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10 Nov 2019
aanswer in details please
The pH of a 4.48x10-4 M solution of a weak base is 10.02. Calculate Kb for this base to three significant figures. The mole fraction of an aqueous solution of lithium nitrite is 0.116. Calculate the molarity (in mol/L) of the lithium nitrite solution, if the density of the solution is 1.49 g mL-1. Determine the mole fraction of sodium iodate in a 4.62 M aqueous solution of sodium iodate. The density of the solution is 1.49 g mL-1.
aanswer in details please
The pH of a 4.48x10-4 M solution of a weak base is 10.02. Calculate Kb for this base to three significant figures. The mole fraction of an aqueous solution of lithium nitrite is 0.116. Calculate the molarity (in mol/L) of the lithium nitrite solution, if the density of the solution is 1.49 g mL-1. Determine the mole fraction of sodium iodate in a 4.62 M aqueous solution of sodium iodate. The density of the solution is 1.49 g mL-1.
Nelly StrackeLv2
10 Nov 2019