A 5.00 mL solution of BaCl_2 dissolved in water weighed 5.360 g. After the water

Question

A 5.00 mL solution of BaCl_2 dissolved in water weighed 5.360 g. After the water was removed by heating 0.369 g of BaCL_2, remained. Using the formulas on page 38 in the lab manual calculate the following knowing that BaCl_2 is the component. What is the density of the BaCl_2 solution in g/mL? Percent by-mass the BaCl_2 in the solution: Concentration of BaCl_2 in the solution: How many moles of BaCl_2 in the solution. The formula mass of BaCl_2 is 208.24 g/mol (Use mol as unit for mole)? What is the molarity of the BaCl_2 solution in mol/L?

Explanation / Answer

A) density of solution=mass of solution/volume of solution

density=5.36/5=1.072g/ml

B) % of BaCl2:- mass of BaCl2/total mass=(0.369/5.36)×100=6.884%

C) concentration of BaCl2 in solution=mass of BaCl2/volume of solution=0.369/5=0.0738g/ml

D) moles of BaCl2:- given mass/molar mass=0.369/208.24

Moles=0.0177

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