Question

How many mL of a 56.2mEq K /L solution contain 42.8 Eq K

Answer 1

There is approximately 761.56 mL of the 56.2 mEq/L solution is required to have 42.8 Eq of K⁺.

To find the volume of a solution containing a specific amount of potassium ions (K⁺), we can use the equation:

`\[ \text{Volume (mL)} = \frac{\text{Amount of K⁺ (Eq)}}{\text{Concentration (mEq/L)}} \]`

Given:

- Concentration of K⁺ in the solution = 56.2 mEq/L

- Amount of K⁺ needed = 42.8 Eq

Plug these values into the formula:

`\[ \text{Volume (mL)} = \frac{42.8 \, \text{Eq}}{56.2 \, \text{mEq/L}} \]`

Calculate:

`\[ \text{Volume (mL)} = (42.8)/(56.2) * 1000 \]`

`\[ \text{Volume (mL)} \approx 761.56 \, \text{mL} \]`

So, approximately 761.56 mL of the 56.2 mEq/L solution is needed to contain 42.8 Eq of K⁺.