▼ Which of the following buffer systems would be the best choice to create a buffer with pH = 9.05? HF/KF HNO2/KNO2 NH3/NH4Cl OHCIO/KCIO Submit Previous Answers ✓ Correct The best buffer will be the one whose weak acid component has a pK, closest to the desired pH of the buffer. Since the pK₂ of NH4+ is 9.25, and the desired buffer pH is 9.05, the best choice for the buffer is NH3/NH4Cl. 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. [5] ΑΣΦ m (NH3) m (NH,CI) 3 → ?

▼ Which of the following buffer systems would be the best choice to create a buffer with pH = 9.05? HF/KF HNO2/KNO2 NH3/NH4Cl OHCIO/KCIO Submit Previous Answers ✓ Correct The best buffer will be the one whose weak acid component has a pK, closest to the desired pH of the buffer. Since the pK₂ of NH4+ is 9.25, and the desired buffer pH is 9.05, the best choice for the buffer is NH3/NH4Cl. 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. [5] ΑΣΦ m (NH3) m (NH,CI) 3 → ?

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

A buffer is made up of 15.0 mL of 0.1 M HC2H3O2 and 15.0 mL of 0.1 M N a C2H3O2. The pH of the buffer solution is 4.71. What is the pKą? HINT : Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB)
Find the pH of the following buffer solutions: 100 M in acetic acid (HC2H3O2) and 0.100 M in sodium acetate (NaC2H3O2) 16 M in NH3 and 0.22 M in NH4Br 50 mL of 0.15 M HCHO2 with 75.0 mL of 0.13 M NaCHO2
Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl 10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH 10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO
The pK₂ value for HCN is 9.40. Would a buffer prepared from HCN and NaCN with a pH of 7.60 be considered to be an effective buffer? A buffer in which the mole ratio of NaCN to HCN is 2.0 has a pH of 9.71. Would this buffer solution have a greater capacity for added acid ( H3O+) or added base (OH)?
A buffer is made with 0.50 M weak acid and 0.50 M sodium salt of the conjugate base. The pKa of the weak acid is 9.30 After the addition of a small amount of strong concentrated acid, the new equilibrium concentrations are 0.6 M weak acid and 0.4 M base. Calculate the new pH. Enter result with 2 decimal places, digits only.
5
answer pls
A buffer made of weak acid [WA] and its conjugate base [CB] is most effective when a)pH = pKa of the weak acid b)its concentration is high c)[WA] = [CB] d)all of the choices are correct
Calculate the pH of a buffer that is 0.280M in NaHCO3 and 0.330M in Na, CO. Express your answer to two 2 3 decimal places. pH = Request Answer Part B Calculate the pH of a solution formed by mixing 65mL of a sctution that is 0.23M in NaHCO3 with 75mL of a solution that is 0.18M in Na 2 CO 3. Express your answer to two decimal places. pH = Request Answer Provide Feedback
If a small amount of a strong base is added to a buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solution does not change appreciably because the strong base reacts with A- to give H2O no reaction occurs the strong base reacts with A- to give HA the strong base reacts with HA to give A- rhe Ka of HA has changed
What is the [H3O+] and the pH of a buffer that consists of 0.52 M HNO2 and 0.87 M KNO2? (Ka of HNO2 = 7.1 × 10−4) [H3O+] ______ pH ______