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larisa86 [58]
3 years ago
7

A chemist prepares a solution by adding 258 mg of K2Cr2O7 (MW = 294.19 g/mol ) to a volumetric flask, and then adding water unti

l the total volume of the contents of the flask reaches the calibration line that indicates 500 mLmL. Determine the molarity of the prepared solution.
Chemistry
1 answer:
Maksim231197 [3]3 years ago
3 0

Answer: Molarity of the prepared solution is 1.75\times 10^{-3}mole/L

Explanation:

Molarity is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n\times 1000}{V_s}

where,

n= moles of solute

V_s = volume of solution in ml = 500 ml

moles of solute =\frac{\text {given mass}}{\text {molar mass}}=\frac{0.258g}{294.19g/mol}=8.77\times 10^{-4}mol

Now put all the given values in the formula of molarity, we get

Molarity=\frac{8.77\times 10^{-4}moles\times 1000}{500ml}=1.75\times 10^{-3}mole/L

Thus molarity of the prepared solution is 1.75\times 10^{-3}mole/L

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