A buffer solution of acetic acid and sodium acetate reacts with hydrochloric acid (or sodium hydroxide) according to the reactions below. Calculate the pH of 70.0mL of a buffer solution formed from 3.0 M sodium acetate and 4.0 M acetic acid after the addition. Don't forget - use moles instead of Molarity Ⓒ HCI+ NaC₂H302→ NaCl +HC₂H3O₂ NaOH + HC₂H302 → H₂O + NaC2H3O2 Moles HCI or NaOH PH 10.0 mL of 3.00 M HCI 30.0 mL of 3.00 M HCI 60.0 mL of 3.00 M HCI 10.0 mL of 3.00 M NaOH 30.0 mL of 3.00 M NaOH 60.0 mL of 3.00 M NaOH pH = pka + log pH =pKa + log salt + base acid-base) salt-acid- acid + acid,

A buffer solution of acetic acid and sodium acetate reacts with hydrochloric acid (or sodium hydroxide) according to the reactions below. Calculate the pH of 70.0mL of a buffer solution formed from 3.0 M sodium acetate and 4.0 M acetic acid after the addition. Don't forget - use moles instead of Molarity Ⓒ HCI+ NaC₂H302→ NaCl +HC₂H3O₂ NaOH + HC₂H302 → H₂O + NaC2H3O2 Moles HCI or NaOH PH 10.0 mL of 3.00 M HCI 30.0 mL of 3.00 M HCI 60.0 mL of 3.00 M HCI 10.0 mL of 3.00 M NaOH 30.0 mL of 3.00 M NaOH 60.0 mL of 3.00 M NaOH pH = pka + log pH =pKa + log salt + base acid-base) salt-acid- acid + acid,

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

See similar textbooks

Similar questions

A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.
Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?
A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)
1. Pure water is neutral in pH or has a pH value of exactly 7.00. How does the pH of pure water vary when it undergoes distillation and boiling? Show the important equations if necessary, to explain why distilled and boiled water deviate from the neutral pH. 2. Some distilled water showed pH of 9.00 or marketed as alkaline water. What is the procedure involved in converting the pH of neutral water to basic? Show the necessary equations if possible. Can alkaline water help in the treatment of hyperacidity and gastroesophageal reflux disease? Explain your answer.