Question

How many moles of solute particles are present in 4.98 mL of 0.72 M (NH4)2SO4? When you have your answer, take the LOG (base 10) of your answer and enter it with 2 decimal places.

Answer 1

Answer: The number of moles of ammonium sulfate is 0.0036 moles and its logarithmic value is -2.44

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$

Molarity of ammonium sulfate solution = 0.72 M

Volume of solution = 4.98 mL

Putting values in above equation, we get:

$0.72M=\frac{\text{Moles of ammonium sulfate}\times 1000}{4.98mL}\\\\\text{Moles of ammonium sulfate}=0.0036mol$

Taking the log (base 10) of the calculated moles of ammonium sulfate we get:

$\log_{10}(0.0036)=-2.44$

Hence, the number of moles of ammonium sulfate is 0.0036 moles and its logarithmic value is -2.44