- Scan Question
- + Post
- Get Coins
1) Acetic Acid is mixed with water in an experiment. The resulting concentration of H3O+ ions in the reaction at equilibrium (after everything has been mixed) is 0.013M. What is the pH of the new solution at equilibrium?
A neutralization reaction with Acetic Acid and Sodium Hydroxide is run:
CH3COOH + NaOH -> CH3COONa + H2O
When the conjugate base (CH3COONa) concentration is 0.008M and the conjugate acid (CH3COOH) concentration in 0.0032M, what is the pH of the solution?
Ka for CH3COOH is 1.77x10-5.
1) Acetic Acid is mixed with water in an experiment. The resulting concentration of H3O+ ions...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
For the following dissociation of acetic acid, Ka = 1.760 x 10-5: CH3COOH + H2O ? CH3COO- + H3O+ Sodium acetate completely dissociates in solution according to the following reaction: NaCH3COO ? Na+ + CH3COO- A solution was prepared which contains CH3COOH at a pre-equilibrium concentration of 0.05782 M and NaCH3COO at a pre-equilibrium concentration of 0.04991 M. I know all answers, just do not know how to find them. What is the equilibrium concentration of H3O+? (Answer: 0.00002037) What...
please help l, will rate! thabk you!! Why does a solution of a weak acid and its conjugate base act as a better buffer than does a solution of the weak acid alone? The presence of both the acid and the base provides a significant concentration of both an acid and a base, making it harder to change the pH A solution of a weak acid alone has no base present to absorb added acid. The presence of both the...
please show all work neatly 5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...
I. REACTION EQUILIBRIUM IN NON-IDEAL SYSTEMS The acetic acid (CH:COOH) aqueous solution with a concentration of 0.1 mol/kg has a hydrogen ion concentration of 1.35x10-3 mol/kg. i. Write the acid dissociation equation. ii. Calculate the acid dissociation constant, Ka, considering the ionic activity. jïi. Calculate the pH of the acidic solution. iv. What is the new pH if the solution contains 0.1 mol CH3COOH and 0.4 mol of sodium acetate, CH3COONa, in 1.0 L of water? Consider the negligible quantitities....
Acetic acid (CH3COOH,CH3COOH, ?a=5.62×10−5)Ka=5.62×10−5) is a weak acid, so the salt sodium acetate (CH3COONa)CH3COONa) acts as a weak base. Calculate the pH of a 0.445 M0.445 M solution of sodium acetate.
A 7.00 mL aliquote of acetic acid was mixed with water and the resulting solution was titrated with 0.250 M NaOH. It took 40.2 mL of base to reach the equivalence point. What was the concentration of the acetic acid? 1) 0.043 M 2) 0.070 M 3) 0.143 M 4) 1.43 M
1) Calculate the pH in the titration of 50.00 mL of 0.060 M acetic acid (CH3COOH) with a 0.120 M sodium hydroxide, NaOH solution after the addition of the following volumes of base: Ka for acetic acid = 1.8 x 10-5 A) 0 mL pH = B) 10 ml pH =
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
You are provided with 100 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5), which you will be asked to titrate with 0.050 M sodium hydroxide (NaOH). (a) What is the pH after the addition of 80 mL of the 0.050 M sodium hydroxide solution? Show your work. In your answer, show the reaction that occurs when the sodium hydroxide is added. (b) What is the pH at of the solution at the equivalence point (where the...