Would you expect a difference in the mass of #"AgCl"# produced by the reaction depending on whether you used the #"1 M"# or #"0.1 M"# of #"NaCl"#? Give reasons for your answer.

There wouldn't be a difference in mass, right? would only require a greater volume of #"NaCl"#.

Answer 1

Well, that depends...

Here, it is important to always remember which reactant, if any, serves as a limiting reagent.

Assuming you are dealing with a reaction that is akin to this double-replacement reaction

#"AgNO"_ (3(aq)) + "NaCl"_ ((aq)) -> "AgCl"_ ((s)) darr + "NaNO"_ (3(aq))#

If sodium chloride is present in excess in both scenarios, then the mass of silver chloride generated by the reaction will not be affected by the concentration of the sodium chloride solution.

Put another way, you can add as many moles of sodium chloride as you like as long as the number of moles of silver nitrate is always less than the number of moles of the latter, since the former will always be the limiting reagent, i.e., figure out how many moles of silver chloride are produced by the reaction.

so long as you've

#"moles of AgNO"_3 " "< " ""moles of NaCl"#

The precise number of moles of sodium chloride you possess is irrelevant.

But if you've

#"moles of AgNO"_3 " "< " ""moles of NaCl in 1-M solution"#

and

#"moles of AgNO"_3 " "> " ""moles of NaCl in 0.1-M solution"#
then in the case of the #"0.1-M"# sodium chloride solution, silver nitrate will no longer be the limiting reagent and the number of moles of sodium chloride will determine the mass of silver chloride produced by the reaction.
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Answer 2

No, the mass of AgCl produced by the reaction would not be affected by whether 1 M or 0.1 M of NaCl is used. The mass of AgCl produced depends on the number of moles of AgCl formed, which is determined by the stoichiometry of the reaction and not the concentration of the NaCl solution. As long as there is sufficient Cl^- ions present in the reaction, the mass of AgCl produced will remain the same regardless of the concentration of the NaCl solution.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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