What happens when we add NaOH to a CH3COOH solution?
(A) Nothing happens
(B) Formation of CH3COONa in solution
I know the answer is B, but can you explain why and how?
acetic acid is weak acid, so it dissociates partially and there is an establishment of an equilibrium between acetic acid and thier respective ions as
CH3COOH CH3COO- + H+
Where as sodium hydroxide is strong base. so it dissociates completely into Na+ and OH- ions as
NaOH Na+ + OH-
The acetate ion (CH3COO-) and the sodium cation (Na+) combine to form CH3COONa and the H+ ion combine with OH- ion form water as
CH3COO- + Na+ CH3COONa
H+ + OH- H2O
What happens when we add NaOH to a CH3COOH solution? (A) Nothing happens (B) Formation of...
What will happen to the pH (increace/decrease/same) of an aqueous solution of CH3COOH if I add A) solid CH3COONa B) gas HCl C) solid NaCl D) solid KNO3
1) What is the pH of a solution in which 25 mL of 0.10 M NaOH is added to 15 mL of 0.10 M HCl? 2) If you add 2.50 mL of 0.150 M HCl to 100 mL of a buffer consisting of 0.100 M CH3COOH and 0.200 M CH3COONa, what will be the change in pH? (Ka of CH3COOH is 1.8x10^-5)
Lab Questions 1. Explain what happens to the moles of H" in the flask when you add boiled, deionized water to rinse the wall of the flask during the titration. Explain what happens to the moles of OH' needed from the buret to neutralize the acid after adding the water. What is the overall effect on the calculated acetic acid % of your sample? 2. Suppose that you do not add the water to rinse the wall of the flask,...
CH3COOH(aq)+NAOH(aq)=CH3COONa+H2O i just need clarification on these questions | Example CH3COOH Titration Curve Standardizing a Solution of Sodium Hydroxide H pH=7.0 line TETROFFEN -2302392 ARXARAR ERDEREEEEEE EEEEEEEEEEEEEE Question 20 (1 point) Saved For the CH3COOH titation, given the autoionization of water, what is the impact of adding hydroxide ions on the concentration of H307? O [H3O+] increases O [H3O+] decreases [H30*) remains the same For the CH3COOH titation, given that impact on the concentration of H307, what is the shift...
What will be the pH value when we add 10 mL of 2 molar NaOH solution to 1 litre of 0.2 molar acetate buffer whose pH is 4.7? Pka = 4.7
What will happen if we add some concentrated sodium hydroxide to a saturated solution of sodium chloride? A) NaCl will precipitate. B) NaOH will precipitate. C) We’ll get a salty solution that has a kick. D) Nothing will happen.
What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 x 10-5 So the answer is 4.64. However, I was under the impression that it is Ka * (base/acid). So wouldn't that be 1.8 x 10^-5 * (.35/.45)? Isn't the CH3COONa the base? Someone please explain. Thank you.
When you add NaOH to a solution, the pH of the solution should 1)___________ because NaOH is a 2)_________ , which 3) ___________in solution. Choices: 1) Increase, decrease 2) base, acid, buffer 3)Decrease proton concentration, increase proton concentration, decrease hydroxide concentration
2. What happens when a few crystals are added to a supersaturated solution? Identify the situation in the experiment where a supersaturated solution existed. Explain. 3. Was the KCl sample under Condition A unsaturated, saturated, or supersaturated? How do you know? 4. Was the KCl sample under Condition Dunsaturated, saturated, or supersaturated? Explain your observation that confirms your answer. Part II. Solubility and Structure Observations- Observations- Conclusion-Predict whether the substance is ionic, nolar covalent, Substance
please help with equilibrium reaction and what happens to the OH ions in the solution PART ASSOCIATION/DISSOCIATION OF A PRECIPITATE Data Collection 1. Get a clean test tube and place -1 mL (20-25 drops) of NaOH solution in the tube. 2. Slowly add drops of CaCl, solution until you notice a precipitate form in the tube. 3. Write a net ionic reaction for the formation of the precipitate below as an equilib- rium reaction: -NaOH ans + CaClzrag NaCl +...