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Calculate the number of moles of solute present in eahc other following solutions: a) 60.0g of an aqueous solution that is 1.25 percent KI by mass, b) 250g of an aqueous solution that is 0.460 percent NaCl by mass, c) 0.600L of 1.25M H2SO4.
How many moles of atoms are in each of the following? 4.1*10^24 Pb atoms ,2.15*10^22 He atoms
What is the volume of .885 M hydrochloric acid required to react with (a) 25 mL of .288 M aqueous ammonia (b) 10 g of sodium hydroxide (c) 25 mL of a solution
Concentration of Fe(SCN)2+ in calibration Solutions-Recall that the concentration of Fe(SCN)2+ in the calibration solutions is essentially the concentration of SCN- initially in the solution
What is the molar concentration of the solution? How many moles of solute are in the solution? What is the molar mass of the solute?
or the reaction H2(g)+CO2(g) H2O(g)+CO2(g) at 700C, Kc=.534. Calculate the number of moles of H2 that are present at equilibrium
A 250-L tank is evacuated and connected to a 50.0-L bulb filled with compressed argon. After they are joined, the pressure in the bulb falls to 2.20 atm.
If 0.80 g of sulfur dioxide at 10.00 atm pressure (P) dissolves in 5.00 L of water at 25.0°C, how much of it will dissolve in 1 L of water at 9.00 atm pressure (P) and the same temperature?
The mass of the isotope, I-129, is 128.905 amu while the atomic mass of the contaminated iodine sample is 127.1982 amu. What is the mass of the contaminant?
HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous water
How many double bonds are present in the "best" resonance structure of the phosphate ion?
Some solid remained in the beaker after stirring with HCl. You washed the filter paper with ketone, which caught on fire and the filter paper was scorched
In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 26.50 mL of 0.0502 M NaOH but overshoot the end point, and the solution turns deep pink.
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