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- 1. Multiple ChoiceIdentify [OH−] = 1.0 × 10−6M as being true of acidic or basic solutions at 25◦C and then determine the pH.basic; pH = 6acidic; pH = 6basic; pH = 8acidic; pH = 8
- 2. Multiple ChoiceCalculate the [H+] in a solution which shows a pH of 11.70.11.7 M2.0 × 10−12 M5.0 × 10−3 M2.3 M
- 3. Multiple ChoiceThe pH of a solution is 4.0. What is the H3O+ concentration in this solution? Is this an acidic or a basic solution?1.0x10-4M; Acidic1.0x10-4M; Basic1.0x10-10M; Acidic1.0x10-10M; Basic
- 4. Multiple ChoiceA solution contains 0.00100M HCl. Determine the [OH−].1.00x10-3M [OH−]1.00x10-14M [OH−]1.00x10-7M [OH−]1.00x10-11M [OH−]
- 5. Multiple ChoiceA solution in which the pH is 12.5 would be described as _______ and would have a pOH of ____.Basic; 1.5Basic; 12.5Acidic; 1.5Acidic; 12.5
- 6. Multiple ChoiceThe [H3O+] of a solution is 5.0x10-8. How would you determine the [OH-]?Divide 1.0x10-14 by
5.0x10-8Multiply 1.0x10-14 by
5.0x10-8Add 5.0x10-8 to
1.0x10-14Subtract 5.0x10-8 from
1.0x10-14 - 7. Multiple ChoiceA solution has a
[OH-]=2.4x10-4M.
Does this correspond to a pOH greater than or less than 4? Is the solution acidic or basic?pOH < 4; acidicpOH > 4; acidicpOH < 4; basicpOH > 4; acidic - 8. Multiple ChoiceHow does the concentration of Sr(OH)2 compare to the concentration of OH- in the same solution?[Sr(OH)2] = [OH-][Sr(OH)2] < [OH-][Sr(OH)2] > [OH-][Sr(OH)2] ? [OH-]
- 9. Multiple ChoiceIf you add 0.001 moles of HCl to 1 liter of water, the pH of the solution will be2.05.03.01.0
- 10. Multiple ChoiceA sample of pure water is neutral because it containssome hydronium ions.equal amounts of hydroxide and hydronium ions.some hydroxide ions.only H2O molecules.
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