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A 4.867 g sample of a monoprotic acid was dissolved in water. It took 30.24 mL of a 0.1578 M NaOH solution to neutralize the acid. Calculate the molar mass of the acid.
Acetylene gas (C2H2) is produced as a result of the following reavtion. CaC2(s) + 2H2O(l) yield C2H2(g) +Ca(OH)2(aq)
A fluoridated water supply contains F- at a concentration of 8.9 ppm. What is the maximum concentration of Mg2+ that can exist in this water supply without causing precipitation.
If a 2.743g sample of MgSO4.7H2O were heated strongly,what would be the expected mass of the cooled dehydrated salt
A solution is made by mixing 500 mL of .121 M NaOH with 500 mL of .1 M CH3COOH. Calculate the equalibrium concentrations of H+. CH3COOH, CH3COO-, OH- and Na+
72.0 mL of a 1.40 M solution is diluted to a volume of 278 mL. A 139-mL portion of that solution is diluted using 161 mL of water. What is the final concentration.
The initial concentration of some weak acid, HA, in an aqueous solution is 0.2150 M, at equilibrium the concentration of HA becomes 0.0955 mol/L.
Using a sample of gas has a mass of 38.7mg. Calculate the molar mass if its volume is 228mL at a temperature of 57°C and a pressure of 832torr?
A mixture of gases containing 21.0 g of N2, 106.5 g of Cl2, and 12.0 g of He at 14 oC is in a 50.0 L container. What is the partial pressure of N2?
Determine the trend in sizes of the ions O 2- ,N 3- , F - and also explain why does the trend exist? Also describe which of the molecules contains polar covalent bonds but is NOT itself a polar molecule?
Acetone, the solvent in some nail polish removers, has a density of 0.791 g/mL. What is the volume of 20.4 g of acetone?
At 8:00 a.m., a patient receives a 58-mg dose of I -131 to obtain an image of her thyroid. If the nuclide has a half-life of 8 days, what mass of the nuclide remains in the patient at 5:00 p.m.
Determine How much heat energy, is needed to convert 64.0 grams of ice at -18.0 degrees Celsius to H 2 O at 25.0 Normal Temperature ? express your answer in kilojoules
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