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Alja [10]
3 years ago
15

Sugar is easily soluble in water and has a molar mass of 342.30 g/mol. What is the molar concentration of a 259.8 mL aqueous sol

ution prepared with 73.1 g of sugar?
Chemistry
1 answer:
DanielleElmas [232]3 years ago
5 0

Answer:

M=0.822M

Explanation:

Hello,

In this case, given the mathematical definition of molar concentration as the moles of solute divided by the liters of solution:

M=\frac{n}{V}

We can easily compute it by firstly computing the moles of sugar by using its molar mass:

n=73.1g*\frac{1mol}{342.30g} =0.214mol

After that, we compute the concentration by realizing 259.8 mL equals 0.2598 L:

M=\frac{0.214mol}{0.2598L}\\ \\M=0.822mol/L

Or just:

M=0.822M

Considering molar units as mol/L

Best regards.

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Which coefficient before potassium (K) balances this chemical equation?
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Read 2 more answers
.an open flask contains 0.200 mol of air. atmospheric pressure is 745 mmhg and room temperature is 68˚f. how many moles are pres
aleksklad [387]

<u>0.219 moles </u><u>moles are present in the flask when the </u><u>pressure </u><u>is 1.10 atm and the temperature is 33˚c.</u>

What is ideal gas constant ?

  • The ideal gas constant is calculated to be 8.314J/K⋅ mol when the pressure is in kPa.
  • The ideal gas law is a single equation which relates the pressure, volume, temperature, and number of moles of an ideal gas.
  • The combined gas law relates pressure, volume, and temperature of a gas.

We simple use this formula-

The basic formula is PV = nRT where. P = Pressure in atmospheres (atm) V = Volume in Liters (L) n =  of moles (mol) R = the Ideal Gas Law Constant.

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n = PV/RT = 1.1atm*4.992L/(0.08206Latm/molK * 306K)

n = 0.219 moles

Therefore, 0.219 moles moles are present in the flask when the pressure is 1.10 atm and the temperature is 33˚c.

Learn more about ideal gas constant

brainly.com/question/3961783

#SPJ4

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