Section 15.5- pH Flashcards

1
Q

pure water ____________ ionize

A

does (to a small extent)

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2
Q

equilibrium constant expession

A

K sub w = [? +] [? -]

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3
Q

the equilibrium constant (Ksubw) is called the

A

ion-product constant of water

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4
Q

like other equilibrium constants, Kw varies with

A

temperature

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5
Q

in ___________ solutions, the concentrations of H3O+ and OH- are equal

A

neutral (like pure water)

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6
Q

a solution in which hydronium ions predominate (H3O+ is greater than 1.00 x 10 ^-7 M)

A

acidic solution

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7
Q

a solution in which hydroxide ions predominate (OH- is greater than 1.00 x 10^-7 M)

A

basic solution

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8
Q

scale that measure the power of hydrogen

A

pH scale

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9
Q

if the pH scale is 0-6

A

acidic

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10
Q

if neutral, pH is

A

7

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11
Q

if the pH scale is 8-14

A

basic

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12
Q

a more convenient way to represent the H3O+ concentration is the

A

pH scale

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13
Q

the pH of a solution is defined as the

A
  • log of the hydronium ion molarity
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14
Q

equation for determining pH

A

pH= - log [H3O+]

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15
Q

simply another way to express a number as a power of 10

A

logarithm

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16
Q

to find the pH of a given solution, simply find the logarithm of [H3O+] in that solution and

A

change the sign

17
Q

in a logarithm, only the digits to the ______________________ count as significant figures

A

right of the decimal point

18
Q

the OH- concentration may be expressed using

19
Q

the pH and pOH scales are closely related; in any aqueous solution at 25 C, the sum of the pH and pOH is

A

14
pH + pOH= 14

20
Q

the pH of a solution is most conveniently measured by an electronic

determines pH of a solution by precisely measuring the electric current generated when a pair of special electrodes are immersed in the solution to be tested

21
Q

less precise pH value may be obtained by using

organic acids or bases whose color changes with the pH of the solution

A

acid-base indicators

22
Q

the best-known indicator is

an organic dye that is Blue in Basic solutions and reD in aciDic solutions

23
Q

high concentrations of H3O+ tend to suppress the ionization of the indicator, keeping it largely

A

nonionized (Le Chatelier’s Principle)

color of the acid form thus predominates

24
Q

ways to obtain approximate pH values include

A

universal indicator
pH paper

25
Q

a mixture of several indicators that imparts a characteristic color to the solution over the whole range of pH values

A

universal indicator