A solution of F^- is prepared by dissolving 0.0889 plusminus 0.0004g of NaF(molecular weight= 41.989 plusminus 0.001g/mol) in 163.00 plusminus 0.06 mL of water. Calculate the concentration of F^- in solution and its absolute uncertainty.
A solution of F^- is prepared by dissolving 0.0889 plusminus 0.0004g of NaF(molecular weight= 41.989 plusminus...
A solution of F− is prepared by dissolving 0.0722±0.0005 g NaF (molar mass = 41.989±0.001 g/mol) in 154.00±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.
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.
A solution of F− is prepared by dissolving 0.0744±0.0005 g NaF (molar mass = 41.989±0.001 g/mol) in 157.00±0.07 mL of water. Calculate the concentration of F− in solution and its absolute uncertainty.
A solution of F− is prepared by dissolving 0.0887±0.0006 g NaF (molar mass = 41.989±0.001 g/mol) in 152.00±0.09 mL of water. Calculate the concentration of F− in solution and its absolute uncertainty.
A 0.5L of a solution is prepared by dissolving 120.9g of NaF in it. The molecular weight of NaF is 41.9g/mol). If I took 0.18L of that solution and diluted it to 0.4, what is the molarity of the resulting solution? Answer to 3 significant figures Read about significant figures and rounding in the Helpful Resources page! .Do not include units when reporting your answer Use standard notation or scientific notation as accepted by blackboard e.g. 0.001 or 1E-3, not...
3. A solution of A is prepared by dissolving 0.1658+0.0006 g NaA (molar mass = 55.462+0.001 g/mol) in 235.00+0.04 mL of water. Calculate the molarity of A in solution and its absolute uncertainty. Be sure to use the correct number of significant figures for the final answer. (10 points)
3. A solution of Ais prepared by dissolving 0.1658+0.0006 g NaA (molar masse 55 A6240.001 g/mol) in 235.00:0.04 ml. of water. Calculate the molarity of Ain solutice and its absolute uncertainty. Be sure to use the correct number of significant figures for the final answer (10 points)
3. A 0.9L of a solution is prepared by dissolving 126.2g of NaF in it. The molecular weight of NaF is 41.9g/mol). If I took 0.13L of that solution and diluted it to 0.5, what is the molarity of the resulting solution? Answer to 3 significant figures Read about significant figures and rounding in the Helpful Resources page! Do not include units when reporting your answer Use standard notation or scientific notation as accepted by blackboard e.g. 0.001 or 1E-3,...
A solution prepared by dissolving 14.5 mg of a nonelectrolyte in water and diluting to a volume of 10.0 mL gives an osmotic pressure of 33.8 mmHg at 300. K. What is the molecular weight of the nonelectrolyte in g/mol?
A 500.0±0.2-mL solution was prepared by dissolving 25.00±0.03 mL of methanol (CH3OH, density=0.7914±0.0002 g/mL, molecular mass=32.0419±0.0009 g/mol) in chloroform. Find the molarity ± uncertainty of the methanol.