# Chapter 13 - The Chemistry of Solutes and Solutions - Exercise 13.8 - Mass Fraction and Weight Percent - Page 579: a

$0.02\%$

#### Work Step by Step

Mass of water= $density \times volume$ $=\frac{1.00\,g}{mL}\times1.00\,L$ $=\frac{1.00\,g}{10^{-3}\,L}\times1.00\,L=1000\,g$ Mass fraction of $NaHCO_{3}$ $=\frac{mass\,of\,NaHCO_{3}}{mass\,of\,all\,solutes\,and\,the\,solvent}$ = $\frac{0.20\,g}{6.5\,g+0.20\,g+0.10\,g+0.10\,g+1000\,g}= 0.0002$ Weight percent= $mass\, fraction\times100\%$ $= 0.0002\times100\%=0.02\%$

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