Question #133bf
1 Answer
Explanation:
I'll assume the hydrate is copper
We're asked to find the percentage by mass of
To do this, what we can do is find the molar mass of
#5(overbrace((2)(1.008color(white)(l)"g/mol"))^"hydrogen" + overbrace(15.999color(white)(l)"g/mol")^"oxygen")#
#= color(red)(ul(90.076color(white)(l)"g/mol")#
#overbrace(63.546color(white)(l)"g/mol")^"copper" + overbrace(32.066color(white)(l)"g/mol")^"sulfur" + overbrace((4)(15.999color(white)(l)"g/mol"))^"oxygen" + overbrace(color(red)(90.076color(white)(l)"g/mol"))^"water"#
#= color(green)(ul(249.68color(white)(l)"g/mol"#
The mass percentage of
#%"H"_2"O" = ("mass H"_2"O")/("mass CuSO"_4·5"H"_2"O") xx 100%#
#= (color(red)(90.076color(white)(l)"g/mol"))/(color(green)(249.68color(white)(l)"g/mol")) xx 100% = color(blue)(ulbar(|stackrel(" ")(" "36.1%" ")|)#