How much water is formed when 1.0 mol of #HCl# reacts completely with 1.0 mol of #NaOH#?

1 Answer
Edmund Liew
May 13, 2016

Assume that:
n = number of moles
m = mass of substance
M = molar mass

Looking at the equation:
#HCl + NaOH => H_2O + NaCl#.

Since all compounds in this reaction have 1 mole, it will not affect the number of moles (n).

If 1 mole of HCl or NaOH gives you 1 mole of #H_2O#, then the number of moles in #H_2O# is: [#1 -: 1 xx 1#] = 1 mole.

Now you have to find out the molar mass (M) of water (#H_2O#).
Before that, take note that you know what atoms are present in #H_2O# - in that case, hydrogen and oxygens are present.

Refer to your periodic table and you can see molar mass of (?) is:
Hydrogen = 1.0 g/mol
Oxygen = 16.0 g/mol

Therefore the molar mass (M) of #H_2O# is:
[#2 xx 1.0 + 1 xx 16.0#] = 18.0 g/mol.

Last step, find the mass (m) of water.
The formula of finding mass of substance (m) is:
#m = n xx M#.
The mass of #H_2O# is: [m = 1.0 moles #xx# 18.0 g/mol = 18.0 grams]

Therefore 18.0 grams of water is formed when 1 mole of HCl reacts completely with 1 mole of NaOH.

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