Answer :
Certainly! Let's solve the problem step-by-step.
We need to calculate the number of moles of [tex]\( \text{Na}^+ \)[/tex] ions present in 1.64 liters of a 0.272 M [tex]\( \text{NaNO}_4 \)[/tex] solution.
Step 1: Understand the Problem
- We have a solution of sodium nitrate ([tex]\( \text{NaNO}_4 \)[/tex]).
- The concentration of this solution is given as 0.272 M, which means 0.272 moles of [tex]\( \text{NaNO}_4 \)[/tex] are present in 1 liter of solution.
- We have 1.64 liters of this solution.
Step 2: Calculate the Moles of [tex]\( \text{NaNO}_4 \)[/tex]
- To find the moles of [tex]\( \text{NaNO}_4 \)[/tex] in 1.64 liters, use the formula:
[tex]\[
\text{Moles of NaNO}_4 = \text{Molarity} \times \text{Volume in liters}
\][/tex]
[tex]\[
\text{Moles of NaNO}_4 = 0.272 \, \text{mol/L} \times 1.64 \, \text{L}
\][/tex]
Step 3: Calculate the Moles of [tex]\( \text{Na}^+ \)[/tex] Ions
- In the compound [tex]\( \text{NaNO}_4 \)[/tex], each formula unit provides one [tex]\( \text{Na}^+ \)[/tex] ion.
- Therefore, the moles of [tex]\( \text{Na}^+ \)[/tex] ions will be the same as the moles of [tex]\( \text{NaNO}_4 \)[/tex].
Upon calculating, you find that there are approximately 0.44608 moles of [tex]\( \text{Na}^+ \)[/tex] ions in the solution.
This is the number of moles of [tex]\( \text{Na}^+ \)[/tex] ions present in the 1.64 liters of the [tex]\( \text{NaNO}_4 \)[/tex] solution.
We need to calculate the number of moles of [tex]\( \text{Na}^+ \)[/tex] ions present in 1.64 liters of a 0.272 M [tex]\( \text{NaNO}_4 \)[/tex] solution.
Step 1: Understand the Problem
- We have a solution of sodium nitrate ([tex]\( \text{NaNO}_4 \)[/tex]).
- The concentration of this solution is given as 0.272 M, which means 0.272 moles of [tex]\( \text{NaNO}_4 \)[/tex] are present in 1 liter of solution.
- We have 1.64 liters of this solution.
Step 2: Calculate the Moles of [tex]\( \text{NaNO}_4 \)[/tex]
- To find the moles of [tex]\( \text{NaNO}_4 \)[/tex] in 1.64 liters, use the formula:
[tex]\[
\text{Moles of NaNO}_4 = \text{Molarity} \times \text{Volume in liters}
\][/tex]
[tex]\[
\text{Moles of NaNO}_4 = 0.272 \, \text{mol/L} \times 1.64 \, \text{L}
\][/tex]
Step 3: Calculate the Moles of [tex]\( \text{Na}^+ \)[/tex] Ions
- In the compound [tex]\( \text{NaNO}_4 \)[/tex], each formula unit provides one [tex]\( \text{Na}^+ \)[/tex] ion.
- Therefore, the moles of [tex]\( \text{Na}^+ \)[/tex] ions will be the same as the moles of [tex]\( \text{NaNO}_4 \)[/tex].
Upon calculating, you find that there are approximately 0.44608 moles of [tex]\( \text{Na}^+ \)[/tex] ions in the solution.
This is the number of moles of [tex]\( \text{Na}^+ \)[/tex] ions present in the 1.64 liters of the [tex]\( \text{NaNO}_4 \)[/tex] solution.
