Question

A sugar solution is prepared by dissolving 12.5 g sucrose, C12H22O11, in 25.0 mL water. Calculate the mass percent and mole fraction of sucrose in the solution. The density of water is 1.00 g·mL-1. Molar Mass: C12H22O11 = 342.3 g/mol H2O = 18.02 g/mol

          A sugar solution is prepared by dissolving 12.5 g sucrose, C12H22O11, in 25.0 mL water. Calculate the mass percent and mole fraction of sucrose in the solution. The density of water is 1.00 g·mL-1.
Molar Mass:
C12H22O11 = 342.3 g/mol
H2O = 18.02 g/mol

$A sugar solution is prepared by dissolving 12.5 g sucrose, C12H22O11, in 25.0 mL water. Calculate the mass percent and mole fraction of sucrose in the solution. The density of water is 1.00 g·mL-1. Molar Mass: C12H22O11 = 342.3 g/mol H2O = 18.02 g/mol$

Added by Popotinha

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Chapter 13

Instant Answer

Solved by Expert Shalini Tyagi

02/27/2025

Step 1

Given that the density of water is $1.00 \, \text{g/mL}$, the mass of 25.0 mL of water is: \[ \text{Mass of water} = 25.0 \, \text{mL} \times 1.00 \, \text{g/mL} = 25.0 \, \text{g} \] Show more…

Show all steps