What is the pH of the final solution if 4.0g of sodium hydroxide is mixed with 50ml of 2.0*10^-2 M H2SO4?
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Mole = concentration x volume
mole of NaOH = 50ml x 0.2 = 10.0
mole of HCl = 50ml x 0.4= 20.0
10 mole of NaOH exactly neutralized by 10 mole of HCl.
NaOH + HCl = NaCl + H2O
that is 20 -10 = 10 HCl mole
Con of H+ = no of mole of H+ / total volume of solution (50+50 ml = 100 ml)
= 10/100 = 0.1
HOPE IT HELPS YOU
mole of NaOH = 50ml x 0.2 = 10.0
mole of HCl = 50ml x 0.4= 20.0
10 mole of NaOH exactly neutralized by 10 mole of HCl.
NaOH + HCl = NaCl + H2O
that is 20 -10 = 10 HCl mole
Con of H+ = no of mole of H+ / total volume of solution (50+50 ml = 100 ml)
= 10/100 = 0.1
HOPE IT HELPS YOU
anshika160:
yss it should be further i dont know
oh okay. thank you
ohkk no problem
what about this one. 6.3*10^21 molecules of NH3 is how many moles of ammonia
No actually I figured out that one.
I really need help with this one please. 5.2*10^5 HCl molecules in 175ml of water will have what pH.
sorry dear this i dont know
thats okay thank you for everything else
no problem but im feeling so sorry for this question
That's okay!
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