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3 years ago

What is the complete ionic equation for this reaction?

Chemistry

1 answer:

geniusboy [140]3 years ago

5 0

Answer:

The answer is "Option D".

Explanation:

The entire ionic equation for all the substances, which are ionic compounds but are available in an aquatic is represented in the form with ions in the full ionic equation.

In the Net ionic equation, it doesn't have the particulate matter throughout the net ionic equations throughout the equations.

In the Spectator ions, it doesn't participate in interactions mostly on reaction and the material hand. From both sides, the very same ions are present.

The evenly balanced chemical formula is,

$2KOH (aq)+ H_2SO_4(aq) \longrightarrow 2H_2O(l) + K_2SO_4$

It is the separate organic compound that full ion formula will match the choice D.

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geniusboy [140]

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3 years ago

What does the law of conservation of energy imply?

zheka24 [161]

Answer:

B. That energy can only be converted between different forms

Explanation:

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2 years ago

Which is a proper description of chemical equilibrium?

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D) because both reactions are occurring at the same rate. They are not equal but their concentrations are constant.

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3 years ago

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3 years ago

What is the new concentration of a solution of CaSO3 if 10.0 mL of a 2.0 M CaSO3 solution is diluted to 100 ml?

kifflom [539]

Answer: The new concentration of a solution of $CaSO_{3}$ is 0.2 M 10.0 mL of a 2.0 M $CaSO_{3}$ solution is diluted to 100 mL.

Explanation:

Given: $V_{1}$ = 10.0 mL, $M_{1}$ = 2.0 M

$V_{2}$ = 100 mL, $M_{2}$ = ?

Formula used to calculate the new concentration is as follows.

$M_{1}V_{1} = M_{2}V_{2}$

Substitute the values into above formula as follows.

$M_{1}V_{1} = M_{2}V_{2}\\10.0 mL \times 2.0 M = M_{2} \times 100 mL\\M_{2} = 0.2 M$

Thus, we can conclude that the new concentration of a solution of $CaSO_{3}$ is 0.2 M 10.0 mL of a 2.0 M $CaSO_{3}$ solution is diluted to 100 mL.

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2 years ago