Two $1-L$ beakers, A and $B,$ each containing a different aqueous solution of maltose $($a nonvolatile sugar with $MW=342\mathrm{.}30\frac{g}{m}ol)$ are placed together in a box, which is then sealed. The temperature remains constant at $20C.$ Initially, there is $170mL$ of solution in A and $800mL$ of solution in B$.$ As the solutions stand in the sealed box, their volumes change slowly for a while. When they stop changing, beaker A contains $470mL$ and beaker B contains $500mL.$ It is then determined that the solution in $A$ is $1\mathrm{.}06M$ in maltose and has a density of $1\mathrm{.}14gm{L}^{-1}.$

$($a$)$ What is the molar concentration of maltose in the solution in beaker B at the end? M

$($b$)$ Calculate the concentration of maltose in the solution in A at the start.

M

$($c$)$ Calculate the concentration of the maltose in the solution in B at the start.

M

$($d$)$ The vapor pressure of pure water at $20C$ is $17\mathrm{.}5$ torr.

What is the pressure of water vapor in the box at the end, after the volumes have stopped changing? torr