D Question 6 1 pts When equal volumes of the solutions are combined, which of the...

Question

Question

Answer 1

Answer #1

6). Largest buffer capacity produce when weak acid react with its conjugate base or weak base reacts with its conjugate acid.

In the given example 1.0M HF and 1.0M LiF have higher buffer capacity as HF is a weak acid and LiF is its conjugate base.

Ans:- 1.0M HF and 1.0M LiF

7). HBr is a strong acid and NH3 is weak base. When equal volume of these 0.50 M mixed together resultant solution will be acidic in nature.

Ans:- Weakly acidic

Answer 2

Similar Homework Help Questions

D Question 6 1 pts When equal volumes of the solutions are combined, which of the...

D Question 6 1 pts When equal volumes of the solutions are combined, which of the following produces a solution with the largest buffer capacity? O 10MHNO, and 10M NOH O 10M NaF and 10M NOH 1.0MHF and 10M NAOH O 20 MHNO, and 20 M LINO, O 10M HF and 1.0 MUF
Question 7 1 pts Equal volumes of 0.50 M HBr and 0.50 M NH3 are mixed...

Question 7 1 pts Equal volumes of 0.50 M HBr and 0.50 M NH3 are mixed together. The resulting solution can be best described as: a buffer weakly basic weakly acidic. O neutral
Which of the following aqueous solutions produce a buffer when equal volumes are mixed together? a)...

Which of the following aqueous solutions produce a buffer when equal volumes are mixed together? a) 0.10 M HF + 0.10 M NaF b) 0.10 M NaOH + 0.10 M NaF c) 0.10 M HF + 0.10 M HCl d) 0.10 M KF + 0.10 M NaF

Which of the following combinations can be used to make a buffer? (Assume equal volumes are...

Which of the following combinations can be used to make a buffer? (Assume equal volumes are used.) Question 6 of 14 Submit Which of the following combinations can be used to make a buffer? (Assume equal volumes are used.) A) 0.50 M HF and 0.20 M NaF B) 0.50 M F and 0.50 M NaOH C) 0.50 M HF and 0.50 M HCI D) 0.50 M HCl and 0.50 M NaF Teams Bachelor TOT ASSOCI Type here to search O...
10. Which of the following mixtures has lower pH a) Equal volumes of 0.10M HCIO, and...

10. Which of the following mixtures has lower pH a) Equal volumes of 0.10M HCIO, and 0.10M NaOH b) Equal volumes of 0.10M HCIO and 0.10M NH Ans: 1. Does the pH increase, decrease or remain same on addition of each of the following a) NH4NO) to NHs solution Ans: b) Na:CO) to NaHCO3 solution Ans: c) NaCIO4 to NaOH solution Ans: 12. Which of the following solutions give a buffer solution when equal volumes are mixed? a) 0.10M NaF...
Which of the following gives a buffer solution when equal volumes of the two solutions are...

Which of the following gives a buffer solution when equal volumes of the two solutions are mixed? Check all that apply. Check all that apply. 0.10 M NH4Cl and 0.10 M NH3 0.10 M NH3 and 0.10 M HCl 0.20 M NH3 and 0.10 M HCl 0.20 M NH4Cl and 0.10 M NaOH

HAc has Ka = 1.8 10-5, and HF has Ka = 7.2 10-4. If equal volumes...

HAc has Ka = 1.8 10-5, and HF has Ka = 7.2 10-4. If equal volumes of 1 M solutions of HAc and the salt, NaF, are mixed together, the resulting solution would be: A. acidic B. basic C. neutral
4. Which of the following mixtures would result in buffered solutions when 1.0 L of each...

4. Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two solutions is combined? Circle the letter of the appropriate response(s) d. 1.0 M NH3 and 1.0 M NH4 Cl e. 1.0 M NH3 and 0.50 M HCI f. 1.0 M HNO3 and 0.50 M NaOH a. 1.0 M HBr and 1.0 M NaBr b. 2.0 M HF and 1.0 M NaOH c. 1.0 M HF and 1.0 M NaOH
Question 8 Select any and all of the following that would create a buffer if you...

Question 8 Select any and all of the following that would create a buffer if you combined them in equal volumes. None of these 1.0 M NH3 and 1.0M NHACI 1.0 MCH3COOH and 1.0 M NaCH3COO 1.0 MCH3COOH and 10 M NaOH 1.0 M HCI and 1.0 M NaCl N Previous

1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained...

1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...