Question 9 Calculate the number of moles and the mass of the solute in the following solution: 2.00 L of 18.5 M H2SO4, concentrated sulfuric acid Question 10 What volume of a 1.00-M Fe(NO3)3 solution can be diluted to prepare 1.00 L of a solution with a concentration of 0.250 M?
Question 9
Calculate the number of moles and the mass of the solute in the following solution:
2.00 L of 18.5 M H2SO4, concentrated sulfuric acid
Question 10
What volume of a 1.00-M Fe(NO3)3 solution can be diluted to prepare 1.00 L of a solution with a concentration of 0.250 M?
Question 10 options:
Question 11
If 0.1718 L of a 0.3556-M C3H7OH solution is diluted to a concentration of 0.1222 M, what is the volume of the resulting solution?
Question 11 options:
Question 12
The level of mercury in a stream was suspected to be above the minimum considered safe (1 part per billion by weight). An analysis indicated that the concentration was 0.68 parts per billion. Assume a density of 1.0 g/mL and calculate the molarity of mercury in the stream.
Question 12 options:
Question 13
What are the mole fractions of H3PO4 and water in a solution of 14.5 g of H3PO4 in 125 g of water?
1) Mole fraction of H3PO4
2) Mole fraction of water
Given , 2.00 L of 18.5 M H2SO4, concentrated sulfuric acid.
We have to calculate the number of moles and mass of the solute.
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