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ACID BASE AND SALTLoading...
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1-) ACIDS
H + ions in aqueous solutions are called acid.
HCl (water) -> H + (water) + Cl) (water)
H2SO4 (water) -> 2H + (water) + SO2-4 (in water)
Strength of Acids
Acids that are completely ionized in water are called strong acids.
HCI, H2SO4, HI ,,
- Acidic acids in the water are also called weak acids
HF, CH3COOH, HCN C ..
- As the ionization percentage of the acids increases, the electrical conductivity of the solution increases.
- The ionization equation of the strong acids is written with a one-way arrow, while the weak acids use double direction arrow
HCl -> H + (water) + Cl (in water)
- All organic acids are weak acids.,
HCOOH, CH3COOH, H2C204 …
- Acidic strength sequence in oxygen-free acids of group 7A
H + ions in aqueous solutions are called acid.
HCl (water) -> H + (water) + Cl) (water)
H2SO4 (water) -> 2H + (water) + SO2-4 (in water)
Strength of Acids
Acids that are completely ionized in water are called strong acids.
HCI, H2SO4, HI ,,
- Acidic acids in the water are also called weak acids
HF, CH3COOH, HCN C ..
- As the ionization percentage of the acids increases, the electrical conductivity of the solution increases.
- The ionization equation of the strong acids is written with a one-way arrow, while the weak acids use double direction arrow
HCl -> H + (water) + Cl (in water)
- All organic acids are weak acids.,
HCOOH, CH3COOH, H2C204 …
- Acidic strength sequence in oxygen-free acids of group 7A
1-) ACIDS
H + ions in aqueous solutions are called acid.
HCl (water) -> H + (water) + Cl) (water)
H2SO4 (water) -> 2H + (water) + SO2-4 (in water)
Strength of Acids
Acids that are completely ionized in water are called strong acids.
HCI, H2SO4, HI ,,
- Acidic acids in the water are also called weak acids
HF, CH3COOH, HCN C ..
- As the ionization percentage of the acids increases, the electrical conductivity of the solution increases.
- The ionization equation of the strong acids is written with a one-way arrow, while the weak acids use double direction arrow
HCl -> H + (water) + Cl (in water)
- All organic acids are weak acids.,
HCOOH, CH3COOH, H2C204 …
- Acidic strength sequence in oxygen-free acids of group 7A
H + ions in aqueous solutions are called acid.
HCl (water) -> H + (water) + Cl) (water)
H2SO4 (water) -> 2H + (water) + SO2-4 (in water)
Strength of Acids
Acids that are completely ionized in water are called strong acids.
HCI, H2SO4, HI ,,
- Acidic acids in the water are also called weak acids
HF, CH3COOH, HCN C ..
- As the ionization percentage of the acids increases, the electrical conductivity of the solution increases.
- The ionization equation of the strong acids is written with a one-way arrow, while the weak acids use double direction arrow
HCl -> H + (water) + Cl (in water)
- All organic acids are weak acids.,
HCOOH, CH3COOH, H2C204 …
- Acidic strength sequence in oxygen-free acids of group 7A
- The very oxygenated state of an acid is stronger than the less oxygenated state.
For example,
HCIO4> HCIO3> HCIO2> HCIO
For example,
HCIO4> HCIO3> HCIO2> HCIO
GENERAL FEATURES OF ACIDS
They give H + ion to water.
It dissolves by ionizing in water.
Aqueous solutions transmit the electric current. (The electrolyte).
They turn the litmus paper into red.
The flavors are sour.
In room conditions, the pH of the aqueous solutions is less than 7.
Salt and H2 gas are formed from the reactions with other metals except noble metals (Gu, Hg, Ag, Pt, Au).
They react to neutralization with bases.
Since the carbonated compounds of metals 1A and 2A show basic properties, they react with acids to release salt, water and CO2 gas.
For example;
CaCO3 + 2HCl -> CaCl2 + H2O + CO2 (g)
Effect of acid on the number of H + when an acid molecule is dissolved in water
For example;
HCl -> H + Cl (1 acid)
H2SO4 -> 2H ++ SO2-4 (2-valued acid)
There is no relationship between the valence and strength of the acid.
For example;
H2C2O4 divalent acid (weak acid)
HCl is a valuable acid (strong acid)
For example;
H2S04 bivalent acid (strong acid)
HF is a valuable acid (weak acid)
They give H + ion to water.
It dissolves by ionizing in water.
Aqueous solutions transmit the electric current. (The electrolyte).
They turn the litmus paper into red.
The flavors are sour.
In room conditions, the pH of the aqueous solutions is less than 7.
Salt and H2 gas are formed from the reactions with other metals except noble metals (Gu, Hg, Ag, Pt, Au).
They react to neutralization with bases.
Since the carbonated compounds of metals 1A and 2A show basic properties, they react with acids to release salt, water and CO2 gas.
