A solution of F− is prepared by dissolving 0.0986±0.0004 g NaF (molar mass = 41.989±0.001 g/mol...
A solution of F− is prepared by dissolving 0.0986±0.0004 g NaF (molar mass = 41.989±0.001 g/mol ) in 162.00±0.06 mL of water. Calculate the concentration of F− in solution and its absolute uncertainty. Significant figures are graded for this problem. To avoid rounding errors, do not round your answers until the very end of your calculations.
Homework Answers
Concentration of F- = 0.0145 +/- 0.0001 M
Explanation
Mass NaF = 0.0986 +/- 0.0004 g
molar mass NaF = 41.989 +/- 0.001 g/mol
moles NaF = (Mass NaF) / (molar mass NaF)
moles NaF = (0.0986 +/- 0.0004 g) / (41.989 +/- 0.001 g/mol)
moles NaF = 0.002348234061 +/- 0.00000958223 mol
Volume of solution = 162.00 +/- 0.06 mL
Volume of solution = 0.16200 +/- 0.00006 L
Concentration of F- = (moles NaF) / (Volume of solution)
Concentration of F- = (0.002348234061 +/- 0.00000958223 mol) / (0.16200 +/- 0.00006 L)
Concentration of F- = 0.0144953 +/- 0.0000645 M
Concentration of F- = 0.0145 +/- 0.0001 M
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