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Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7?
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Understanding Buffer Preparation
To prepare a buffer solution with a specific pH, you can use the Henderson-Hasselbalch equation. For the system NH3/NH4Cl, we can express the relationship between pH, pKb, and the concentrations of the base and salt.
Given Parameters
- Desired pH = 9
- Total concentration of base (NH3) and salt (NH4Cl) = 0.06 M
- pKb = 4.7
Calculating pKa
- pKa = 14 - pKb = 14 - 4.7 = 9.3
Using Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation for a base and its conjugate acid is:
pH = pKa + log([Base]/[Acid])
Substituting the values we have:
9 = 9.3 + log([NH3]/[NH4Cl])
Solving for the Ratio
Rearranging gives:
log([NH3]/[NH4Cl]) = 9 - 9.3 = -0.3
This implies:
[NH3]/[NH4Cl] = 10^(-0.3) ≈ 0.5
Finding Concentrations
Let [NH3] = x and [NH4Cl] = y.
From the total concentration:
x + y = 0.06 M
And from the ratio:
x/y = 0.5 → x = 0.5y
Substituting into the total concentration equation:
0.5y + y = 0.06
1.5y = 0.06
y = 0.04 M (NH4Cl)
Thus,
x = 0.5 * 0.04 = 0.02 M (NH3)
Summary of Required Amounts
- Amount of NH3 needed: 0.02 M
- Amount of NH4Cl needed: 0.04 M
This combination will effectively create a buffer solution with a pH of 9.
To prepare a buffer solution with a specific pH, you can use the Henderson-Hasselbalch equation. For the system NH3/NH4Cl, we can express the relationship between pH, pKb, and the concentrations of the base and salt.
Given Parameters
- Desired pH = 9
- Total concentration of base (NH3) and salt (NH4Cl) = 0.06 M
- pKb = 4.7
Calculating pKa
- pKa = 14 - pKb = 14 - 4.7 = 9.3
Using Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation for a base and its conjugate acid is:
pH = pKa + log([Base]/[Acid])
Substituting the values we have:
9 = 9.3 + log([NH3]/[NH4Cl])
Solving for the Ratio
Rearranging gives:
log([NH3]/[NH4Cl]) = 9 - 9.3 = -0.3
This implies:
[NH3]/[NH4Cl] = 10^(-0.3) ≈ 0.5
Finding Concentrations
Let [NH3] = x and [NH4Cl] = y.
From the total concentration:
x + y = 0.06 M
And from the ratio:
x/y = 0.5 → x = 0.5y
Substituting into the total concentration equation:
0.5y + y = 0.06
1.5y = 0.06
y = 0.04 M (NH4Cl)
Thus,
x = 0.5 * 0.04 = 0.02 M (NH3)
Summary of Required Amounts
- Amount of NH3 needed: 0.02 M
- Amount of NH4Cl needed: 0.04 M
This combination will effectively create a buffer solution with a pH of 9.
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Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7?
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Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7?.
Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Find amount of NH3 and NH4Cl needed to prepare a buffer of pH=9 when total con. of base and salt is .06M. pKb=4.7?.
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