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IrinaK [193]
3 years ago
7

7.00×10−3 mol of HBrare dissolved in water to make 12.0 L of solution. What is the concentration of hydroxide ions, [OH-], in th

is solution?.
Chemistry
2 answers:
frosja888 [35]3 years ago
7 0
To find it in the best way is 
7.00×10^−3 mol of HBr / 18.0 L of solution.= 3.89 e-4 Molar HBr 

<span>3.89 e-4 Molar HBr releases 3.89 e-4 Molar H+ </span>

<span>the pH = - log of 3.89 e-4 Molar H+ </span>

<span>since [H+] [OH-] = 1 e-14 the Kof water </span>

<span>[OH-] = 1 e-14 / 3.89 e-4 = 2.57 e-11 </span>
so we concluded that 
<span>[OH-} = 2.57 X 10^-11 </span>
butalik [34]3 years ago
3 0
Molarity :

M = n / V

M = 7.00 x 10⁻³ / 12.0

= 0.000583 M  => H+

Kw = [ H+] x [OH-]

1 x 10⁻¹⁴ = 0.000583 x [ OH-]

[ OH-] = 1 x 10⁻¹⁴ / 0.000583

[OH-] = 1.71 x 10⁻¹¹

hope this helps!


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89.4%

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When 551. mg of a certain molecular compound X are dissolved in 100 g of benzonitrile (CH,CN), the freezing point of the solutio
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Answer:

1.12g/mol

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The freezing point depression of a solvent for the addition of a solute follows the equation:

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