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kifflom [539]
2 years ago
13

A solution has a pH of 11.75. Calculate the [H:0*] of the solution

Chemistry
1 answer:
Savatey [412]2 years ago
7 0

The [H₃0⁺] of the solution : 1.778  x 10⁻¹² M

<h3>Further explanation  </h3>

pH is the degree of acidity of a solution that depends on the concentration of H⁺ ions. The greater the value the more acidic the solution and the smaller the pH.  

pH = - log [H⁺]  

So that the two quantities between pH and [H⁺] are inversely proportional because they are associated with negative values.  

A solution whose value is different by n has a difference in the concentration of H⁺ ion of 10ⁿ.  

pH of solution = 11.75

the [H₃0⁺] of the solution :

\tt pH=-log[H_3O^+]\\\\11.75=-log[H_3O^+]\\\\(H_3O^+]=10^{-11.75}=1.778\times 10^{-12}

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The volume (in mL) of 0.242 M NaOH solution needed for the titration reaction is 39.44 mL

<h3>Balanced equation </h3>

CH₃CH₂COOH + NaOH —> CH₃CH₂COONa + H₂O

From the balanced equation above,

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<h3>How to determine the volume of NaOH</h3>
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MaVa / MbVb = nA / nB

(0.204 × 46.79) / (0.242 × Vb) = 1

Cross multiply

0.242 × Vb = 0.204 × 46.79

Divide both side by 0.242

Vb = (0.204 × 46.79) / 0.242

Vb = 39.44 mL

Thus, the volume of NaOH needed for the reaction is 39.44 mL

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brainly.com/question/14356286

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No

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