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Verdich [7]
3 years ago
9

Question 25 An aqueous solution at has a concentration of . Calculate the concentration. Be sure your answer has the correct num

ber of significant digits.
Chemistry
1 answer:
Natalka [10]3 years ago
8 0

The given question is lacking some details, the complete question is following

Question:

An aqueous solution at 25 °C has a OH⁻ concentration of 2.5 x 10⁻⁴ M . Calculate the H₃O⁺ concentration. Be sure your answer has the correct number of significant digits

Answer:

Concentration of H₃O⁺ is:

[H_{3}O^{+}]=4.0X10^{-9} M

Explanation:

In aqueous solutions the product of the concentration of hydronium ions H₃O⁺ and hydroxide ions OH⁻ is 1.0 x 10⁻¹⁴. This value is the dissociation or ionization constant of water at 25 °C. Its formula is given as:

Kw = [H_{3} O^{+}][OH^{-} ]

1.0 X 10^{-14}= [H_{3}O^{+}](2.5 X 10^{-4})

[H_{3}O^{+}]= \frac{1.0X10^{-14}}{2.5 X 10^{-4}}

[H_{3}O^{+}]=4.0X10^{-9} M

P.S: As the smallest number of significant figure in the ratio was two, so the answer contains two significant figures.

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Answer:- Third choice is correct, 17.6 moles


Solution:- The given balanced equation is:


Al_2(SO_4)_3+6KOH\rightarrow 2Al(OH)_3+3K_2SO_4


We are asked to calculate the moles of potassium hydroxide needed to completely react with 2.94 moles of aluminium sulfate.


From the balanced equation, there is 1:6 mol ratio between aluminium sulfate and potassium hydroxide.


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So, Third choice is correct, 17.6 moles of potassium hydroxide are required to react with 2.94 moles of aluminium sulfate.



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