Can someone please check my work and answers on these two titration problems?
1.) If 16.45 mL of 0.135 M nitric acid neutralizes 26.0 mL of ammonium hydroxide, what is the molarity of the base?
HNO3(aq) + NH4OH(aq) --> NH4NO3(aq) + H2O(l)
I used stoichiometry to find the # of moles of ammonium hydroxide:
(0.01645 L HNO3) x (0.135 mol HNO3/1 L HNO3) x (1 mol NH4OH/1 mol HNO3)= 0.002221 mol NH4OH
Then used the molarity formula with the volume for the base:
0.002221 mol NH4OH/0.026 L NH4OH= 0.0854 M
Is this the correct answer (0.0854 M)?
2.) If the titration of a 24.0 ml sample of acetic acid requires 25.90 ml of 0.010 M calcium hydroxide, what is the molarity of the acid?
2HC2H3O2(aq) + Ca(OH)2(aq) --> Ca(C2H3O2)2(aq) + 2H2O(l)
I did this one the same way by using stoichiometry first to find moles of acetic acid:
0.02590 L Ca(OH)2 x (0.010 mol Ca(OH)2/1 L Ca(OH)2) x (2 mol HC2H3O2/1 mol Ca(OH)2)= 0.000518 mol acid
Again, I used the molarity formula with the volume given for acetic acid in the problem:
0.000518 mol HC2H3O2/ 0.024 L= 0.0216 M
Is this ans werrect answer (0.0216 M)?
Your time and help are greatly appreciated by me! Thank you so much!