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ELEN [110]
3 years ago
7

Calculate the poH if 2.95 g of KOH(s) dissolved to make 100mL of solution

Chemistry
1 answer:
Elodia [21]3 years ago
4 0

Answer:

\rm pOH \approx 1.279 if 2.95\; \rm g of \rm KOH is dissolved completely in water to make a 100\; \rm mL solution.

Explanation:

Look up the relative atomic mass data on a modern periodic table:

  • \rm K: 39.098.
  • \rm O: 15.999.
  • \rm H: 1.008.

Calculate the formula mass of \rm KOH:

\begin{aligned}&M(\mathrm{KOH})\\ &= 39.098 + 15.999 + 1.008 \\ &= 56.105\; \rm g \cdot mol^{-1}\end{aligned}.

Find the number of moles of formula units in that 2.95\; \rm g of \rm KOH:

\begin{aligned}& n(\mathrm{KOH}) \\ & = \frac{m(\mathrm{KOH})}{M(\mathrm{KOH})} = \frac{2.95\; \rm g}{56.105\; \rm g \cdot mol^{-1}} \approx 0.0525800\; \rm mol \end{aligned}.

\rm KOH is a strong base. When dissolved in water, it ionizes completely to produce \rm K^{+} ions and hydroxide ions (\rm OH^{-}.)

Note that there are one moles of \rm OH^{-} ions in each mole of \rm KOH formula units. When that 2.95\; \rm g of \rm KOH (approximately 0.0525800\; \rm mol of \rm KOH formula units) dissolves completely in water to make a 100\; \rm mL solution, about 0.0525800\; \rm mol of \rm OH^{-} ions will be produced.

Convert the unit of volume to liters: V = 100\; \rm mL = 0.1\; \rm L.

Calculate the concentration of \rm OH^{-} ions in that solution:

\begin{aligned}&[\mathrm{OH^{-}}] \\ &= \frac{n}{V} \approx \frac{0.0525800\; \rm mol}{0.1 \; \rm L} \approx 0.525800\; \rm mol \cdot L^{-1} \end{aligned}.

Calculate the \rm pOH of that solution:

\begin{aligned}& \mathrm{pOH} \\ &= -\log_{10}[\mathrm{OH^{-}}] \\ &\approx -\log_{10}(0.525800) \approx 1.279\end{aligned}.

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Explanation:

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