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ratelena [41]
3 years ago
5

An HCl solution has a concentration of 9.8 x 10-5 M. What is the pH of this solution

Chemistry
2 answers:
Vilka [71]3 years ago
8 0
C=9.8*10⁻⁵

pH=-lg[H⁺]

HCl = H⁺ + Cl⁻

[H⁺]=c

pH=-lg(9.8*10⁻⁵)=4.0

pH=4.0
Svetach [21]3 years ago
6 0

Answer:

pH of the given HCl solution is 4.0

Explanation:

<u>Given:</u>

Concentration of HCl solution = 9.8*10⁻⁵ M

<u>To determine:</u>

The pH of the solution

<u>Explanation:</u>

pH of a solution refers to the concentration of H+ ions which in turn reflects the acidity of the solution

pH is related to the H+ concentration as follows:

pH = -log[H+} \\\\For\ the \ given\ HCl\ solution\\\\pH = -log(9.8*10^{-5}) = 4.00

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The K w for water at 0 ∘ C is 0.12 × 10 − 14 M 2 . Calculate the pH of a neutral aqueous solution at 0 ∘ C . p H = Is a pH = 7.2
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Answer:

pH → 7.46

Explanation:

We begin with the autoionization of water. This equilibrium reaction is:

2H₂O  ⇄   H₃O⁺  +  OH⁻            Kw = 1×10⁻¹⁴         at 25°C

Kw = [H₃O⁺] . [OH⁻]

We do not consider [H₂O] in the expression for the constant.

[H₃O⁺] = [OH⁻] = √1×10⁻¹⁴   →  1×10⁻⁷ M

Kw depends on the temperature

0.12×10⁻¹⁴ = [H₃O⁺] . [OH⁻]  → [H₃O⁺] = [OH⁻]         at 0°C

√0.12×10⁻¹⁴ = [H₃O⁺] → 3.46×10⁻⁸ M

- log [H₃O⁺] = pH

pH = - log 3.46×10⁻⁸ → 7.46

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