For example;
CaCO3 + 2HCl -> CaCl2 + H2O + CO2 (g)
Effect of acid on the number of H + when an acid molecule is dissolved in water
For example;
HCl -> H + Cl (1 acid)
H2SO4 -> 2H ++ SO2-4 (2-valued acid)
There is no relationship between the valence and strength of the acid.
For example;
H2C2O4 divalent acid (weak acid)
HCl is a valuable acid (strong acid)
For example;
H2S04 bivalent acid (strong acid)
HF is a valuable acid (weak acid)
- The very oxygenated state of an acid is stronger than the less oxygenated state.
For example,
HCIO4> HCIO3> HCIO2> HCIO
For example,
HCIO4> HCIO3> HCIO2> HCIO
GENERAL FEATURES OF ACIDS
They give H + ion to water.
It dissolves by ionizing in water.
Aqueous solutions transmit the electric current. (The electrolyte).
They turn the litmus paper into red.
The flavors are sour.
In room conditions, the pH of the aqueous solutions is less than 7.
Salt and H2 gas are formed from the reactions with other metals except noble metals (Gu, Hg, Ag, Pt, Au).
They react to neutralization with bases.
Since the carbonated compounds of metals 1A and 2A show basic properties, they react with acids to release salt, water and CO2 gas.
For example;
CaCO3 + 2HCl -> CaCl2 + H2O + CO2 (g)
Effect of acid on the number of H + when an acid molecule is dissolved in water
For example;
HCl -> H + Cl (1 acid)
H2SO4 -> 2H ++ SO2-4 (2-valued acid)
There is no relationship between the valence and strength of the acid.
For example;
H2C2O4 divalent acid (weak acid)
HCl is a valuable acid (strong acid)
For example;
H2S04 bivalent acid (strong acid)
HF is a valuable acid (weak acid)
They give H + ion to water.
It dissolves by ionizing in water.
Aqueous solutions transmit the electric current. (The electrolyte).
They turn the litmus paper into red.
The flavors are sour.
In room conditions, the pH of the aqueous solutions is less than 7.
Salt and H2 gas are formed from the reactions with other metals except noble metals (Gu, Hg, Ag, Pt, Au).
They react to neutralization with bases.
Since the carbonated compounds of metals 1A and 2A show basic properties, they react with acids to release salt, water and CO2 gas.
For example;
CaCO3 + 2HCl -> CaCl2 + H2O + CO2 (g)
Effect of acid on the number of H + when an acid molecule is dissolved in water
For example;
HCl -> H + Cl (1 acid)
H2SO4 -> 2H ++ SO2-4 (2-valued acid)
There is no relationship between the valence and strength of the acid.
For example;
H2C2O4 divalent acid (weak acid)
HCl is a valuable acid (strong acid)
For example;
H2S04 bivalent acid (strong acid)
HF is a valuable acid (weak acid)
2-) BASE
The substances that give the OH ~ ion to the aqueous solution are base.
Force of Bases
Bases that are completely ionized in water are called strong bases. All of the 1A metal hydroxides and the Ba (OH) 2 are the strong base. LiOH, NaOH, KOH, Ba (OH) 2
The less ionized bases in water are called weak bases. AgOH, NH3, N2H4.
- The ionization equations of strong bases are written with a one-way arrow. The ionization equations of weak bases are written with a bi-directional arrow.
- NH3 is a weak anhydrous base. Ionization equivalents are not written without water. Reacts with acids only salt is formed.
- The strength of the base increases as a group goes down in metals. This is because the atomic diameter is increased. KOH> NaOH> LiOH
GENERAL CHARACTERISTICS OF BASES
They give the water an OH-ion.
It dissolves by ionizing in water.
The aqueous solutions are electrolyte.
Turn the litmus blue into blue.
In room conditions, the pH of the aqueous solutions is greater than 7.
They react with amphoteric metals to form salt and H2 gas.
The substances that give the OH ~ ion to the aqueous solution are base.
Force of Bases
Bases that are completely ionized in water are called strong bases. All of the 1A metal hydroxides and the Ba (OH) 2 are the strong base. LiOH, NaOH, KOH, Ba (OH) 2
The less ionized bases in water are called weak bases. AgOH, NH3, N2H4.
- The ionization equations of strong bases are written with a one-way arrow. The ionization equations of weak bases are written with a bi-directional arrow.
- NH3 is a weak anhydrous base. Ionization equivalents are not written without water. Reacts with acids only salt is formed.
- The strength of the base increases as a group goes down in metals. This is because the atomic diameter is increased. KOH> NaOH> LiOH
GENERAL CHARACTERISTICS OF BASES
They give the water an OH-ion.
It dissolves by ionizing in water.
The aqueous solutions are electrolyte.
Turn the litmus blue into blue.
In room conditions, the pH of the aqueous solutions is greater than 7.
They react with amphoteric metals to form salt and H2 gas.