Question

8. What was the original concentration in the BHL sample, if the dilution is 1:500 and the concentration 0.07 mg/ml

Answer 1

Answer:

The original concentration is "35 mg/ml".

Explanation:

According to the question,

The solution is diluted,

= 1:50

The initial volume,

V1 = 1 ml

Final concentration,

= 0.07 mg

then,

The final volume,

V2 = 500 ml

As we know,

⇒ $V_1N_1=V_2N_2$

or,

⇒ $N_1=\frac{V_2N_2}{V_1}$

On substituting the values, we get

⇒       $=\frac{500\times 0.07}{1}$

⇒       $=\frac{35}{1}$

⇒       $=35 \ mg/ml$

Answer 2

A 0.07 mg/mL BHL solution was prepared by performing a 1:500 dilution on a 35 mg/mL solution.

A 1:500 dilution was carried out to prepare a 0.07 mg/mL BHL solution. We can find the concentration of the initial solution using the dilution rule.

What is the dilution rule?

It is an equation that relates the concentration and volume of a concentrated and a dilute solution. The mathematical expression is:

C₁ × V₁ = C₂ × V₂

where,

• C₁ is the concentration of the concentrated solution.
• V₁ is the volume of the concentrated solution.
• C₂ is the concentration of the dilute solution.
• V₂ is the volume of the dilute solution.

C₁ = C₂ × (V₂/V₁)

C₁ = 0.07 mg/mL × (500/1) = 35 mg/mL

A 0.07 mg/mL BHL solution was prepared by performing a 1:500 dilution on a 35 mg/mL solution.

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