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1. The difference between HCl and HC2H3O2 as acids is
A. the first has less hydrogen in solutionB. the second has more ionized hydrogenC. the first is highly ionizedD. the second is highly ionizedE.
2. The hydronium ion is represented as
A. H2O+B. H3O+C. HOH+D. H-E.
3. H2SO4 is a strong acid because it is
A. slightly ionizedB. unstableC. an organic compoundD. highly ionizedE.
4. The common ionic reaction of an acid with a base involves ions of
A. hydrogen and hydroxideB. sodium and chlorideC. hydrogen and hydroniumD. hydroxide and nitrateE.
5. Which pH is an acid solution?
A. 3B. 7C. 9D. 10E.
6. The pH of a solution with a hydrogen ion concentration of 1 × 10-3 is
A. +3B. -3C. ±3D. 1 + 3E.
7. According to the Bronsted-Lowry Theory, an acid is
A. a proton donorB. a proton acceptorC. an electron donorD. an electron acceptorE.
8. A buffer solution
A. changes pH rapidly with the addition of an acidB. does not change pH at allC. resists changes in pHD. changes pH only with the addition of a strong baseE.
9. The point at which a titration is complete is called the
A. end pointB. equilibrium pointC. calibrated pointD. chemical pointE.
10. If 10.mL of 1 M HCl was required to titrate a 20.mL NaOH solution of unknown concentration to its end point, what was the concentration of the NaOH?
A. 0.5 MB. 1.5 MC. 2 MD. 2.5 ME.
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