(5) Using the periodic table in the lab manual, the molar mass of mercury (II) n

Question

(5) Using the periodic table in the lab manual, the molar mass of mercury (II) nitrate dihydrate is_____ g/mol.

(6) How many grams of mercury (II) nitrate dihydrate are needed to prepare 100.00 mL of 0.0975 M solution? ____

(7) Using the periodic table in the lab manual, the molar mass of copper (II) bromide trihydrate is _____ g/mol.

(8) How many grams of copper (II) bromide trihydrate are needed to prepare 50.00 mL 0.215938 M solution? g

(24) Parts per Million (ppm) is defined as ug (of solute)/g (of solution). How many grams of potassium bromide will be needed to prepare 500.00 mL of 275 ppm Br- solution? g

(29) When performing dilutions, the dilution law C1V1=C2V2 is very helpful. What is the final concentration if 15.00 mL of 6.39% NaClO solution is diluted to 250.00 mL? %

(11) Using the periodic table in the lab manual, the molar mass of magnesium phosphate octahydrate is _____ g/mol.

(12) If 6.7815 g of magnesium phosphate octahydrate was used to prepare 250.00 mL of solution, what is the molarity?____ M

Explanation / Answer

5 ) HgNO3 .2H2O molar mass = 298.63 g/mol

6)

molarity = (mass / molar mass ) x (1000 / volume)

0.0975 = (mass / 298.63) x (1000/ 100)

mass = 2.91 g

7)   CuBr2 .3 H2O molar mass = 277.40 g /mol

8)

0.215938 = (mass / 277.40 ) x 1000 / 50

mass = 3.0 g

11 ) 442.86 g/mol

12 )

molarity =( 6.7815 / 442.86 ) x 1000/ 250

molarity = 0.061 M

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