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Chem CIE > acids, bases, and salts > Flashcards

acids, bases, and salts Flashcards

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1
Q

What is the formula between Acids with metal carbonates?

A

Acid + Metal Carbonate → Salt + Carbon Dioxide + Water

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2
Q

What is the formula between Acids with bases?

A

Acid + Base → Salt + Water (neutralization reaction)

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3
Q

What is the formula between Acids and metals?

A

Acid + Metal → Salt + Hydrogen

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4
Q

What is the formula between Alkalis and ammonium salts? (decomposition reaction)

A

For example, NH4Cl + NaOH →NaCl + H2O + NH3

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5
Q

What’s an acid?

A

A specie that dissociates in water to release H+ ions

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6
Q

What are the physical properties of acid?

A
  • Sour taste
  • Corrosive
  • Turns blue litmus to red
  • Strong acids are good electrolytes (conduct electricity)
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7
Q

How do you use the universal indicator differentiate between strong and weak acids? (process)

A
  • Dip universal indicator in equal amount
    of different acids
  • Compare the color with the pH chart
  • If pH is low then it is a strong acid; vice versa
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8
Q

Why is ethanoic acid described as a weak acid?

A

It is only slightly dissociated in water

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9
Q

What is the meaning of the term ‘weak acid’?

A

It means that it partially dissociates in water

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10
Q

Methanesulfonic acid is a stronger acid than ethanoic acid.

Explain this statement

A

Methanesulfonic acid completely dissociates in water to release H+ ions whereas ethanoic acid partially dissociates in water

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11
Q

What’s an alkali?

A

a specie that dissociates in water to
release OH- ions

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12
Q

What are the physical properties of bases?

A
  • bitter taste
  • feels soapy and slippery
  • Turns red litmus to blue
  • Strong alkalis are good electrolytes (can conduct electricity due to free ions)
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13
Q

How do you use the universal indicator to differentiate between strong and weak alkalis? (process)

A
  • Dip the universal indicator in equal amounts of both alkali solutions
  • Compare the color with the pH chart
  • The greater the pH, the stronger the alkali
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14
Q

Which statement describes a weak acid?

A

It is a proton donor and is partially ionized in an aqueous solution

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15
Q

Define pH.

A

A measure of acidity or alkalinity of solutions

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15
Q

Aqueous ammonia reacts with a compound to form a salt, ammonium phosphate.

What type of reaction will ammonia undergo to form ammonium phosphate?

A

Neutralization

16
Q

How can we find pH?

A
  • Litmus solution ( test for acids and bases)
  • it only tells us about acid or base and no pH
17
Q

Methyl orange indicator.

COLOR in ACID:

COLOR in NEUTRAL:

COLOR in BASE:

A

COLOR in ACID: RED

COLOR in NEUTRAL: ORANGE

COLOR in BASE: YELLOW

18
Q

Phenothalein indicator.

COLOR in ACID:

COLOR in NEUTRAL:

COLOR in BASE:

A

COLOR in ACID: Colorless

COLOR in NEUTRAL: Colorless

COLOR in BASE: Pink

19
Q

Thymolphthalein indicator.

COLOR in ACID:

COLOR in NEUTRAL:

COLOR in BASE:

A

COLOR in ACID: Colorless

COLOR in NEUTRAL: Colorless

COLOR in BASE: Blue

20
Q

Why do we use the universal indicator method to find pH on paper?

A
  • It gives a rough idea of the pH
  • Therefore, It’s better than using the litmus test method
21
Q

Why is it not advisable to add fertilizers and limewater simultaneously? (2)

A
  • Ammonium salts react with limewater to give off ammonia gas.
  • As a result, nitrogen content for plants decreases since ammonia gas escapes to its surroundings.
22
Q

What’s salts?

A

it is a specie formed when hydrogen of an acid is replaced by a metal.

23
Q

Explain the process of titration.

A
  • Take the measured amount of HCl and NaOH in a burette and conical flask.
  • Pour a few drops of indicator into the conical flask
  • Allow HCl to pour into the conical flask until a color change is observed.
  • Note the volume of HCl used
  • perform titration again using the noted volumes of HCL and NaOH
  • {for evaporation} Boil off the solution 1/3rd and allow it to cool and crystallize.
  • {for evaporation} Dry them between sheets of filter paper
24
Q

Explain the process of crystallization.

A
  • Put excess CuO in a beaker containing HCl
  • Gently mix it until no more solid is disappearing
  • Filter off the excess CuO
  • {for evaporation} Boil off the solution 1/3rd and allow it to cool and crystallize.
  • {for evaporation} Dry them between sheets of filter paper
25
Q

Why is the excess CuO used?

A

To ensure that all the acid has reacted

26
Q

Explain the process of insoluble salts.

PRECIPITATION: TWO SOLUBLE salts react to give an INSOLUBLE salt and SOLUBLE salt

A
  • Put salt solution 1 into a beaker of salt solution 2
  • Gently mix until no more solid is forming
  • Perform filtration to obtain the insoluble salt formed
  • Wash the salt crystals with distilled water and dry them between sheets of filter paper.

Chem CIE (3 decks)

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