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The magnesium and calcium ions present in seawater([Mg2+] = 0.059 M and [Ca2+] = 0.011 M) can be separated by selective precipitation with KOH. What is the concentration of [Mg2+] when Ca(OH)2 starts to precipitate?
A gas mixture being used to simulate the atmosphere of another planet consists of 324 mg of methane, 217 mg of argon, and 228 mg of nitrogen.
A sample of gas originally at 37.2oC and 1.25 atm pressure in a 3.4 L container is allowed to expand until the pressure is 0.73 atm and the temperature is 14.9oC.
Consider the following reaction: SO2Cl2 (g) SO2 (g) + Cl2 (g). K = 2.99*10^-7 at 227 degrees celsius. If a reaction mixture initially contains 0.159 , what is the equilibrium concentration.
Prepare the molecular formula for given compounds and determine the amount of molecules present and write the molecular formula and determine how many grams of each you have
For the concentration of hydroxyl radical of 7.5E06 molecules/cm3 and a carbon monoxide concentration of 18 ppm, calculate the rate of its reaction with atmospheric carbon monoxide at 11 degrees C.
500cm3 of 0.250M of Na2SO4 is added to an aqueous solution of 15.0g of BaCl2 resulting in a white precipitate of insoluble BaSO4.
What is the volume occupied by 25.0 gm of Ar (g) at a temperature of 301K and pressure of 1.30atm.
An unknown mass of each of the given substances as with The final temperature is recorded as indicated 1.Pyrex glass (tf=67.6 C), 2.Sand (tf=70.4 C), 3.ethanol (tf=45.9 C), initially at 19.0 degrees celsius, absorbs 1930 Joules of heat
You have prepared a saturated solution of at 20 degree celcius using 31.0 of water. How much more solute can be dissolved if the temperature is increased to 30 degree celcius.
If 30mL of 6.8M H2SO4 was spilled , what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid.
If the actual yield is 220.0 g and the theoretical yield is 275.6 g then what will be the percent yield of ferrous sulfide.
What is the percentage protonation of the solute and Calculate the pH of the solute in an aqueous solution of 0.611 M Aqueous solution of Ammonia
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