Which is more acidic 0.1 m HCl or 1M CH3COOH?

1M HCl has higher concentration of H+ ions because HCl is a strong acid while CH3COOH is a weak acid. So HCl dissociate completely in aqueous solution but CH3COOH dissociate partially in aqueous solution according to it’s dissociation coefficient.

What will be the pH of 0.1 molar 0.1 M HCl?

1
Strong Acids and Bases pH of 0.1 M HCl = 1, etc.

What is the pH of a 0.1 M solution of hydrochloric acid HCl )?

1.083
The pH of the 0.1 molar HCl solution is 1.083 (rather than 1.0 as often assumed).

Why is the pH of the 0.1 M HCl solution not the same as a 0.1 M acetic acid solution?

In theory, the pH of 0.1 M HCl solution should be 1.0 (strongly acidic). Although both solutions were 0.1 M in concentration, HCl is a strong acid and is fully ionized, whereas acetic acid is a weak acid and only partially ionized.

Which one will be more acidic and why explain with example 1M HCl and 1M CH3COOH?

1m HCl will have a higher concentration of H+ ions than 1m of CH3COOH. This is because of one simple reason – the acidity of the compounds. HCl is generally classified as a strong acid in comparison to CH3COOH which is a weak acid. Hydrochloric acid (HCl) will produce more H+ ions.

What is the pH of 0.1 m?

13
Therefore, the pH of 0.1 M NaOH solution is 13.

What is the pH of a 0.1 M solution of hydrocyanic acid?

5.2
The pH of 0.1M hydrocyanic acid solution is 5.2 .

Why is the pH of a 0.1 M solution of acetic acid in water higher than that of a 0.1 M solution of HCl in water?

Why is the pH of a 0.1 M solution of acetic acid in water higher than that of a 0.1 M solution of HCl in water? The acetic acid does not fully ionize in water, whereas HCl does. Frozen water is less dense than liquid water.

Why does 1 M HCl solution have higher concentration of H+ ion than 1 m CH3COOH?

HCl is stronger than CH3COOH. There is complete dissociaton of HCl which produces more H+ ions as compare to CH3COOH which is weak acid. So, 1 M HCL have higher concentration than 1 M CH3COOH.

What is the pH of 200 ml of HCl and CH3COOH?

What is the pH of 200mL of 0.1 M HCl mixed with 50mL of 0.1M CH3COOH (Ka = 1.8 x 10-5)? Both of them are acids, so the pH will definitely be below 7. HCl is a strong acid, while CH3COOH is a weak acid. This is important to remember, since while a strong acid will virtually be completely dissociate in water, not all molecules of a weak acid will.

What is the pH of a buffer solution containing CH3COOH and CH3COONa?

The pH of a buffer solution containing 0.1 M CH3COOH and 0.1 M CH3COONa is 4.74 . What will be the pH if 0.05 mole of HCl is added to one litre of this buffer solution?

What is a solution with a pH greater than 7?

Solutions with a pH less than 7 are acidic and solutions with a pH greater than 7 are basic. Pure water is neutral, at pH 7 (25 °C), being neither an acid nor a base. Contrary to popular belief, the pH value can be les

What is the dissociation of CH3COOH in HCl?

CH3COOH is a weak acid that does not dissociate to a great extent. In the presence of HCl which is a strong acid that dissociates completely , the dissociation of the CH3COOH will further reduced. We start by calculating the H+ contributed by the CH3COOH using the Ka equation. 0.01H = (1.8*10^-5)*0.1