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Acids, bases & salts Revision.

Published byEvangeline Robertson Modified over 6 years ago

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Presentation on theme: "Acids, bases & salts Revision."— Presentation transcript:

1 Acids, bases & salts Revision

2 Properties Reactions Definition Weak Vs. Strong Common acids acids

3 definition A compound which produces hydrogen ions, H+, when dissolved in water Acid + H2O H+

4 Strong vs weak acids Strong acids IONIZED COMPLETELY in water Weak acids IONIZED PARTIALLY in water Strong Acid Dissociate completely HCl Cl- H+ Cl- H+ Cl- H+ water

5 Weak acids CH3COOH Weak acid does Not dissociate completely H+ CH3COOH
Ada CH3COOH Masih tetinggal CH3COOH water

6 Common acids Sulfuric Acid HCl H2SO4 Nitric Acid HNO3 Ethanoic Acid
Hydrochloric Acid CH3COOH

7 Properties Taste: Sour taste Litmus paper: Blue Red

8 Reactions of dilute acids
1. Some METALS to give SALT and HYDROGEN gas Zn + 2HCL ZnCl2 + H2 2. Bases to give SALT and WATER only 2NaOH + H2SO4  Na2SO4 + H2O 3. Carbonates and hydrogencarbonates (insoluble or soluble) to give salt, water and CO2 gas CaCO3 + 2HCl  CaCl2 + H2O + CO2

9 H+ OH- ACIDS BASES IONS THAT ARE PRODUCED!

10 Properties Reactions Definition Weak Vs. Strong Common bases bases

11 Substance which reacts with an acid to form salt and water only
Definition Substance which reacts with an acid to form salt and water only NEUTRALIZATION ACIDS + BASE  SALT + WATER

12 REACTIONS NaOH + NH4Cl  NaCl + NH3 + H2O
1) Reacts with acids to produce salt and water only 2) Ammonium salts to produce AMMONIA NaOH + NH4Cl  NaCl + NH3 + H2O AMMONIA

13 Common bases CaO Copper(II) Oxide Calcium Oxide MgO Magnesium Oxide
CuO Ammonia NaOH Sodium Hydroxide NH3

14 Then, what is an alkali Alkali are BASES THAT ARE SOLUBLE IN WATER
Insoluble in water ALKALI

15 ALKALI PROPERTIES Slippery Turns Litmus paper: Red Blue
Produces OH- when dissolved in water

16 Dissociation examples (remember)
Alkali when dissolved in water NaOH OH- + Na+ NaOH OH- Na+ Na+ OH- OH- Na+ water

17 What if we try to dissolve ammonia gas?
NH3 + H2O  NH4+ + OH- Do not forget OH-

18 Again, what is a weak alkali?
Weak Alkali when dissolved in water NH3 + H2O NH4+ + OH- NH3 NH4+ OH- OH- NH4+ NH3 water

19 neutralization H+ + OH-  H2O
In neutralization, the H+ from the ACID and the OH- from the Alkali react to form water H+ + OH-  H2O Energy Energy is being released: EXOTHERMIC

20 OXIDES ACIDIC OXIDES- OXIDES THAT ARE ACIDIC
BASIC OXIDES- OXIDES THAT ARE BASIC AMPHOTERIC OXIDES- OXIDES THAT ARE ACIDIC AND BASIC

21 EXAMPLES OF OXIDES BASIC Amphoteric ACIDIC Na2O CaO Al2O3 CO2 Fe2O3
ZnO H2O CO2 SO2 P4O10 CO, NO Neutral

22 indicators Substances that change COLORS in acidic and alkaline solutions Litmus indicator Red Acids Blue Bases These are used in TITRATION Phenolphthalein Colorless Acids Red/Pink Base

23 pH scale pH is a number to show how acidic or alkaline a solution is
Super acidic Getting Less basic Becoming Less acidic Super basic neutral 1 3 6 7 14 8 10 13 Very acidic Very Little acidity Very Less alkaline Very basic

24 Examples of neutral solution
Pure Water NaCl solution Most soluble salts Ethanol solution (not ethanoic acid)

25 Application: PH in soil
Soil can become too acidic because: Excessive use of chemical fertilizers Acid rain from air pollution by sulfur dioxide and nitrogen oxides Most plants grow well almost neutral Plants grow poorly in very high Or very low pH Soil How to fix an acidic soil?

26 Salts A salt is obtained from an acid when the H+ is replaced by metal ion or ammonium ion Na H Cl Acid Salt

27 Solubility of salts: Memorize this please
Type of salts Soluble Insoluble Carbonates (NH4)2CO3 Na2CO3 K2CO3 All the rest Chlorides PbCl2 AgCl Nitrates All - Sulfates BaSO4 PbSO4 (CaSO4 is slightly soluble)

28 Practice Soluble Insoluble K2SO4 Na2CO3 KNO3 Pb(NO3)2 BaSO4 CuSO4
BaCO3 AgCl

29 How do we prepare salts???

30 Case 1: I want to make an insoluble salt, pbcl2 (solid)
Step 1: think where PbCl2 comes from: Pb Pb2+ An aqueous solution (soluble) Pb(NO3)3 Cl2 Cl- An aqueous solution (soluble) NaCl Step: 2 Precipitation reaction Pb(NO3)2(aq) + NaCl(aq) Soluble Soluble  NaNO3(aq) + PbCl2(s) Soluble Insoluble

31 illustration Pb2+ Na+ NO3- PbCl2 solid Na+ NO3- Cl- Pb(NO3)2 solution
NaCl solution water

32 Getting the salt how? FILTRATION We have solid in a liquid Na+ NO3-
PbCl2 solid FILTRATION

33 This is how you get pbcl2

34 Case 2: Soluble salts 1. acid + excess metal/insoluble metal oxide/carbonate 2. acid+ alkali

35 How to prepare salts START NO Is the salt soluble? YES
React acid with metal/alkali/metal oxide/metal carbonate Product soluble? NO YES Mix acid with excess metal/ metal oxide/metal carbonate

36 Work this out: I want to make copper sulfate

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