Question

The ammonia solution that is purchased for a stockroom has a molarity of 15 M. Determine the volume of 15 M NH3(aq) that must be diluted to 500 mL to prepare 1.46 M NH3(aq). Answer in units of mL.

Answer 1

Answer: The volume of stock solution of ammonia that is needed is 48.67 mL

Explanation:

To calculate the volume of stock solution, we use the equation:

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of the stock ammonia solution

$M_2\text{ and }V_2$ are the molarity and volume of diluted ammonia solution

We are given:

$M_1=15M\\V_1=?mL\\M_2=1.46M\\V_2=500mL$

Putting values in above equation, we get:

$15\times V_1=1.46\times 500\\\\V_1=\frac{1.46\times 500}{15}=48.67mL$

Hence, the volume of stock solution of ammonia that is needed is 48.67 mL

Answer 2

48.66mL is the required volume of stock solution that must be diluted to 500 mL to prepare 1.46 M NH₃(aq).

How we calculate the volume using the molarity?

If molarity of two solutions are given and we have to make solution of different molarity whose molarity is less than the stock solution then we use the formula:

M₁V₁ = M₂V₂

According to the question:

M₁ = molarity of stock ammonia solution NH₃ = 15M

V₁  = volume of stock ammonia solution NH₃ = to find?

M₂ = molarity of diluted ammonia solution NH₃ = 1.46M

V₂ = volume of diluted ammonia solution NH₃ = 500mL

Now we put all these values in the above equation, we get

15 × V₁ = 1.46 × 500

V₁  = 1.46 × 500 / 15 = 48.66mL

Hence, 48.66mL is the required volume of stock solution.

To know more about molarity, visit the below link:

https://brainly.com/question/14469428