Make sure to put the correct sig fig!!!!!!!!!!! A 5.00 mL solution of BaCl2 diss

Question

Make sure to put the correct sig fig!!!!!!!!!!!

A 5.00 mL solution of BaCl2 dissolved in water weighed 5.149 g. After the water was removed by heating 0.158 g of BaCl2 remained. Using the formulas on page 44 in the lab manual calculate the following knowing that BaCl2 is the component. Please provide answers in three significant figures. Do not include units in answer. What is the density of the BaCl2 solution in g/mL? Percent-by-mass of the BaCl2 in the solution: Concentration of BaCl2 in the solution in g/mL: How many moles of BaCl2 in the solution. The formula mass of BaCl2 is 208.24 g/mol? What is the molarity of the BaCl2 solution in mol/L?

Explanation / Answer

Density of BaCl2 solution = mass of solution / volume of solution

= 5.149g / 5.00 mL

= 1.0298 g/mL

% BaCl2 in solution = mass of BaCl2 x 100 / mass of solution

= 0.158g x 100 / 5.149g

= 3.0685 %

Concentration of BaCl2 = mass of BaCl2 / volume of solution

= 0.158g / 5.00 mL

= 0.0316

Moles of BaCl2 = mass of BaCl2 / molecular weight

= 0.158g / 208.24g/mol

= 0.0007587 mol

= 7.587 x 10^-4 mol

Molarity of BaCl2 = moles of BaCl2 / volume of solution

= 7.587 x 10^-4 mol / (5.00 mL x 1L/1000 mL)

= 0.152 M

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