What is an example of an aqueous base?

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What is an example of an aqueous base?

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Answer 1 · 2017-09-06T04:39:28

Any aqueous solution of a base qualifies......

Explanation:

$N a O H (a q)$ $NaOH(aq)$ , $K O H (a q)$ $KOH(aq)$ , $N a_{2} C O_{3} (a q)$ $Na_2CO_3(aq)$

Water undergoes the following equilibrium.....the $autoprotolysis reaction$ $"autoprotolysis reaction"$ :

$2 H_{2} O (l) ⇌ H_{3} O^{+} + H O^{-}$ $2H_2O(l) rightleftharpoonsH_3O^+ + HO^-$

And the given equilibrium has been precisely measured under standard conditions....

$[H_{3} O^{+}] [H O^{-}] = 10^{- 14}$ $[H_3O^+][HO^-]=10^-14$

If $[H O^{-}] > 10^{- 7} \cdot m o l \cdot L^{- 1}$ $[HO^-]>10^-7*mol*L^-1$ , then the solution is basic.......and if $[H O^{-}] < 10^{- 7} \cdot m o l \cdot L^{- 1}$ $[HO^-]<10^-7*mol*L^-1$ , then the solution is acidic.....

We can introduce the $p H$ $pH$ measurement by taking $- {log}_{10}$ $-log_10$ of both sides...... $[H_{3} O^{+}] [H O^{-}] = 10^{- 14}$ $[H_3O^+][HO^-]=10^-14$

Thus $-log_10[H_3O^+]-log_10[HO^-]=underbrace(-log_10(10^-14))_14$

And thus our defining relationship, which you will use shortly.....

$underbrace(-log_10[H_3O^+])_(pH)underbrace(-(log_10[HO^-]))_(pOH)=underbrace(-log_10(10^-14))_14$

p H+ p OH = 14

So actual examples..... $NaOH(aq)$ , $Na_2CO_3(aq)$ , $NH_3(aq)$ , $KOH(aq)$ , $NaF$ ..........

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What is an example of an aqueous base?

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Explanation:

p H+ p OH = 14

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