A 300 mL solution of 0.0500 M HCl is titrated with 1.00 M KOH. How many mL of the KOH solution will be needed to reach the equivalence point of this titration?
A.5 mL
B.10 mL
C.50 mL
D20 mL
E15 mL
The answer i got was E. 15ml
2 answers
Can you explain to me why?
HCl + KOH ==> KCl + H2O
mols HCl = M x L = 0.015
mols KOH = the same since 1 mol HCl reacts with 1 mol KOH = 0.015
Then M KOH = mols KOH/ L KOH. You know M and mols, solve for L.
1.00 = 0.015/L and L = 0.015/1.00 = 0.015L. Convert that to mL for 15 mL.
mols HCl = M x L = 0.015
mols KOH = the same since 1 mol HCl reacts with 1 mol KOH = 0.015
Then M KOH = mols KOH/ L KOH. You know M and mols, solve for L.
1.00 = 0.015/L and L = 0.015/1.00 = 0.015L. Convert that to mL for 15 mL.
4 answers