Question 3 (Molarity)
What is the molarity of a solution made by dissolving 50.0 g of HBr in enough water to
make 600. mL of solution?

The molarity of the solution is 1,03 M.

Explanation:

Molarity is a concentration measure that expresses the moles of solute (in this case HBR) in 1 liter of solution (1000ml). First we calculate the mass of 1 mol of HBr, to calculate the moles that are in 50 g of said compound:

Weight 1 mol HBr= Weight H + Weight Br= 1,01g + 79,90g= 80, 91 g/mol

80,91 g 1 mol HBr

50,0 gx= (50,0 g x1 mol HBr)/80,91 g= 0,62 mol HBr

600 ml solution0,62 mol HBr

1000ml solutionx= (1000ml solution x 0,62 mol HBr)/600 ml solution

x=1,03 moles HBr ---> The solution is 1,03M

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.