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nignag [31]
9 months ago
8

Calculate the molar solubility of silver(i) bromate with ksp = 5. 5×10-5. also, convert the molar solubility to the solubility.

the molar solubility is ___________ and the solubility is ____________
Chemistry
1 answer:
Sindrei [870]9 months ago
7 0

The molar solubility is 7.4×10^{-3} M and the solubility is  7.4×10^{-3} g/L .

Calculation ,

The dissociation of silver bromide is given as ,

AgBr → Ag ^{+} + Br^{-}

S  

 -          S        S        

Ksp =  [Ag ^{+} ] [ Br^{-} ]  =  [S] [ S ] = S^{2}

S = √ Ksp = √ 5. 5×10^{-5} = 7.4×10^{-3}

The solubility =7.4×10^{-3} g/L

The molar solubility is the solubility of one mole of the substance.

Since ,  one mole of AgBr is dissociates and form one mole of each  Ag ^{+} and Br^{-} ion . So, solubility is equal to molar solubility but unit is different.

Molar solubility = 7.4×10^{-3} mol/L = 7.4×10^{-3} M

To learn more about molar solubility ,

brainly.com/question/16243859

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In a 1.0x10^-4 M solution of HClO(aq), identify the relative molar amounts of these species:HClO, OH-, H3O+, OCl-, H2O
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HClO is a weak acid, which means the ions do not fully dissociate. The hydrolysis reaction for the hypochlorous acid is:

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Then the equilibrium constant, Ka, of dilute HClO would be:

K_{a} = \frac{[ H_{3}  O^{+} ][O Cl^{-} ]}{HClO}

Then we do the ICE table. I is for the initial concentration, C for the change and E for the excess.
      
          HClO       + H2O   ⇄   H3O+ +  OCl-
I     1.0x10^-4                          0             0
C        -x                                 +x           +x 
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Substituting the excess (E) concentration to the Ka equation:

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Simplifying the equation would yield a quadratic equation:

x^{2} + K_{a}x-(1.0 \ x \ 10^{-4}) K_{a}=0

The Ka for HClO is an experimental data which was determined to be 2.9 x 10^-8. Substitute this to the equation, determine the roots, then you get the value for x, which is the concentration of H3O+ and ClO-. Just use your calculator feature Shift-Solve.

x = 1.688 x 10^-6 M = [H3O+] = [ClO-]

Then, you can determine the conc of [OH-] through pH.

pH = -log {H3O+] = -log [1.688 x 10^-6] = 5.77
pOH = 14 - pH = 14 - 5.77 = 8.23
pOH = 8.23 = -log [OH-]
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Also, since HClO is (1.0x10^-4 - x), then it's concentration would be:
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Thus in relative amounts, the order would be

H2O >>> HClO > H3O+ = ClO- > OH-


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