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Georgia [21]
3 years ago
12

What is the [H3O+] of a solution with a pH of 2.56? 2.56 M, 2.75 x 10-3 M, 363 M, or -0.408 M

Chemistry
2 answers:
mote1985 [20]3 years ago
8 0
PH=2.56

pH=-lg[H₃O⁺]

[H₃O⁺]=10^(-pH)

[H₃O⁺]=10⁻²·⁵⁶=0.00275=2.75×10⁻³ mol/L

2.75×10⁻³ M

bonufazy [111]3 years ago
8 0

Answer:

The concentration of hydronium ions in solution is 2.75\times 10^{-3} M.

Explanation:

The pH of the solution is defined as negative logarithm of hydronium ions concentration in a solution. Mathematically written as:

pH=-\log[H_3O^+]

Given, the pH of the solution = 2.56

2.56=-\log[H_3O^+]

[H_3O^+]=0.002754 M=2.75\times 10^{-3} M

The concentration of hydronium ions in solution is 2.75\times 10^{-3} M.

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Balanced equation : C. CH₄ + 4Cl₂⇒  CCl₄+ 4HCl

<h3>Further explanation  </h3>

Equalization of chemical reactions can be done using variables. Steps in equalizing the reaction equation:  

1. gives a coefficient on substances involved in the equation of reaction such as a, b, or c, etc.  

2. make an equation based on the similarity of the number of atoms where the number of atoms = coefficient × index (subscript) between reactant and product  

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Reaction

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  • Give coefficient :

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Answer:

Explanation:

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