To calculate the mass of silver(II) oxide added to the flask, we first need to convert the concentration of the solution from mmol/L to mol/L.

1. Convert the concentration from mmol/L to mol/L:
9.81 x 10^-5 mmol/L = 9.81 x 10^-8 mol/L

2. Convert the volume from mL to L:
405.0 mL = 0.405 L

3. Use the formula for calculating the amount of substance (n) in moles:
n = concentration (mol/L) x volume (L)
n = 9.81 x 10^-8 mol/L x 0.405 L = 3.98 x 10^-8 mol

4. The molar mass of silver(II) oxide (AgO) is approximately 231.74 g/mol. Convert this to µg/mol:
231.74 g/mol = 231.74 x 10^6 µg/mol

5. Calculate the mass (m) in micrograms:
m = amount of substance (mol) x molar mass (µg/mol)
m = 3.98 x 10^-8 mol x 231.74 x 10^6 µg/mol = 9.23 µg

So, the chemist has added approximately 9.23 µg of silver(II) oxide to the flask. However, we need to round this to 2 significant digits, so the final answer is 9.2 µg.

Question

To calculate the mass of silver(II) oxide added to the flask, we first need to convert the concentration of the solution from mmol/L to mol/L.

1. Convert the concentration from mmol/L to mol/L:
   9.81 x 10^-5 mmol/L = 9.81 x 10^-8 mol/L

2. Convert the volume from mL to L:
   405.0 mL = 0.405 L

3. Use the formula for calculating the amount of substance (n) in moles:
   n = concentration (mol/L) x volume (L)
   n = 9.81 x 10^-8 mol/L x 0.405 L = 3.98 x 10^-8 mol

4. The molar mass of silver(II) oxide (AgO) is approximately 231.74 g/mol. Convert this to µg/mol:
   231.74 g/mol = 231.74 x 10^6 µg/mol

5. Calculate the mass (m) in micrograms:
   m = amount of substance (mol) x molar mass (µg/mol)
   m = 3.98 x 10^-8 mol x 231.74 x 10^6 µg/mol = 9.23 µg

So, the chemist has added approximately 9.23 µg of silver(II) oxide to the flask. However, we need to round this to 2 significant digits, so the final answer is 9.2 µg.

Knowee AI · Accepted Answer

To calculate the mass of silver(II) oxide added to the flask, we first need to convert the concentration of the solution from mmol/L to mol/L.

1. Convert the concentration from mmol/L to mol/L:
   9.81 x 10^-5 mmol/L = 9.81 x 10^-8 mol/L

2. Convert the volume from mL to L:
   405.0 mL = 0.405 L

3. Use the formula for calculating the amount of substance (n) in moles:
   n = concentration (mol/L) x volume (L)
   n = 9.81 x 10^-8 mol/L x 0.405 L = 3.98 x 10^-8 mol

4. The molar mass of silver(II) oxide (AgO) is approximately 231.74 g/mol. Convert this to µg/mol:
   231.74 g/mol = 231.74 x 10^6 µg/mol

5. Calculate the mass (m) in micrograms:
   m = amount of substance (mol) x molar mass (µg/mol)
   m = 3.98 x 10^-8 mol x 231.74 x 10^6 µg/mol = 9.23 µg

So, the chemist has added approximately 9.23 µg of silver(II) oxide to the flask. However, we need to round this to 2 significant digits, so the final answer is 9.2 µg.

A chemist adds 405.0mL of a ×9.810−5/mmolL silver(II) oxide AgO solution to a reaction flask. Calculate the mass in micrograms of silver(II) oxide the chemist has added to the flask. Round your answer to 2 significant digits.

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