A 15.7mL sample of HNO3 reacts to neutralize 27.7mL of 0.187M KOH solution. What is the molarity of the HNO3 solution?
HNO3 + KOH ==> KNO3 + HOH
mols KOH = L x M = 0.0277 x 0.187 = ??
mols HNO3 = mols KOH (1 mol reacts with 1 mol).
mols HNO3 = L x M
You have mols HNO3 and L, solve for M.
Check my thinking. Check my arithmetic.
I lost you on this one, I got a little confused on the 3rd step.
mols = L x M
mols KOH = 0.0277L x 0.187M = 0.00518 mols KOH.
The equation is
HNO3 + KOH ==> KNO3 + HOH
The equation shows 1 mol HNO3 reacts with 1 mol KOH; therefore, 0.00518 mols KOH requires 0.00518 mol HNO3.
Then mols HNO3 = L x M
0.00518 mol HNO3 = L x M
0.00518 mol HNO3 = 0.0157 L x M/
Solve for M.
Check to make sure I didn't make a typo.
Thanks for your help but I cant seem to get this one to come out to any of my possible answers. I think I am just getting confused on this one for some reason.
What are the possible answers?
0.165
0.330
0.498
0.298
0.198
0.0277*0.187/0.0157 = 0.32993 which rounds to 3 s.f. as 0.330. I see one like that. Don't you?
I got it finally.
Thank You
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