8.00g of NaOH are dissolved in water to make 3.00 L of solution. What is the concentration of hydronium ions, , in this solution?
this was wrong, thanks
To find the concentration of hydronium ions (H3O+) in the solution, we need to understand the relationship between sodium hydroxide (NaOH) and hydronium ions in water.
When NaOH is dissolved in water, it dissociates into sodium ions (Na+) and hydroxide ions (OH-). In water, these hydroxide ions can combine with water molecules to form hydronium ions. The balanced equation for this reaction is:
NaOH + H2O -> Na+ + OH- + H2O -> Na+ + H3O+ + OH-
Note that one water molecule is used in both the dissociation of NaOH into Na+ and OH- and the formation of hydronium ions. Thus, the concentration of hydronium ions can be considered equal to the concentration of hydroxide ions.
Given that 8.00g of NaOH are dissolved in 3.00 L of solution, we can calculate the concentration of hydroxide ions by first finding the number of moles of NaOH and then dividing it by the volume of the solution.
Step 1: Calculate the number of moles of NaOH.
The molar mass of NaOH is:
Na: 22.99 g/mol
O: 16.00 g/mol
H: 1.01 g/mol
NaOH: 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol
To find the number of moles, divide the mass of NaOH (8.00 g) by its molar mass (40.00 g/mol):
moles of NaOH = 8.00 g / 40.00 g/mol = 0.20 mol
Step 2: Calculate the concentration of hydroxide ions.
Since NaOH is a strong base, it completely dissociates in water. This means that for every one mole of NaOH, we get one mole of hydroxide ions.
The volume of the solution is 3.00 L.
Concentration (in mol/L) = moles of solute / volume of solution
Concentration of OH- ions = 0.20 mol / 3.00 L = 0.067 M
Since the concentration of hydroxide ions is equal to the concentration of hydronium ions in this case, the concentration of hydronium ions in the solution is also 0.067 M.
Molarity = # moles/L
moles NaOH = 8.00/molar mass NaOH.
L = 3.00.
You work it out.