A sample of 25.00 g of borax, Na₂B₄O₇· 10H₂O, is heated gently until it loses all its water, and…

A sample of $25.00\ \text{g}$ of borax, $\text{Na}_{2}\text{B}_{4}\text{O}_{7}\cdot 10\text{H}_{2}\text{O}$, is heated gently until it loses all its water, and then strongly until it forms a clear glass of sodium metaborate and boron(III) oxide: $\text{Na}_{2}\text{B}_{4}\text{O}_{7} \to 2\text{NaBO}_{2} + \text{B}_{2}\text{O}_{3}$. The molar masses are $381.37\ \text{g/mol}$ for borax, $201.22\ \text{g/mol}$ for $\text{Na}_{2}\text{B}_{4}\text{O}_{7}$, $65.80\ \text{g/mol}$ for $\text{NaBO}_{2}$ and $69.62\ \text{g/mol}$ for $\text{B}_{2}\text{O}_{3}$. Find the mass of water lost, the mass of anhydrous $\text{Na}_{2}\text{B}_{4}\text{O}_{7}$ left, and the masses of $\text{NaBO}_{2}$ and $\text{B}_{2}\text{O}_{3}$ in the glass.