According to a 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.
1. what is the molarity of concentrated hcl.
2. what volume of it would you need to prepare 985 ml of 1.6 m hcl?
3. 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?

1) 11.64 mol/L is the molarity of concentrated HCl.

2) 135.40 mL of  volume of 11.64 M will need to prepare 985 mL of 1.6 M HCl.

3) 1,711.08 grams of sodium bicarbonate would be needed to neutralize the spill HCl solution.

Explanation:

HCl solution with 36.0% HCl by mass, menas that in 100 g of solution 36.0 gram of HCl is present.

Mass of HCl= 36.0 g

Moles of HCl =

Mass of solution ,m= 100 g

Volume of solution = V = ?

Density of the solution ,d= 1.18 g/mL

Molarity of the solution :

11.64 mol/L is the molarity of concentrated HCl.

2)

( Dilution equation)

135.40 mL of  volume of 11.64 M will need to prepare 985 mL of 1.6 M HCl.

3.

Concentration of HCl solution = 11.64 M

Volume of the HCl solution = 1.75 L

Moles of HCl in 1.75 L solution = n

According to reaction 1 mole of HCl neutralized by 1 mole of sodium carbonate.

Then 20.37 moles of HCl will neutralized by ;

of sodium carbonate

Mass of 20.37 moles of sodium carbonate :

= 20.37 mol × 84g/mol = 1,711.08 g

1,711.08 grams of sodium bicarbonate would be needed to neutralize the spill HCl solution.

answer

i think the answer is a) as air pressure in an area increases, the density of the gas particles in that area decreases.

hope it

the answer is either b or c