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You have 26.44 ml of 1.83 M HCl in a beaker. You dilute this acid with 40.08 ml of water. When...

Question:

You have {eq}\rm 26.44\ ml {/eq} of {eq}\rm 1.83\ M\ HCl {/eq} in a beaker. You dilute this acid with {eq}\rm 40.08\ ml {/eq} of water. When you analyze the solution you find that the number of moles of {eq}\rm HCl {/eq} in the new solution is {eq}\rm \_\_\_\_\ {/eq}.

Moles:

Moles are a convenient way of counting large numbers of any quantity. Typically, moles are used in chemistry to count atoms and molecules. One mole is equal to {eq}\displaystyle 6.022\ \times\ 10^{23} {/eq} of any given quantity. Typically, the equivalent mass of one mole of most substances is measurable using everyday weighing scales (that is, typical molar masses are in grams per mole).

Answer and Explanation:

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When we add water we don't change the overall number of moles of HCl in the solution because no extra HCl is added or removed.

This means we can...

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Concentration of Solutions: Definition & Levels

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Chapter 13 / Lesson 2
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Learn the dilute and concentrated solution definition. Compare and contrast dilute vs concentrated solution examples and see how a solution changes physically and chemically as it goes from dilute to concentrate.


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