Find the pH of resultant solution when 100ml of 0.005MH2SO4 at 25oC is diluted to 1000ml. What is the amount of NaOH required to be dissolved in 500ml to exactly neutralize the above solution?
A
4g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
4×10−2g
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
40g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
0.4g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution
The correct option is B4×10−2g Number of moles of H+ in 0.005MH2SO4=0.005×2×0.1=0.001moles
After dilution concentration of H+ ions= 0.0011=0.001mole/l
pH=−log[0.001]=3
Amount of NaOH required to neutralize the solution= 0.001mole