What mass of AgOH is present in a sample if it is titrated to its equivalence point with 58.5 mL of 0.0663 M HNO₃? The balanced chemical equation is as follows: AgOH + HNO₃$\rightarrow$AgNO₃ + H₂O A) 0.485 g B) 0.00388 g C) 258 g D) 1.13 g E) 2.27 g

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The balanced chemical equation shows a 1:1 mole ratio between AgOH and HNO₃. To find the mass of AgOH, first calculate the moles of HNO₃ used: $58.5 \, \text{mL} \times 0.0663 \, \text{M} = 0.00388 \, \text{moles}$. Since the mole ratio is 1:1, there are also 0.00388 moles of AgOH. The molar mass of AgOH is approximately 124.88 g/mol, so the mass of AgOH is $0.00388 \, \text{moles} \times 124.88 \, \text{g/mol} = 0.485 \, \text{g}$.

What Mass of AgOH Is Present in a Sample If →\rightarrow→

What Mass of AgOH Is Present in a Sample If $\rightarrow$