1.
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Solid sodium nitrite is added to a solution that is 0.10 M HNO2. Which of the following best describes what occurs?
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2.
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Which of the following constitutes a buffer solution?
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3.
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A 100-mL sample of a buffer is 0.10 M NH3 and 0.10 M NH4Cl. If 100 mL of water is added to this solution, what occurs?
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4.
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Which of the following equations is correct? 
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5.
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Why is an indicator different colors at different pH's?
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6.
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If the following acids are titrated with 0.10 M NaOH, which will have the largest near-vertical "jump" in its titration curve?
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7.
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What is the pH after 10 mL of 0.10 M HCl(aq) is added to 14 mL of 0.10 M NaOH(aq)?
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8.
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When 1 x 10-8 mol of HCl is added to 1.0 liter of water, the hydronium-ion concentration from HCl is 10-8 M. This seems to indicate that the pH of the solution would be 8. This would indicate a basic solution was prepared by adding a strong acid to water. What factor have we overlooked?
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9.
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Which one of the following would not be a good buffer pair?
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10.
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A 7.500-g sample of a monoprotic weak acid, HA, is added to enough distilled water to produce 500.0 mL of a solution with pH = 2.716. The solution is then titrated with NaOH solution. At the point where the acid is half titrated, i.e., [HA] = [A-], the pH = 4.602. What is the molar mass of this acid?
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