Titration Problems
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The concentration of NaOH is 0. 5 M, if 30 ml is needed to titrate 35 mL of acid, what is the concentration of the acid?
- 1.The concentration of NaOH is 0.5 M, if 20 ml is needed to titrate 35 mL of acid, what is the concentration of the acid?
- A.
0.875 M of acid
- B.
0.0029 M of the acid
- C.
0.29 M of the acid
- D.
0.00875 M of acid
- 2.
- A.
0.157 M acid
- B.
0.29 M acid
- C.
0.0157 M acid
- D.
0.029 M acid
- 3.If 20.0 mL of 0.100 M HCl are titrated with 19.5 mL of an NaOH solution. What is the molarity of the NaOH solution?
- A.
0.0975 M NaOH
- B.
0.0103 M NaOH
- C.
0.103 M NaOH
- D.
0.975 M NaOH
- 4.The concentration of HCl, a strong acid is 0.5 M. If 20 ml HCl is needed to titrate 40 mL of NaOH, what is the concentration of NaOH?
- A.
0.25 M NaOH
- B.
0.5 M NaOH
- C.
1 M NaOH
- D.
0.1 M NaOH
- 5.The concentration of LiOH is 0.50 M. If 25 mL of LiOH is needed to titrate 40 mL of HNO3 (nitric acid) what is the concentraiton of HNO3?
- A.
0.03125 M HNO3
- B.
0.8 M HNO3
- C.
0.3125 M HNO3
- D.
0.08 M HNO3
- 6.
- A.
It tells when there is enough acid in the solution.
- B.
It tells when the equivalence point is obtained.
- C.
It tells when there is enough base in the solution
- 7.
- A.
H+ (aq) + OH- (aq) --> H2O
- B.
KOH (aq) + HCl (aq) -->H2O (l) + KCl
- C.
POH (aq) + HClO (aq) --> H2O (l) + PClO (aq)
- D.
KOH (aq) + HCl (aq) -->K2Cl (aq)+ H2O (l)
- E.
KOH (aq) + HCl (aq) --> K2Cl (aq)+ H2O (l) + H+
- 8.Calculate the molarity of a HCl solution if 25.0 mL of the solution is neutralized by 15.5 mL of 0.800 M NaOH:
- A.
0.248 M
- B.
0.496 M
- C.
1.29 M
- D.
0.645 M
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