Question

Calculate the volume (ml) of 0.5 mol/L solution, containing 2 g of barium nitrate.​

Answer 1

Answer:

The more the solution of a reactant is diluted, the slower the reaction will occur.

Explanation:

The key thing you need to understand here is that chemical reactions depend on reactant particles bumping into each other (collision theory).

The more concentrated a reactant is, the more likely it will be to bump into other reactants and product chemical change.

Here is video of a quick lab performed to test this. In the video, varying concentrations of

N

a

2

S

2

O

3

are allowed to react with HCl. A timer is included in the video so you can see how the changing concentration changes the overall speed of the reaction!

Answer 2

Given: 0.5 mol/L solution is given containing 2 g of barium nitrate

To find: Volume in mL

Explanation: Given mass of barium nitrate= 2 g

Molar mass of barium nitrate= 261 g/mol

Number of moles

= Given mass/ Molar mass

= 2/261

= 0.0076 moles

Strength of the solution= 0.5 mol/L

Strength= Number of moles/ Volume in L

=> Volume in L

= Number of moles/ Strength

= 0.0076/0.5

= 0.0153 L

Volume in mL

= 0.0153 * 1000( 1 L = 1000 mL)

= 15.3 mL

Therefore, the volume of the solution is 15.3 mL.