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Crazy boy [7]
3 years ago
11

Suppose 7.05 g of zinc iodide is dissolved in 150. mL of a 0.20M aqueous solution of potassium carbonate. Calculate the final mo

larity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Round your answer to 3 significant digits.
Chemistry
1 answer:
sasho [114]3 years ago
4 0

Answer:

M=0.294M

Explanation:

Hello!

In this case, since the molarity of the iodide ion is computed by dividing the moles of iodide ions by the volume of solution in liters (0.150 L), we first need to compute the moles of zinc iodide (ZnI2) by using its molar mass and then using a mole ratio of 1 mol of zinc iodide to 2 mol of iodide ion:

n_{I^-}=7.05gZnI_2*\frac{1molZnI_2}{319.22 gZnI_2}*\frac{2molI^-}{1molZnI_2}=0.0442molI^-

Therefore, the resulting molarity turns out:

M=\frac{0.0442molI^-}{0.150L} \\\\M=0.294M

Best regards!

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4 0
2 years ago
4. which answer below is the formula mass of a water molecule?
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True or False - Changing the temperature will not affect the pressure of the mixture?
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If you needed to make 100 mL of a 0.2 M fruit drink solution from the 1.0 M fruit drink solution, how would you do it? (Hint: Us
grigory [225]

Answer:

We take 20.0 mL of the 1.0 M fruit drink solution and then add 80.0 mL of water to  make 100 mL of a 0.2 M fruit drink solution.

Explanation:

  • Using the rule that: the no. of millimoles of a solution before dilution is equal to the no. of millimoles of the solution after the dilution.

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<em>∴ V before dilution = (MV) after dilution / M before dilution </em>= (0.2 M)(100 mL) / (1.0 M) = <em>20.0 mL.</em>

<em>So, we take 20.0 mL of the 1.0 M fruit drink solution and then add 80.0 mL of water to  make 100 mL of a 0.2 M fruit drink solution.</em>

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