What volume of 0.10 M H2SO4 must be added to 50ml of 0.10 M NAOH solution to make a solution in which the molarity H2SO4 is 0.050 M!?
What volume of 0.10 M H2SO4 must be added to 50ml of 0.10 M NAOH solution to make a solution in which the molarity H2SO4 is 0.050 M!?
First convert molarity to normality
N=M*basicity
As we know acid and base reacts with each so FOR base and acid reaction:
(N)(total volume)=(NaVa-NbVb)=(NbVb-NaVb)
where Na and Nb are the normality of the acid and base respectively, Va and Vb are the volume of acid and base respectively.
You can convert ml to litres but you want answer in ml so its easier you don't convert it.
Let volume of acid be x
Total volume(V)=50+x
Final normality(N)=0.05*2 [since basicity of H2SO4=2]
Initial normality of acid(Na)=0.1*2 [since basicity of H2SO4=2]
Initial normality of base(Nb)=0.1*1 [since basicity of NaCl=1]
NV=(NaVa-NbVb)
0.05*2*(50+x)= 0.1*2*x-0.1*1*50
0.05*2*(50+x)=0.1(2*x-50)
50+x=2x-50
x=100 ml
Thus VoLUME required = 100ml
First convert molarity to normality
N=M*basicity
As we know acid and base reacts with each so FOR base and acid reaction:
(N)(total volume)=(NaVa-NbVb)=(NbVb-NaVb)
where Na and Nb are the normality of the acid and base respectively, Va and Vb are the volume of acid and base respectively.
You can convert ml to litres but you want answer in ml so its easier you don't convert it.
Let volume of acid be x
Total volume(V)=50+x
Final normality(N)=0.05*2 [since basicity of H2SO4=2]
Initial normality of acid(Na)=0.1*2 [since basicity of H2SO4=2]
Initial normality of base(Nb)=0.1*1 [since basicity of NaCl=1]
NV=(NaVa-NbVb)
0.05*2*(50+x)= 0.1*2*x-0.1*1*50
0.05*2*(50+x)=0.1(2*x-50)
50+x=2x-50
x=100 ml
Thus VoLUME required = 100ml
