\( \frac { 0.6 g \times 0.082 atm . L / mol . K \times 500 K } { 0.984 atm \times 0.5 K } \)

Example Naturally occurring chlorine consists of \( 75.77 \% \) chlorine-35 atoms (mass 34.97 amu ) and \( 24.23 \% \) chlorine-37 atoms (mass 36.97 amu ). Calculate its atomic mass.

\( \frac { 0.6 g \times 0.082 atm . L / mol . K \times 500 K } { 0.984 atm \times 0.5 K } \)

Classify this solution as acidic, basic, or neutral.

\( \mathrm{NH}_{4} \mathrm{OH} \) \( \begin{array}{l}\text { strong } \\ \text { weak }\end{array} \)

\( \mathrm{HI}(a q) \) and \( \mathrm{NaOH}(a q) \) Express your answer as a balanced chemical equation. Identify all of the phases in your answer.