Q3.134CP - Chemistry: Molecular Nature Of Matter And Change

Question

Assuming that the volume are additive, what is the concentration of KBr in a solution prepared by mixing 0.200 L of 0.053 M KBr with 0.550 L of 0.078 M KBr?

Step-by-Step Solution

Answer

The concentration of solution after mixing is$0.0713\text{M}$

Step 1: Calculation of moles:

Given:

Volume of KBr solution(V₁) = $\text{0.200 L}$

Molarity of KBr solution(M₁)=$\text{0.053M}$

Volume of KBr solution(V₂) = $\text{0.550 L}$

Molarity of KBr solution(M₂)=$\text{0.078 M}$

 $$\begin{gathered} \text{Molarity = }\frac{\text{moles of solute}}{\text{liters of solution}} \\ \text{moles of solute}=\text{Molarity}\times \text{liters of solution} \end{gathered}$$

$$\begin{gathered} \text{moles of KBr in 0.200 L of 0.53M} \\ \text{ = 0.200 L }\times \text{ 0.53M} \\ \text{ = 0.0106 moles} \\ \text{moles of KBr in 0.550 L of 0.078 M} \\ \text{ = 0.550 L }\times \text{ 0.078M } \\ \text{ = 0.0429 moles} \end{gathered}$$

Step 2: Calculation of total number of moles

Let us calculate the total number of moles present in solution after mixing.

$$\begin{gathered} \text{0.0106 moles}+\text{0.0429 moles} \\ 0.0535\text{moles} \end{gathered}$$

Step 3: Calculation of total volume of solution after mixing

Let us calculate the total volume of solution after mixing.

$$\begin{gathered} \text{0.200 L}+\text{0.550 L} \\ \text{ = 0.750 L} \end{gathered}$$

Step 4: Calculation of concentration of solution after mixing

Let us calculate the concentration of solution after mixing.

$\text{Molarity = }\frac{\text{Total number of moles of solute}}{\text{ Total volume of solution}}$

$$\begin{gathered} \text{Molarity = }\frac{0.0535\text{mole}}{\text{ 0.750 L}} \\ =0.0713\text{M} \end{gathered}$$

Result:

The concentration of solution obtained after mixing is $0.0713 \text{M}$