Question

how many ml of 0.25 M NaOH solution are required to neutralize 45.00 ml of 0.37 M HCL

Answer 1

These types of questions involves the same steps:
1) Write the equation
NaOH + HCl --> H2O + NaCl
2) Find out how many moles of acid or base you have
n(HCl) = cV = 0.37M x 0.045L (make sure you use L and not ml since M means mol/L)
=0.0167 mol
3) Compare the molar ratio of acid to base in the formula to find out how many moles of acid or base you need.
Since mol(NaOH):mol(HCl) = 1:1 we need 0.0167 mol of NaOH to neutralise 0.0167 mol HCl.
4) substitute this value of n into n = cV to find the volume (or sometimes concentration)
Again, since n = cV, V = n/c = 0.0167mol/0.25mol/L = 0.067L or 67mL