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


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 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).

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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


Chapter 13 / Lesson 2

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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