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What is the product of CH3COOH plus (C2H5)2O?
Ch3coo(-) + h2o ---> ch3cooh + oh(-)
Balanced equation CH3COOH?
What is the balanced equation for Ch3COOH alone
What kind of solid is CH3COOH?
CH3COOH, or acetic acid, is a covalent molecular solid at room temperature.
Is CH3COOH a mixture or pure substance?
CH3COOH is a pure substance. It is the chemical formula for acetic acid.
How many atoms are in formula CH3COOH?
CH3COOH contains 8 atoms. Two carbon, two oxygen, and four hydrogen.
Is CH3COOH a weak acid?
Yes, CH3COOH (acetic acid) is a weak acid. It partially dissociates in water to release H+ ions, resulting in an equilibrium between the undissociated acid and its dissociated ions.
Which is more highly ionized HCl or CH3COOH?
HCl is more highly ionized than CH3COOH. When HCl dissolves in water, it completely dissociates into H+ and Cl- ions, while CH3COOH only partially dissociates into H+ and CH3COO- ions. This difference is due to the strength of the bonds in the molecules, with HCl having a stronger bond than CH3COOH, making it easier to break apart into ions.
How do you make caco3 ch3cooh into a double displacement reaction?
To convert CaCO3 and CH3COOH into a double displacement reaction, you would need to first separate CaCO3 into Ca2+ and CO32- ions, and CH3COOH into CH3COO- and H+ ions in solution. The double displacement reaction would occur when Ca2+ ions react with CH3COO- ions to form Ca(CH3COO)2, a water-insoluble compound that precipitates out of solution.
At a certain temperature a 0.12 m solution of acetic acid ch3cooh has a pH of 3.0 what is the ka of ch3cooh at this temperature?
Given that the pH of a 0.12 M solution of acetic acid (CH3COOH) is 3.0, you can calculate the concentration of H+ ions in the solution using the formula pH = -log[H+]. Once you have the concentration of H+ ions, you can use it to calculate the concentration of CH3COO- ions using the ionization constant expression for acetic acid (CH3COOH) and then determine the Ka value.
Why wouldn't CH3COOH an acetic acid be considered an Arrhenius acid?
CH3COOH (acetic acid) is not considered Arrhenius acid because it is a weak acid that does not completely dissociate in water to produce H+ ions. Arrhenius acids are defined as substances that dissociate in water to produce H+ ions. Acetic acid only partially ionizes in water, forming both H+ ions and CH3COO- ions.
Chemical reaction of k3fecn6 in ch3cooh?
When potassium hexacyanoferrate(III) (K3[Fe(CN)6]) is added to acetic acid (CH3COOH), it reacts to form potassium acetate (CH3COOK), ferric ions (Fe^3+), and cyanide ions (CN^-). This reaction involves the displacement of cyanide ligands from the hexacyanoferrate(III) complex by acetate ions.
What best describes solutions of equal concentrations of HCL and CH3COOH?
At equal concentrations, the pH of HCl solution will be lower than that of CH3COOH solution due to HCl being a stronger acid than CH3COOH. This is because HCl fully dissociates in water to produce more H+ ions compared to the partial dissociation of CH3COOH.
What is the most spectated Canadian sport?
hockey
What is the most spectated sport in the world?
Soccer
Is agch3coo ionic compound?
No, acetic acid (CH3COOH) is a covalent compound. Its ions only form when it dissociates in water, creating acetate ions (CH3COO-) and hydronium ions (H3O+).
What is the chemical equation for acetic acid and potassium hydroxide?
Acetic acid (Ethanoic acid) is a weak acid, and when reacted with a strong base like Potassium hydroxide, it establishes an equilibrium: CH3COOH + KOH <=> CH3COOK + H2O The reaction mixture contains all four products in different proportions, and as such, an acid buffer is created. When an acid is added, the CH3COO- ions (those mixed with the K+ ions) 'mop up' the H+ ions from the acid. When a base is added, the H+ ions from the CH3COOH 'mop up' the OH- ions so the pH is little affected. NB. pH=-log10(H+)
Why a mixture of ch3cooh and ch3coona can act as a buffer while a mixture of hcl and nacl can not?
Buffers are made out of what are called weak acids or weak bases. Mixtures of CH3COOH and CH3COONa can act as buffers because they don't break apart completely in solution like HCl and NaCl. As the CH3COOH and CH3COONa are in solution they keep the pH constant by either donating or accepting protons because they don't act like strong acids or bases. HCl is known as a strong acid where the hydrogen disassociates completely from the chloride. NaCl is not a buffer because it dissolves completely as welll
