What volume of 0.826 MKOH solution do you need to make 3.74 L of a solution with a pH of 12.500?

Question

asked Jun 15, 2022 94.1k views

1 Answer

Losses Don · Answer 1 · 2022-06-21T01:35:56+0000

Given that –

We know that –

Then –

$\qquad$
$\bf\longrightarrow pOH = 14 -12.5$

$\qquad$
$\sf \longrightarrow pOH = 1.5$

$\qquad$
$\sf \longrightarrow [OH^- ] = 10^(-1.5 )$

$\qquad$
$\bf \longrightarrow [OH^-] = 3.16 × 10^(-2)$

Now the number of moles of KOH need to ensure that concentration of Hydroxide anions is equal to –

$\qquad$
$\bf \longrightarrow 3.74\: L * (3.16× 10^(-2))/(1 \: L )$

$\qquad$
$\bf \longrightarrow 1. 18 × 10^(-1 )M$

Volume of the solution contains the need number of moles of Hydroxide anions –

$\qquad$
$\sf \longrightarrow ( 1.18×10^(-1) \: moles \: OH^-)/(0.826 \: moles \: OH^-)$

$\qquad$
$\sf \longrightarrow 0.143 L$

$\qquad$
$\sf \longrightarrow 0.143 * 1000$

$\qquad$
$\pink{\bf\longrightarrow 143 mL }$

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