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n200080 [17]
3 years ago
15

What is the ph of a 0.01 m solution of the strong acid hno3 in water?

Chemistry
2 answers:
kumpel [21]3 years ago
6 0
Answer is: pH <span>of a 0,01 M solution is 2.
c(HNO</span>₃) = 0,01 M = 0,01 mol/L.
pH = -log(c(HNO₃).
pH = -log(0,01 mol/L).
pH = 2.
pH<span> is a numeric scale used to specify the </span>acidity<span> or </span>basicity<span> of an </span>aqueous solution<span>. If pH is less than seven, than solution is acidic and if pH is greater seven, solution is basic, if pH is equal seven, solution is neutral.</span>
frutty [35]3 years ago
4 0
The pH = - log (H+)
a 0.01 solution of a strong acid HNO3 in water contains 0.01 M of hydrogen ions(H+)
Therefore, pH = - log (0.01)
                       = 2
Therefore, the pH is 2
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sattari [20]

Answer:

Your strategy here will be to use the molar mass of potassium bromide,

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So, a compound's molar mass essentially tells you the mass of one mole of said compound. Now, let's assume that you only have a periodic table to work with here.

Potassium bromide is an ionic compound that is made up of potassium cations,

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M

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−

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For Br:

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M KBr

=

39.0963 g mol

−

1

+

79.904 g mol

−

1

≈

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−

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3

moles KBr

⋅

molar mass of KBr



119 g

1

mole KBr

=

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You should round this off to one sig fig, since that is how many sig figs you have for the number of moles of potassium bromide, but I'll leave it rounded to two sig figs

mass of 3 moles of KBr

=

∣

∣

∣

∣

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a

a

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a

a

∣

∣

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