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wolverine [178]
3 years ago
7

What mass of potassium hypochlorite (FW-90.6 g/mol) must be added to 4.50 x 10 mL of water to give a solution with pH 10.20? [Ka

(HCIO) 4.0 x 10-8] 0.032g ? 2.4 g 04.1 g 9.1 g 20. g
Chemistry
1 answer:
marta [7]3 years ago
6 0

Answer : The mass of potassium hypochlorite is, 4.1 grams.

Explanation : Given,

pH = 10.20

Volume of water = 4.50\times 10^2ml=0.45L

The decomposition of KClO  will be :

KClO\rightarrow K^++ClO^-

Now the further reaction with water (H_2O) to give,

ClO^-+H_2O\rightarrow HClO+OH^-

First we have to calculate the pOH.

pH+pOH=14\\\\pOH=14-pH\\\\pOH=14-10.20=3.8

Now we have to calculate the OH^- concentration.

pOH=-\log [OH^-]

3.8=-\log [OH^-]

[OH^-]=1.58\times 10^{-4}M

Now we have to calculate the base dissociation constant.

Formula used : K_b=\frac{K_w}{K_a}

Now put all the given values in this formula, we get :

K_b=\frac{1.0\times 10^{-14}}{4.0\times 10^{-8}}=2.5\times 10^{-7}

Now we have to calculate the concentration of ClO^-.

The equilibrium constant expression of the reaction  is:

K_b=\frac{[OH^-][HClO]}{[ClO^-]}

As we know that, [OH^-]=[HClO]=1.58\times 10^{-4}M

2.5\times 10^{-7}=\frac{(1.58\times 10^{-4})^2}{[ClO^-]}

[ClO^-]=0.0999M

Now we have to calculate the moles of ClO^-.

\text{Moles of }ClO^-=\text{Molarity of }ClO^-\times \text{Volume of solution}

\text{Moles of }ClO^-=0.0999mole/L\times 0.45L=0.0449mole

As we know that, the number of moles of ClO^- are equal to the number of moles of KClO.

So, the number of moles of KClO = 0.0449 mole

Now we have to calculate the mass of KClO.

\text{Mass of }KClO=\text{Moles of }KClO\times \text{Molar mass of }KClO

\text{Mass of }KClO=0.0449mole\times 90.6g/mole=4.07g\approx 4.1g

Therefore, the mass of potassium hypochlorite is, 4.1 grams.

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