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What is the "mass per volume" percent of a household bleach product? I believe the question is asking for a calculation but I do not know how to proceed
calculate the molarity (M) of the solution when water is added to prepare each of the following: a)25.0 mL of a 18.0 M HCl solution is diuted to 500 mL. b)50.0 mL of a 1.50 M NaCl solution is diluted to 125 mL. c)4.50 mL of a 8.50 M KOH solution i..
Make an energy level diagram, showing ALL suborbitals, large enough to accomodate the 1st 36 elements
The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is __________ kJ. The specific heats of ice, water, and steam are and respectively. For H2O, Hfus = 6.01 kJ/mol, and
What is the minimum flowrate (in m3 hr-1) needed to maintain a maximum CO concentration of 1 ppm in the room at steady-state? (b) What is the residence time of air in the room?
How many grams of lead may be formed by the passage of 65.5 amps for 1.07 hours through an electrolytic cell that contains an aqueous Pb(IV) salt.
what is the volume percent of a solution prepared by dissolving 43 g of NaOH in enough water to make a final volume of 120 ml.
water in a coffee-cup calorimeter (see above figure) the temperature rises from 24.00 oC to 40.03 oC. Calculate H in kJ/mol FeCl3 for the solution process.FeCl3(s) Fe3+(aq) + 3 Cl-(aq)
Important information about Solution Concentrations, Find the concentration of 500mg of alltrans retinol 0.1% per 1 ounce of solution.
Hydrogen sulfide () is a common and troublesome pollutant in industrial wastewaters. One way to remove is to treat the water with chlorine, in which case the following reaction occurs:
Design a reaction scheme to synthesize pentylbenzene from benzene using a Friedel-Crafts acylation and any other reaction
macroscopic model describing what happens when solutions of salt (NaCl) and sugar (c12h22011) are prepared to measure their conductivity. Describe what you would observe before and after you added salt and sugar to water
The heat of formation of liquid diatomic bromine is 0 kJ/mole. The heat of formation of gaseous diatomic bromine 30.9 kJ/mole. The heat of formation of gaseous monatomic bromine
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