How many moles of water form when 40.0 ml of .800 M HNO3 solution is completely neutralized by NaOH?
To find the number of moles of water formed when the HNO3 solution is neutralized by NaOH, we need to first determine the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between HNO3 and NaOH is:
HNO3 + NaOH → NaNO3 + H2O
From the balanced chemical equation, we can see that for every 1 mole of HNO3 reacted, 1 mole of water is formed.
In order to determine the number of moles of water formed, we need to know the number of moles of HNO3 that reacted. To find this, we can use the equation:
moles = concentration (M) × volume (L)
Given that the concentration of the HNO3 solution is 0.800 M and the volume is 40.0 mL (which needs to be converted to liters), we can calculate the number of moles of HNO3:
moles of HNO3 = 0.800 M × 0.040 L = 0.032 mol
Since the molar ratio between HNO3 and H2O is 1:1, the number of moles of water formed will also be 0.032 mol.
Therefore, when 40.0 mL of 0.800 M HNO3 solution is completely neutralized by NaOH, 0.032 moles of water are formed.