Question

a popular sports drink has 30.43 g of the sugar sucrose in 500. ml of the beverage. the formula for sugar is c₁₂h₂₂o₁₁. what is the molarity of the sugar in the beverage? c₁₂h₂₂o₁₁ = ? m

Explanation:

Step1: Calculate molar mass of $\ce{C_{12}H_{22}O_{11}}$

Molar mass of C: $12.01\ g/mol$, H: $1.008\ g/mol$, O: $16.00\ g/mol$.
Molar mass $= 12\times12.01 + 22\times1.008 + 11\times16.00$
$= 144.12 + 22.176 + 176.0$
$= 342.296\ g/mol$

Step2: Find moles of $\ce{C_{12}H_{22}O_{11}}$

Moles $= \frac{\text{mass}}{\text{molar mass}} = \frac{30.43\ g}{342.296\ g/mol} \approx 0.0889\ mol$

Step3: Convert volume to liters

$500\ mL = 0.500\ L$

Step4: Calculate molarity

Molarity $= \frac{\text{moles}}{\text{volume (L)}} = \frac{0.0889\ mol}{0.500\ L} \approx 0.178\ M$

Answer:

$0.178$