Question

What volume of a 1.0 M HCl is required to completely neutralize 25.0 ml of a 1.0 M KOH?

Answer 1

To completely neutralize the 25.0 mL of 1.0 M KOH, you would need 25.0 mL of 1.0 M HCl.

Step-by-step explanation:

To completely neutralize the 25.0 mL of 1.0 M KOH, we need to use the concept of stoichiometry and the balanced equation for the reaction between HCl and KOH. The balanced equation is:

HCl + KOH -> KCl + H2O

From the equation, we can see that the stoichiometric ratio between HCl and KOH is 1:1. Since the concentrations of HCl and KOH are the same (1.0 M), and the volume of the KOH solution is given as 25.0 mL, the volume of 1.0 M HCl required to completely neutralize the KOH is also 25.0 mL.

Answer 2

x 0,025
HCl+KOH--> KCl + H2O
1 1


c=1M
V=25ml=0,025l ( you need the volume to be in l)
c = n/V
n=c*V
n=1*0,025=0,025 m KOH


x=0,025m
c=1 M
V=n/c
V=0,025/1=0,025l=25ml HCl