 94 : 4.0 : 1.5 : 0.50, calculate the partial pressure (in atmospheres) of each gas.
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