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irinina [24]
3 years ago
13

Calculate the concentration of H3O+ in a solution that contains 5.5 × 10-5 M OH- at 25°C. Identify the solution as acidic, basic

, or neutral.
a. 1.8 × 10-10 M, acidic
b. 9.2 × 10-1 M, basic
c. 5.5 × 10-10 M, neutral
d. 9.2 × 10-1 M, acidic
e. 1.8 × 10-10 M, basic
Chemistry
1 answer:
defon3 years ago
6 0

Answer:

The correct answer is option (e).

Explanation:

Concentration of hydroxide ions [OH^-]= 5.5\times 10^{-5} M

The pOH of the solution is defined as negative logarithm of hydroxide ions of in an aqueous solution.

  • Higher the value of pOH more will be the acidic solution.
  • Lower the value of pOH more will be the basic solution.
  • At value  equal to 7 the solution is said to be neutral.

pOH=-\log[OH^-]

pOH=-\log[5.5\times 10^{-5} M]=4.259

pH +pOH = 14

pH = 14-pOH

pH=14 - 4.259 = 9.741

The pH of the solution is defined as negative logarithm of hydronium ions of in an aqueous solution.

  • Higher the value of pH more will be the basic solution.
  • Lower the value of pH more will be the acidic solution.
  • At value equal to 7 the solution is said to be neutral.

pH=-\log[H_3O^+]

9.741=-\log[H_3O^+]

[H_3O^+]=1.8\times 10^{-10} M

The solution is basic as pH of the solution is 9.741.

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Calculate the concentration of so42− ions in a 0.010 m aqueous solution of sulfuric acid. express your answer to four decimal pl
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<span>Answer: 0.00649M


The question is incomplete,
</span>

<span>You are told that the first ionization of the sulfuric acid is complete and the second ionization of the sulfuric acid has a constant Ka₂ = 0.012
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<span>
With that you can solve the question following these steps"
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<span>1) First ionization:
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<span>
H₂SO₄(aq) --> H⁺ (aq) + HSO₄⁻ (aq)


Under the fully ionization assumption the concentration of HSO4- is the same of the acid = 0.01 M


2) Second ionization
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<span>HSO₄⁻ (aq) ⇄ H⁺ + SO₄²⁻ with a Ka₂ = 0.012
</span>

<span>Do the mass balance:
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<span><span>        HSO₄⁻ (aq)        H⁺        SO₄²⁻</span>
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<span /><span /><span>        0.01 M  - x          x            x


</span><span>Ka₂ = [H⁺] [SO₄²⁻] / [HSO₄⁻]</span>
<span /><span>
=> Ka₂ = (x²) / (0.01 - x) = 0.012
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<span>3) Solve the equation:


</span><span>x² = 0.012(0.01 - x) = 0.00012 - 0.012x</span>
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<span>Using the quadratic formula: x = 0.00649
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<span>So, the requested concentratioN is [SO₄²⁻] = 0.00649M</span>

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You have a sample of 75.6 g of C3H8. How many moles of C3H8 are in the sample?
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The number of moles that are contained in the given mass of propane (C_3H_8 is 1.7143 moles.

<u>Given the following data:</u>

  • Mass of propane = 75.6 grams.

<u>Scientific data:</u>

  • The molar mass of propane = 44.1 g/mol.

To calculate the number of moles that are contained in the given mass of propane (C_3H_8):

<h3>How to calculate the moles of a compound.</h3>

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