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3 years ago

What is the pH of a 5.4 x 10-3 M HCl solution?A. 2.3B. 3.3C. 3.7D. 11.7

Chemistry

1 answer:

quester [9]3 years ago

8 0

Answer: A. 2.3

Explanation:

pH of a solution is given by the following mathematical expression;

pH = - Log [ H+]

= -Log [ 5.4 x 10-3]

= 3 - 0.7324

pH = 2.27 aprrox 2.3

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The first thing that you need to do here is to calculate the theoretical yield of the reaction, i.e. what you get if the reaction has a

100

yield.

The balanced chemical equation

(

)

(

)

→

(

)

tells you that every

mole of nitrogen gas that takes part in the reaction will consume

moles of hydrogen gas and produce

mole of ammonia.

In your case, you know that

mole of nitrogen gas reacts with

mole of hydrogen gas. Since you don't have enough hydrogen gas to ensure that all the moles of nitrogen gas can react

what you need

3 moles H (sub 2)

what you have

1 mole H (sub2)

you can say that hydrogen gas will act as a limiting reagent, i.e. it will be completely consumed before all the moles of nitrogen gas will get the chance to take part in the reaction.

So, the reaction will consume

mole of hydrogen gas and produce

mole H

⋅

2 moles NH

moles H

0.667 moles NH

100

yield. This represents the reaction's theoretical yield.

Now, you know that the reaction produced

0.50

moles of ammonia. This represents the reaction's actual yield.

In order to find the percent yield, you need to figure out how many moles of ammonia are actually produced for every

100

moles of ammonia that could theoretically be produced.

You know that

0.667

moles will produce

0.50

moles, so you can say that

100

moles NH

in theory

⋅

0.50 moles NH

actual

0.667

moles NH

in theory

75 moles NH

actual

Therefore, you can say that the reaction has a percent yield equal to

% yield = 75%

−−−−−−−−−−−−−

or 75 moles NH sub3

I'll leave the answer rounded to two sig figs.

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3 years ago

What is the pH of a 5.4 x 10-3 M HCl solution?A. 2.3B. 3.3C. 3.7D. 11.7​

What is the pH of a 5.4 x 10-3 M HCl solution?A. 2.3B. 3.3C. 3.7D. 11.7