Chemistry, 26.06.2020 15:01 haileymaree

Calculate the following buffer solutions. A buffer solution was made by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.00 M acetic acid. Assuming the change in volume when the sodium acetate is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. The Ka for acetic acid is 1.7 x 10-5. Calculate the ratio of ammonium chloride to ammonia that is required to make a buffer solution with a pH of 9.00. The Ka for ammonium ion is 5.6 x 10-10. After completing the calculations answer the following questions 1) Is the pH of the solution consistent with the Ka or is there a better Ka that could be used? 2) If 100 mL of buffered solution is used, what is the pH change if 20 mL of 0.5M HCl is added? Does the pH change exceed the buffering capacity of the solution? Explain 3) If 100 mL of buffered solution is used, what is the pH change if 20 mL of 0.5M NaOH is added? Does the pH change exceed the buffering capacity of the soltuion? Explain

Answers: 2

Show answers

Another question on Chemistry

Chemistry, 21.06.2019 16:40

Which of the following is a testable hypothesis? a. if i brush my teeth, i will get fewer cavities than if i don't brush my teeth. b. green toothpaste tastes better than blue toothpaste or red toothpaste. c. smart, careful, healthy people always brush their teeth. d. it's wrong to not brush your teeth before you have an important conversation with someone.

Answers: 1

Answer

Chemistry, 22.06.2019 14:30

What type of reaction fuels the processes seen here?

Answers: 2

Answer

Chemistry, 22.06.2019 16:30

For the reaction shown, calculate how many moles of no2 form when each of the following completely reacts. 2n2o5(g)→4no2(g)+o2(g) part a 1.0 mol n2o5 express your answer using two significant figures. nothing mol m o l request answer part b 5.4 mol n2o5 express your answer using two significant figures.

Answers: 2

Answer

Chemistry, 22.06.2019 16:50

Answer asap need by wednesday morning explain how a buffer works, using an ethanoic acid/sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.

Answers: 1

Answer

You know the right answer?

Calculate the following buffer solutions. A buffer solution was made by dissolving 10.0 grams of sod...

Questions