A $0.200 \cdot g$ $0.200g$ mass of sodium hydroxide is dissolved in a $0.500 \cdot L$ $0.500L$ volume of water? What are $p O H$ $pOH$ , and $p H$ $pH$ of this solution?

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A $0.200 \cdot g$ $0.200g$ mass of sodium hydroxide is dissolved in a $0.500 \cdot L$ $0.500L$ volume of water? What are $p O H$ $pOH$ , and $p H$ $pH$ of this solution?

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Answer 1 · 2017-01-04T06:13:16

$p H = 14 - p O H$ $pH=14-pOH$

Explanation:

$[H O^{-}] = \frac{Moles of hydroxide}{Volume of solution}$ $[HO^-]="Moles of hydroxide"/"Volume of solution"$

$= \frac{\frac{0.2 \cdot g}{40.00 \cdot g \cdot m o l^{- 1}}}{0.500 \cdot L} = 0.01 \cdot m o l \cdot L^{- 1}$ $=((0.2*g)/(40.00*g*mol^-1))/(0.500*L)=0.01*mol*L^-1$ .

We (reasonably) assume no volume change on dissolution. Some heat will be evolved. Why?

$p O H = - {log}_{10} [H O^{-}] = - {log}_{10} (10^{- 2}) = - (- 2) = 2$ $pOH=-log_10[HO^-]=-log_10(10^-2)=-(-2)=2$ .

But we know for a fact that $p H + p O H = 14$ $pH+pOH=14$

And thus $pH=............?$

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A $0.200 \cdot g$ $0.200g$ mass of sodium hydroxide is dissolved in a $0.500 \cdot L$ $0.500L$ volume of water? What are $p O H$ $pOH$ , and $p H$ $pH$ of this solution?

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A 0.200*g0.200⋅g0.200*g mass of sodium hydroxide is dissolved in a 0.500*L0.500⋅L0.500*L volume of water? What are pOHpOHpOH, and pHpHpH of this solution?

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A $0.200 \cdot g$ $0.200g$ mass of sodium hydroxide is dissolved in a $0.500 \cdot L$ $0.500L$ volume of water? What are $p O H$ $pOH$ , and $p H$ $pH$ of this solution?