Part A Submit MyAnswers GiveUp Correct Part B For the best system, calculate the

Question

Part A

SubmitMyAnswersGiveUp

Correct

Part B

For the best system, calculate the ratio of the masses of the buffer components required to make the buffer.

Express your answer using two significant figures.

SubmitMyAnswersGiveUp

Need help on Part B please!

Part A Which of the following buffer systems would be the best choice to create a buffer withpH= 9.00? {rm HF}/{rm KF} {rm{HNO}}_2 / {rm{KNO}}_2 {rm{NH}}_3 /{rm{NH}}_4 {rm{Cl}} {rm HClO}/{rm KClO} Part B For the best system, calculate the ratio of the masses of the buffer components required to make the buffer. Express your answer using two significant figures.

Explanation / Answer

HF/KF; HNO2/KNO2; HClO/KClO are all weak acid systems. They would give a buffer with pH < 7.0.

The only system which will give a basic buffer solution (pH > 7.0) is the NH3/NH4Cl since NH3 is a weak base.

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.