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babymother [125]
3 years ago
9

Which statement is true about a neutral solution? Its pH is less than 7. Its pH is greater than 7. It has the same concentration

of hydronium and hydroxide ions. It has a greater concentration of hydroxide ion than hydronium ions.
Chemistry
2 answers:
kumpel [21]3 years ago
7 0

Answer:

Option C It has the same concentration of hydronium and hydroxide ions is correct.

Explanation:

A neutral solution will have pH=7

and the concentration of hydronium ions and hydroixde ions is the same.

So, Option C It has the same concentration of hydronium and hydroxide ions

is correct.

katrin [286]3 years ago
6 0

Answer: Option (c) is the correct answer.

Explanation:

A solution whose pH is less than 7 is known as an acidic solution. In this solution, concentration of hydrogen ions is more than hydroxide ions.

Whereas a solution whose pH is more than 7 is known as a basic solution. In this solution, concentration of hydroxide ions is more than hydrogen ions.

On the other hand, when pH of a solution is equal to 7 then the solution will be known as neutral solution. That is, the concentration of both hydrogen and hydroxide ions is same in a neutral solution.

Thus, we can conclude that the statement it has the same concentration of hydronium and hydroxide ions, is true about a neutral solution.

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A solution of 0.0470 M HCl is used to titrate 26.0 mL of an ammonia solution of unknown concentration. The equivalence point is
DanielleElmas [232]

The pH at equivalence point is 12.46

At equivalence point, number of moles of acid, n equals number of moles of base, n'

So, n = n'

CV = C'V' where

  • C = concentration of acid (HCl) = 0.0470 M,
  • V = volume of acid = 16.0 mL,
  • C' = concentration of base (ammonia solution) and
  • V' = volume of base = 26.0 mL.
<h3>Concentration of ammonia solution</h3>

Making C' subject of the formula, we have

C' = CV/V'

Substituting the values of the variables into the equation, we have

C' = CV/V'

C' = 0.0470 M × 16.0 mL/26.0 mL

C' = 0.752 MmL/26.0 mL

C' = 0.0289 M

<h3>The concentration of acid at equivalence point</h3>

We know that the ion-product of water Kw is

Kw = [H⁺][OH⁻] =  where

  • [H⁺] = concentration of HCl at equivalence point,
  • [OH⁻] = C' = concentration of ammonia solution = 0.0289 M and
  • Kw = 1.01 × 10⁻¹⁴

Making [H⁺] subject of the formula, we have

[H⁺} = Kw/[OH⁻]

[H⁺] = 1.01 × 10⁻¹⁴/0.0289

[H⁺] = 34.95 × 10⁻¹⁴

[H⁺] = 3.495 × 10⁻¹³

<h3>pH at equivalence point</h3>

Since pH = -㏒[H⁺]

pH = -㏒[3.495 × 10⁻¹³]

pH = -㏒[3.495] + (-㏒10⁻¹³)

pH = -㏒[3.495] + [-13(-㏒10)]

pH = 13 - 0.5434

pH = 12.4566

pH ≅ 12.46

So, the pH at equivalence point is 12.46

Learn more about pH at equivalence point here:

brainly.com/question/25487920

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