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chemistry > Unit 11 test > Flashcards

Unit 11 test Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

An acid with two ionizable protons

A

diprotic

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2
Q

The number of hydrogen ions equals the number of moles of hydroxide ions

A

titration

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3
Q

A proton donor

A

Bronsted Lowry Acid

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4
Q

Process of adding a known amount of solution of known concentration to determine the concentration of another solution

A

titration

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5
Q

Indicator changes color at the

A

end point

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6
Q

A 0.12M of an acid that ionizes only slightly in a solution would be termed

A

dilute and weak

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7
Q

The ratio of moles of a solute in a solution to the total number of moles both solute and solvent

A

mole fraction

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8
Q

A solution whose concentration is accurately known

A

standard solution

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9
Q

When an acid reacts with a metallic carbonate the products are

A

salt, carbon dioxide, and water

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10
Q

What is a distinct property of an acid?

A

sour taste

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11
Q

What is an acid according to Arrunius

A

a substance that is a hydrogen ion donor

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12
Q

What is an example of a strong acid?

A

perchloric acid

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13
Q

What has a weak acid and a strong base

A

acetic acid, sodium hydroxide

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14
Q

With solutions of strong acids and strong bases the word strong refers to

A

the degree of ionization

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15
Q

A solution containing maximum amount of solute

A

saturated solution

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16
Q

What is transferred between a conjugate acid base pair

A

a proton

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17
Q

Moles of solute in one liter of solution

A

molarity

18
Q

if 2.0M of a 6.0M HCl is to make 500.0ml of solution, what is the molarity of the dilute solution?

A

(2.0M x 6.0M)/ 500ml = 0.024M dilute solution

19
Q

What does not change when a solution is diluted by the addition of a solvent?

A

number of moles of solute

20
Q

What mass of sodium sulfate is needed to make 2.5L of a 2.0M solution?

A

(2.0mol/1L) x 2.5L/1 x 142.04g/ 1 mol
= 710.02
=710g

21
Q

What is the number of moles of solute in 250ml of a 0.4 M solution

A

0.4mol/1000ml x 250ml = 0.1mol

22
Q

What is the molarity of a solution containing 409.5 grams of sodium chloride in 569 ml of solution?

A

409.5gNaCl x 1mol/ 58.44gNaCl x 1/569ml x 1000ml/1L = 12MNaCl

23
Q

Which of the following substances is less soluble in hot water than cold water?

A

carbon dioxide

24
Q

Which compound can act both as a B Lowry acid and base?

A

water

25
Q

Which of the following is an Arrhenius base?

A

LiOH (any OH)

26
Q

Calculate the ion concentration of a solution with a pH of 5

A

10^-5

27
Q

What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0mL of 0.400M NaOH

A

16, 1 NaOH + 1 HCl → 1 NaCl + 1 H2O 0.32

28
Q

Measure of the amount of solute in a specified amount of solvent

A

concentration

29
Q

What is the pH of a 1 x10 -5 MKOH solution

A

-log (1x10 -5)

30
Q

What is the pH when the hydronium ion concentration is 1 x 10 -3M

A

3

31
Q

A solution is a homogeneous mixture of two or more substances

A

True

32
Q

Contains free ions

A

electrolyte

33
Q

Steel is an example of a solid solution

A

true

34
Q

The major component in a solution is called the solute

A

false

35
Q

A saturated solution holds the maximum amount of solute under the solution conditions

A

true

36
Q

A sugar solution is an example of a weak electrolyte solution

A

false

37
Q

The solubility of solids in water generally increases with increasing temperatures

A

true

38
Q

What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 MHCl to a final volume of 1.20 L

A

do the dilution equation M1V1=M2V2

39
Q

After you have completed the task of diluting a solution, which statement below must be true

A

more volume, but lower concentration

40
Q

How many grams of KCl are needed to make 500mL of 2.45MKCl

A

2.45M/1000mL x 500mL x molar mass of KCl

41
Q

What is the missing molarity of a solution prepared by dissolving 10.7 g NaI in 0.250L

A

(10.7/molar mass NaI ) / 0.250L

42
Q

which of the following substances is not a solution?

-copper
-vodka
-air
-brass

A

copper

chemistry (2 decks)

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