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Which effect can explain increase in dissociation of acetic acid on addition of naoh?
The increase in dissociation of acetic acid upon addition of NaOH can be explained by Le Chatelier's principle. The additional NaOH added reacts with the acetic acid to form acetate ions and water, shifting the equilibrium of the acetic acid dissociation reaction to the right to replace the consumed acetic acid. This results in increased dissociation of acetic acid to maintain equilibrium.
20 ml of acetic acid is titrated with a solution of 0.15 M NaOH If 35 ml of NaOH are required to reach the equivalence point what is the concentration of the acetic acid solution?
The moles of NaOH at the equivalence point will equal the moles of acetic acid present in the solution. Therefore, using the volume and concentration of NaOH used at the equivalence point, you can calculate the moles of NaOH used. Then, based on the stoichiometry of the reaction, you can determine the moles of acetic acid, and finally, determine the concentration of the acetic acid solution.
Why there is a steep rise in the pH of acetic acid on titrating it with NaOH?
The steep rise in pH of acetic acid when titrated with NaOH occurs near the equivalence point because at that point nearly all the acetic acid has been neutralized, resulting in a rapid increase in pH from the addition of hydroxide ions. This phenomenon is due to the buffering capacity of acetic acid being overwhelmed as it reacts with the base to form acetate ions.
How many mL of 0.55 M NaOH would be required to reach the equivalence point for 25.0 mL of a 0.75 M solution of acetic acid?
To determine the volume of 0.55 M NaOH needed to reach the equivalence point with 25.0 mL of 0.75 M acetic acid, you need to use the stoichiometry of the reaction. Acetic acid reacts with NaOH in a 1:1 ratio, so moles of acetic acid equals moles of NaOH at the equivalence point. Calculate moles of acetic acid from its concentration and volume, equate it to moles of NaOH, and then calculate the volume of NaOH solution needed.
Comlpete molecular equation of acetic acid and sodium hydroxide?
The complete molecular equation for the reaction between acetic acid (CH3COOH) and sodium hydroxide (NaOH) is: CH3COOH (aq) + NaOH (aq) -> CH3COONa (aq) + H2O (l)
Which effect can explain increase in dissociation of acetic acid on addition of naoh?
The increase in dissociation of acetic acid upon addition of NaOH can be explained by Le Chatelier's principle. The additional NaOH added reacts with the acetic acid to form acetate ions and water, shifting the equilibrium of the acetic acid dissociation reaction to the right to replace the consumed acetic acid. This results in increased dissociation of acetic acid to maintain equilibrium.
20 ml of acetic acid is titrated with a solution of 0.15 M NaOH If 35 ml of NaOH are required to reach the equivalence point what is the concentration of the acetic acid solution?
The moles of NaOH at the equivalence point will equal the moles of acetic acid present in the solution. Therefore, using the volume and concentration of NaOH used at the equivalence point, you can calculate the moles of NaOH used. Then, based on the stoichiometry of the reaction, you can determine the moles of acetic acid, and finally, determine the concentration of the acetic acid solution.
Why there is a steep rise in the pH of acetic acid on titrating it with NaOH?
The steep rise in pH of acetic acid when titrated with NaOH occurs near the equivalence point because at that point nearly all the acetic acid has been neutralized, resulting in a rapid increase in pH from the addition of hydroxide ions. This phenomenon is due to the buffering capacity of acetic acid being overwhelmed as it reacts with the base to form acetate ions.
20ml of acetic acid is titrated with a solutuion of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
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How many mL of 0.55 M NaOH would be required to reach the equivalence point for 25.0 mL of a 0.75 M solution of acetic acid?
To determine the volume of 0.55 M NaOH needed to reach the equivalence point with 25.0 mL of 0.75 M acetic acid, you need to use the stoichiometry of the reaction. Acetic acid reacts with NaOH in a 1:1 ratio, so moles of acetic acid equals moles of NaOH at the equivalence point. Calculate moles of acetic acid from its concentration and volume, equate it to moles of NaOH, and then calculate the volume of NaOH solution needed.
Comlpete molecular equation of acetic acid and sodium hydroxide?
The complete molecular equation for the reaction between acetic acid (CH3COOH) and sodium hydroxide (NaOH) is: CH3COOH (aq) + NaOH (aq) -> CH3COONa (aq) + H2O (l)
Which is the best method of estimate acetic acid in pharmaceutical and commercial preparation?
The best method for estimating acetic acid in pharmaceutical and commercial preparations is typically titration using a standardized sodium hydroxide (NaOH) solution. This method involves titrating a known volume of acetic acid solution with NaOH until a color change occurs, indicating neutralization. The volume of NaOH used can then be used to calculate the concentration of acetic acid in the sample.
How Many milliliters of 0.258 M NaOH are required to complétely neutrilize 2.00 g of aceitic acid HC2H3O2?
To find the volume of 0.258 M NaOH needed to neutralize 2.00 g of acetic acid (HC2H3O2), you can use the molar ratio between NaOH and acetic acid. First, determine the moles of acetic acid using its molar mass. Then, use the mole ratio from the balanced chemical equation to find moles of NaOH required. Finally, use the concentration of NaOH to find the volume needed.
20 ml of acetic acid ch3cooh is titrated with a solution of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
Using the balanced equation, CH3COOH + NaOH -> CH3COONa + H2O, we know that one mole of acetic acid reacts with one mole of NaOH at the equivalence point. Since 35 ml of 0.15 M NaOH are required to reach the equivalence point, this is equal to 35 ml * 0.15 mol/L = 5.25 mmol of NaOH. As the reaction is 1:1, the amount of acetic acid is also 5.25 mmol. Therefore, the concentration of the acetic acid solution is 5.25 mmol / 20 ml = 0.2625 mol/L.
What is the process to calculate the percentage of acetic acid in vinegar?
To calculate the percentage of acetic acid in vinegar, you can use a simple titration method. First, you need to titrate a known volume of vinegar with a standardized solution of sodium hydroxide (NaOH) using phenolphthalein as an indicator. The volume of NaOH required to neutralize the acetic acid in the vinegar can be used to calculate the concentration of acetic acid. Finally, you can convert the concentration to a percentage by considering the molar mass of acetic acid.
What are the products of the reaction between acetic acid and sodium hydroxide?
the products are CH3COOH + NaOH ------CH3COONa + H2O
What is equation for sodium hydroxide and acetic acid?
The reaction between sodium hydroxide (NaOH) and acetic acid (CH3COOH) forms sodium acetate (CH3COONa) and water (H2O). The balanced chemical equation is: CH3COOH + NaOH -> CH3COONa + H2O.
