A salt crystal has a mass of 0.15mg. How many NaCl formula units does it contains?

Answer 1

We need (i) the molar quantity of #"sodium chloride"#........

#"Number of moles"# #=# #"Mass"/"Molar mass"#
#=# #(0.15xx10^-3*g)/(58.44*g*mol^-1)# #=# #"?? moles"#
And (ii) we need the number of sodium chloride units. Now it is a fact that #"Avogadro's number, "N_A# #-=# #6.022xx10^23*mol^-1#

Thus, to get the number of units of the sodium chloride formula, we multiply the number of moles by "Avogadro's number":

#(0.15xx10^-3*g)/(58.44*g*mol^-1)xx6.022xx10^23*mol^-1#, and we get the answer as a number, as required.
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Answer 2

In order to find the number of NaCl formula units in the salt crystal, you must first calculate the number of moles of NaCl using its molar mass (58.44 g/mol), and then convert moles to formula units using Avogadro's number (6.022 × 10^23 formula units/mol). First, convert the mass of the salt crystal from milligrams to grams: 0.15 mg = 0.15 × 10^-3 g. Next, calculate the number of moles of NaCl: moles = mass / molar mass moles = 0.15 × 10^-3 g / 58.44 g/mol. Lastly, use Avogadro's number to find the number of formula units: formula units = moles × Avogadro's number

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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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