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kiruha [24]
1 year ago
8

Calculate the ph of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions.

Chemistry
1 answer:
Makovka662 [10]1 year ago
8 0

The pH of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions is 13.5.

<h3>What is pH? </h3>

pH is defined as the concentration of the hydrogen bond which is released or gained by the species in the solution which depicts the acidity and basicity of the solution.

<h3>What is pOH? </h3>

pOH is defined as the concentration of the hydronium ion present in solution.

pOH value is inversely proportional to the value of pH.

pH value increases, pOH value decreases and vice versa.

Given,

Total H+ ions = 2.95 ×10^(-12)M

<h3>Calculation of pH</h3>

pH = -log[H+]

By substituting the value of H+ ion in given equation

= log(2.95× 10^(-12) )

= 13.5

Thus we find that the pH of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions is 13.5.

learn more about pH:

brainly.com/question/12942138

#SPJ4

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If a block has the mass of 15.00 grams and measurements of 5.00cm by 3.00cm by 2.00cm what is the volume of the block?
Natalija [7]

Answer:

Volume = 30cm³

Explanation:

A block is a geometrical figure and its volume, -look at the figure-, follows the equation:

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2 years ago
At what temperature (in C) will a sample of gas occupy 91.3 L if it occupies 45.0 L at 70.0°C? Assume constant pressure.)
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Solution is here,

for initial case,

temperature(T1)=70°C=70+ 273=343K

vloume( V1) =45 L

for final case,

temperature( T2)=?

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at constant pressure,

V1/V2 = T1/T2

or, 45/91.3 = 343/ T2

or, T2= (343×91.3)/45

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