1) A) A buffer solution made from acetic acid (HCH3CO2) and sodium acetate (NaCH3CO2) was titrated with hydrochloric acid ? B) A buffer solution made from nitrous acid and sodium nitrite was titrated with sodium hydroxide. What is the net ionic equation for the reaction?
2) Which of the following pairs will not form a buffer solution? A ) H3PO4/KH2PO4 B) NH3/ NH4Cl C) KOH, HCl D) HC2H3O2/ NaOH E) KOH/ HF
1) A) A buffer solution made from acetic acid (HCH3CO2) and sodium acetate (NaCH3CO2) was titrated...
For a buffer made from sodium acetate and acetic acid, the Ka of acetic acid is 1.8E-5. What mass of sodium acetate (NaCH3CO2) must be added to 2.50 L of 0.68 M acetic acid to make a buffer solution with pH = 5.75? The answer should be in two significant figures.
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab was prepared using the following components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M HC2H3O2 55.0 mL of water If you take half of this solution and add 2 mL of 1.00 M HCl to it, then what is the pH of this new solution?
D. Buffers 1. A buffer solution was made by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.50 M acetic acid. Assuming the change in volume when the sodium acetate is added is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. The K, for acetic acid is 1.8 x 105. 2. Calculate the pH of a buffer solution that initially consists of 0.0400 moles of ammonia and 0.0250 moles of ammonium ion, after 20.0...
calculate the buffer capacity of an acetate buffer made with 50mL 0.4M acetic acid and 0.4M sodium acetate. it's initial pH was 4.67 and adding 0.2M of NaOH to a 20mL sample of the acetate buffer. then find the buffer capacity when adding 0.2M HCl to a 20mL sample of the acetate buffer.
38) A buffer is made that contains 0.50M acetic acid and 0.50M sodium acetate. To a 10o.0mL sample f the buffer 50.0 mL of 0.50M NaOH is added. What is the pH of the new solution? (K, 1.8x 10 for acetic acid) a) 5.11 b) 5.22 c) 5.33 d) 5.44 e) 5.55
A) A buffer containing acetic acid and sodium acetate has a pH of 5.45. The Ka value for CH3CO2H is 1.80 × 10-5. What is the ratio of the concentration of CH3CO2H to CH3CO2-? [CH3CO2H]/[ CH3CO2-] = _________ B) What is the pH change when 29.6 mL of 0.117 M NaOH is added to 95.4 mL of a buffer solution consisting of 0.123 M NH3 and 0.179 M NH4Cl (Ka for ammonium ion is 5.6x10^-10.) pH change =_______
QUESTION 10 Which of the following compounds could you mix with acetic acid (HCH3CO2) to create a buffer? Potassium acetate (KCH3CO2) Sodium bicarbonate (NaHCO3) Hydrochloric acid (HCI) Ammonia (NH3) Nitric acid (HNO3)
QUESTION 10 Which of the following compounds could you mix with acetic acid (HCH3CO2) to create a buffer? Ammonia (NH3) Hydrochloric acid (HCI) Sodium bicarbonate (NaHCO3) Potassium acetate (KCH3CO2) Nitric acid (HNO3)
A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 2.00 mL of a 1.00 M solution of hydrochloric acid is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5. What is the pH of HCl?
Which of the following cannot be a buffer solution? Group of answer choices 1.0-L solution, in which 0.10 mol acetic acid (CH3COOH) and 0.050 mol potassium hydroxide (KOH) are dissolved. 0.50-L solution, in which 0.25 mol ammonia (NH3) and 0.18 mol hydrochloric acid (HCl) are dissolved. 0.75-L solution, in which 1.0 mol hydrofluoric acid (HF) and 2.0 mol sodium hydroxide (NaOH) are dissolved. 1.0-L solution, in which 3.0 mol lithium hydroxide (LiOH) and 5.0 mol formic acid (HCOOH) are dissolved....