H3PO4(aq)+3KOH(aq)→3H2O(l)+K3PO4(aq)
A solution of 0.244M KOH is used to titrate 10.5mL of a 0.196M H3PO4 solution. What volume, in milliliters, of the KOH solution is required?
3KOH + H3PO4 ==> K3PO4 + 3H2O
millimiles H3PO4 = mL x M = 10.5 mL x 0.196 M = 53.6
Convert to millimiles KOH needed. Done the same way as the previous problem.
Then M KOH = millimoles KOH/mL KOH. You know M and you know millimoles. You can solve for mL.
Post your work if you get stuck.
m1v1=m2v2
m1=0.196M
v1=10.5ml
m2=0.244M
v2=??
0.196×10.5= 0.244×v2
2.058=0.244v2
v2=2.058/0.244
v2=8.434ml
therefore, 8.434ml of KOH solution is required