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2 years ago

A solution has a [H+] of 0.20 M. Find the pH of this solution.

Chemistry

1 answer:

Rus_ich [418]2 years ago

4 0

The pH of this solution : 0.699

<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.

A solution has a [H+] of 0.20 M, so [H⁺]=0.2

$\tt pH=-log[H^+]\\\\pH=-log[0.2]\\\\pH=1-log~2\\\\pH=0.699$

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2 years ago

Two different bromide solutions are mixed with each other: Solution 1 is an aqueous solution of 4.85 g aluminum bromidein 150. m

erma4kov [3.2K]

Answer:

M=0.380 M.

Explanation:

Hello there!

In this case, given those two solutions of aluminum bromide and zinc bromide, it is firstly necessary to compute the moles of bromide ions in each solution as shown below:

$n_{Br^-}^{in\ AlBr_3}=4.85 gAlBr_3*\frac{1molAlBr_3}{266.69gAlBr_3}*\frac{3molBr^-}{1molAlBr_3} =0.05456molBr^-\\\\n_{Br^-}^{in\ ZnBr_2}=7.75gZnBr_2*\frac{1molZnBr_2}{225.22gZnBr_2}*\frac{2molBr^-}{1molZnBr_2} =0.06882molBr^-$

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2 years ago

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<h3>What is electrolytic solution?</h3>

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Learn more about Electrolytic solutions here: brainly.com/question/14654936

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