Comparison of the concentration of acetate ions, and comparison of the concentration of ions in sodi

Ionization: CH3COOH = (reversible) CH3COO-+H+ (Acetic acid is a weak acid, and the degree of ionization is extremely weak.) )

Because in solution, water is also ionized. H2O = (reversible) OH-+H+ First, analyze what particles are in the solution. CH3COOH (molecule), CH3COO-, H+, OH-, (water molecules do not compare their concentration size).

Then, see what the solute is in solution! As a result, the concentration of CH3COOH (molecule) is maximum.

H+** ionizes acetic acid and water, so the concentration is greater than that of CH3COO-.

The smallest is the concentration of OH-!

In summary, C(CH3COOH) is greater than C(H+) is greater than C(CH3CoO-) is greater than C(OH-).

Merry Christmas to you. (*

Because it is an acid, c(h+) is greater than c(oh-).

Whereas, acetic acid is a weak electrolyte, so most of the acetic acid molecules are not ionized.

Whereas c(h+) is obtained by ionization of 2 parts, (part is ionization of acetic acid and the other part is ionization of water), therefore.

C(H+) is greater than C(CH3CoO-).

So: C(CH3COOH) is greater than C(H+) is greater than C(CH3COO-) is greater than C(OH-).

Ionization: CH3COONA=Na++CH3COO-, CH3COO-+H2O=(reversible)CH3COOH+OH-, the hydrolysis is very weak, and the ionization is complete. In the solution, the ion concentration is Na+>CH3COO-> OH-.

Sodium acetate is a strong electrolyte, which is easily soluble in water, so sodium acetate solution lead Qi has electrical conductivity.

Sodium acetate solution production methodOne-half part soda ash (sodium carbonate) (Na2CO3) or one part baking soda (sodium bicarbonate) (NaHCO3) + one part white vinegar or vinegar (acetic acid) (CH3COOH) = CH3Coona (sodium acetate) + H2O + CO2, and when the reaction is over, sodium acetate solution is obtained.

na2co3+2ch3cooh≒2ch3coona+co2↑+h2onahco3+ch3cooh≒ch3coona+co2↑+h2o。

The acetic acid ion concentration can be calculated using the following formula:

Concentration (mol l) = mass of acetic acid (g) molecular weight of acetic acid (g mol) volume of liquid (l).

Give me a thumbs up if you think it's okay! Thank you!

CH3COO- +H2O=(reversible)=CH3COOH+OH-, from the hydrolysis equation, it can be seen that the concentration of hydrolyzed acetate ions = the concentration of acetic acid generated. However, because the degree of monohydrolysis of acetate ions is very small, the concentration of acetate ions without hydrolysis has been water-stared at the concentration of acetate ions, that is, the concentration of acetate or sodium ions in sodium acetate solution will be larger than that of acetate Kaituanzen acid.

With the same concentration of hydrogen ions, the acid concentration of the hydrochloric acid solution is greater than that of the acetic acid solution.

Hydrochloric acid (HCl) is a strong acid that completely dissociates into hydrogen ions (H+) and chloride ions (Cl-) in water. As a result, the hydrochloric acid solution has a higher concentration of hydrogen ions, a lower pH, and a greater concentration of acids.

Acetic acid (CH3COOH) is a weak acid that only partially dissociates into hydrogen ions (H+) and acetate ions (CH3COO-) in water. As a result, the acetic acid solution has a lower concentration of hydrogen ions, a higher pH, and a smaller acid concentration.

Although the hydrogen ion concentration of the two solutions is the same, because hydrochloric acid is a strong acid and completely dissociated, Zheng Shucha found that its acid concentration is greater than that of acetic acid.

I think it's good, oh!

C(CH3COO-)>C(Na+)>C(H+)> C(OH-)CH3COO- is the most abundant, because sodium acetate is completely ionized, and acetic acid ionization will also form acetate ions, which is the largest.

Na+ is the second and comes from the ionization of sodium acetate.

The third is H+, the solution is acidic, and the ionization of acetic acid causes Zheng Lu to be deficient.

The least is to shout oh-

When the concentration of the solution increases, it is beneficial for the free hydrated ions to change into weak electrolyte molecules, and the degree of ionization decreases: When the concentration of the solution decreases, it is beneficial for the weak electrolyte molecules to change into free hydrated ions, and the degree of ionization increases. Because the concentration is rarer, the less chance that the ions will collide with each other and combine into molecules, and the greater the degree of ionization.

Because the ionization process is endothermic, the ionization tendency is strengthened when the temperature increases, and because there is no significant thermal change when most electrolytes are ionized, this leads to the inevitable result that although the temperature has an effect on the ionization degree, the effect is not large. In general, temperature has little effect on the degree of ionization, but the dissociation process of water is significantly endothermic, so the increase in temperature can increase the ionization degree of water.

Therefore, when comparing the relative strength of several electrolytes with the degree of ionization, it is necessary to pay attention to the conditions given, i.e., concentration and temperature, which is usually 25 if the temperature is not indicated. At the same temperature and concentration, the magnitude of the degree of ionization can indicate the relative strength of the weak electrolyte.

First of all, acetic acid is mixed with sodium acetate and does not undergo any chemical reaction, so only the ionization of the solution is considered, and it can be assumed that sodium acetate is completely ionized: ch3coona=na+ +ch3coo-, while acetic acid is a weak acid partially ionized: ch3cooh h+ +ch3coo-, and some exist as ch3cooh molecules.

Both also have the ionization of water: H2O H+ + OH-, and since it is an acidic solution, C(H+) > C(Oh-).

The amount and concentration of acetic acid and sodium acetate in the mixed solution are equal, that is to say, the amount of acetic acid and sodium acetate is the same, so C(CH3Coo-)>C(Na+)>C(H+)>C(OH-).

According to the degree of ionization of acetic acid is greater than the degree of hydrolysis of sodium acetate, it can be seen that the solution is acidic, that is, C(H+)>C(OH-)According to the conservation of charge, it can be known that C(Na+)C(Na+)>C(H+)>C(oh-).

Ionization: CH Coona = Na+ + CH COO - Hydrolysis: CH CoO- +H O = (Reversible) CH CoOH + OH - Hydrolysis is very weak and ionization is complete!

In the solution, the ion concentration size is Na+ >ch CoO->-OH-acetate. In aqueous solution, it is a very weak base (pkb =, strong acids cannot be used in water.

Accurate titration, so non-aqueous titration is required. Choose an appropriate solvent such as glacial acetic acid.

It can greatly improve the alkalinity of sodium acetate.

Sodium acetate solution solute sodium acetate, solvent water. Changes that exist.

ch3coona = ch3coo- +na+ complete, primary.

CH3COO- +H2O == Reversible===CH3COOH +OH- Incomplete, reversible, secondary.

About hydrolysis, or ch3coo-

H2O==Reversible=== H+ +OH- Incomplete, reversible, weak.

na+ >ch3coo- >oh- >ch3cooh > h+

Concentration: sodium ion, acetate, hydroxide, hydrogen ion.

The sodium ion is the most, and the hydrolysis of acetate reduces the hydrogen ion, and the KA in the water remains unchanged, so the hydroxide ion increases.