**Designing a Buffer with a pH of 7.24**To create a buffer with a pH of 7.24 using one of the given weak base/conjugate acid systems, consider the following data:| Weak Base | \(K_b\) | Conjugate Acid | \(K_a\) | \(pK_a\) ||-----------------|-----------------|--------------------|------------------|----------|| \(CH_3NH_2\) | \(4.2 \times 10^{-4}\) | \(CH_3NH_3^+\) | \(2.4 \times 10^{-11}\) | 10.62 || \(C_6H_{15}O_3N\)| \(5.9 \times 10^{-7}\) | \(C_6H_{15}O_3NH^+\) | \(1.7 \times 10^{-8}\) | 7.77 || \(C_5H_5N\) | \(1.5 \times 10^{-9}\) | \(C_5H_5NH^+\) | \(6.7 \times 10^{-6}\) | 5.17 |### Problem Statement:Determine the number of grams of the bromide salt of the conjugate acid and the grams of the weak base required to produce 1.00 L of a buffer that has a concentration of 1.00 M in the weak base.### Calculation Steps:1. **Select the Buffer System:** - Choose a system where the \(pK_a\) is close to the desired pH of 7.24. In this case, \(C_6H_{15}O_3N\) / \(C_6H_{15}O_3NH^+\) is the most suitable with a \(pK_a\) of 7.77.2. **Henderson-Hasselbalch Equation:** - \[ \text{pH} = pK_a + \log\left(\frac{[A^-]}{[HA]}\right) \] - Substitute the values: \[ 7.24 = 7.77 + \log\left(\frac{[C_6H_{15}O_3N

Answered: Image /qna-images/answer/8791fd26-4f85-450c-a953-90fbbfb53802.jpg

Design a buffer that has a pH of 7.24 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pka CH3NH2 4.2 x 10-4 CH3NH3* 2.4 x 10-11 10.62 C6H1503N 5.9 x 10-7 C6H1503NH* 1.7 x 10-8 7.77 C5H5N 1.5 x 10-⁹ C5H5NH+ 6.7 x 10-6 5.17 How many grams of the bromide salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams bromide salt of conjugate acid = grams weak base =

Design a buffer that has a pH of 7.24 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pka CH3NH2 4.2 x 10-4 CH3NH3* 2.4 x 10-11 10.62 C6H1503N 5.9 x 10-7 C6H1503NH* 1.7 x 10-8 7.77 C5H5N 1.5 x 10-⁹ C5H5NH+ 6.7 x 10-6 5.17 How many grams of the bromide salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams bromide salt of conjugate acid = grams weak base =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.10 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)
Design a buffer that has a pH of 4.66 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 × 10-5 4.19 H2PO4- HPO42- 6.2 × 10-8 7.21 HCO3- CO32- 4.8 × 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams potassium salt of weak acid = grams potassium salt of conjugate base =
Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10
Pp
What steps would you take (including amounts) to create a buffer of pH = 2.64 using only K₂PO4. KH₂PO4. K₂HPO4. and H₂PO4 H₂PO4 H+H₂PO4 H₂PO4 H+HPO42 HPO4 ² H+ + PO43 Ka1 = 7.5*10³ Ka2 = 6.2 10.8 K3 = 4.8 10-13
determine the volume of 0.2 M sodium acetate required to be added to prepapre 100 mL of 0.2 M acetate buffer at ph 4.2? Use the table as a reference.
If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5
So I have the correc answer
Which of the following will produce a buffer solution when mixed? 50.0 mL 0.500 M HNO3 + 50.0 mL 0.250 M CH3NH3CI 50.0 mL 0.250 M KOH + 50.0 mL 0.500 M CH3NH3CI 50.0 mL 0.500 M KOH + 50.0 mL 0.500 M CH3NH3CI 50.0 mL 0.500 M HNO3 + 50.0 mL 0.500 M CH3NH2
Do
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH
Calculate the pH of NH3/NH4Cl 1- The 0.2M NH3/0.2M NH4Cl buffer. 2- After the addition of 0.08 mol NaOH Given: Ka (NH4+/NH3) = 5.6 * 10-6