According to the label on a bottle of concentrated hydrochloric acid, the conten

Question

According to the label on a bottle of concentrated hydrochloric acid, the contents are 36.0% HCl by mass and have a density of 1.18 g/mL. 1st attempt Part 1 (0.3 point) In See Periodic Table O See Hirnt What is the molarity of concentrated HCI? Part 2 (0.3 point) What volume of it would you need to prepare 881 mL of 1.00 MHCI? mL Part 3 (0.3 point) What mass of sodium bicarbonate would be needed to neutralize the spill if a bottle containing 1.75 L of concentrated HCl dropped on a lab floor and broke open?

Explanation / Answer

Molar mass of HCl = 36.46 g/mol
Given density = 1.18 g/mL = 1180 g/L
the weight of 1 litre of solution = 1180 grams
Using the percent to calculate the mass of HCl in 1180 g,
1180 x 36.0% = 1190 x 0.36 = 424. 8 g HCl

Now we know the weight of HCl per liter.
Convert the weight of HCl to moles of HCl-
424. 8 g / 36.46 g/mol = 11.65 moles of HCl in 1.000 litre
Molarity = 11.65 M

(b) Using M1V1 = M2V2
11.65 x V = 1.00 x 0.881 L
V = 0.0756 L = 75.6 mL

(c)
moles HCl = 1.75 L x 11.65 M = 20.3875
moles NaHCO3 needed = 20.3875
mass NaHCO3 = 20.3875 x 85 g/mol=1733 g

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