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12345 [234]
2 years ago
13

Score! You manage to find a bottle of bromothymol blue and a few extra beakers. You take one of the empty beakers and add some o

f the first unlabeled solution and some indicator. The color changes to yellow. You then add some solution from the other unlabeled flask into this beaker and see the color change to blue. What are the identities of each unlabeled solution
Chemistry
1 answer:
mamaluj [8]2 years ago
6 0

Answer:

You manage to find a bottle of bromothymol blue and a few extra beakers. You take one of the empty beakers and add some of the first unlabeled solution and some indicator.

The color changes to yellow.

You then add some solution from the other unlabeled flask into this beaker and see the color change to blue.

What are the identities of each unlabeled solution?

Explanation:

Bromothymol blue is a dye and it is used as an indicator.

It is used as a pH indicator.

In acids, it becomes yellow n in color.

In bases, it turns blue.

You take one of the empty beakers and add some of the first unlabeled solution and some indicator. The color changes to yellow.

That means the unlabeled solution is an acid.

You then add some solution from the other unlabeled flask into this beaker and see the color change to blue.

It is a basic solution.

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E_{eV} = E_{J} X (6.241 X 10^{18})

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So, on substituting we get,
E_{eV} = 3.2 X 10^{-19}  X  (6.241 X 10^{18} )


E_{eV} = 1.99 eV so, it can be rounded off to 2.00 eV.
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3 years ago
What is the value of δg°' (or, to put it another way, the cost) when 2nadp+ and 2h2o are converted to 2nadph plus 2h+ plus o2?
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3 years ago
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A balloon contains 5 L of oxygen at a pressure of 90 kPa. How much oxygen will the balloon contain if the pressure is lowered to
laila [671]
Answer is: volume will be 6,7 L.
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3 years ago
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3 years ago
A liquid has an empirical formula CCl2, and a boiling point of 1 21 oC. When vapourised, the gaseous compound has a density of 4
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Based on the data given, the molar mass of the gas is 165.5 g/mol while the molecular weight of the gas is 165.5 amu

<h3>How can molar mass of a gas be obtained from density, temperature and pressure?</h3>

The molar mass of a gas can be obtained from density, temperature and pressure using the formula below:

  • molar mass = density × molar gas constant × temperature/pressure

Molar gas constant, R = R = 0.082 L.atm/mol/K.

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Then, molecular weight of the gas = 165.5 amu

Therefore, the molar mass of the gas is 165.5 g/mol while the molecular weight of the gas is 165.5 amu

Learn more about molar mass of a gas at: brainly.com/question/26215522

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