a)
Here mol of HF and NaOH is equal.
Both will react and form F-.
But there will not be any HF.
So, it cant form buffer
b)
Here, mol of HNO2 and mol of OH- is same.
So, all HNO2 will react
So, it cant form buffer
c)
Mol of NaOH is more than mol of CH3CO2H.
So, finally, there will be NaOH and CH3CO2Na.
They are both basic.
They will not form buffer
d)
Amount of base is less than amount of HF.
So, some of HF will react with all of NaOH to form some F-.
At the end there would be HF and F-.
It form basic buffer.
Answer: d
please explain. PRACTICE 1: Which of the following combinations can result in the formation of a...
Which of the following combinations can be used to make a buffer? A) 0.20 M NH3 and 0.20 M HCI B) 0.20 M NH3 and 0.10 M NH4CI C) 0.20 M NH3 and 0.10 M HF D) 0.10 M NH4CI and 0.10 M NaF
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...
Which of the following combinations can be used to prepare a buffer? a) HCNaCI b) HF/KF c) NH3/NH4C d) HNO3/HNO2 e) NaNO2/HNO3 17.2.1
I am confused on how buffers work.
Which of the following combinations can be used to make a buffer? A) 0.20 M NHz and 0.20 M HCI B) 0.20 M NH3 and 0.10 M NH_CI C) 0.20 M NHz and 0.10 M HF D) 0.10 M NH Cl and 0.10 M NaF
Please explain.
PRACTICE 1: Which one of the following combinations does not create a buffer? a) HC2H302 and K C2H302 b) H2SO3 and NaHSO3 C) H3PO4 and NaH2PO4 d) HNO3 and KNO3 e) NH4Cl and NH3
please help me with all the steps.
15. Which of the following mixtures would result in a buffered solution? a. Mixing 100.0 mL of 0.100 M HCl with 100.0 mL of 0.100 M NaOH. b. Mixing 100.0 mL of 0.100 M NH3 (K5=1.8 x 10-5) with 100.0 mL of 0.100 M NaOH. c. Mixing 100.0 mL of 0.100 M HCl with 100.0 mL of 0.100 M NH; (K =18x 10 %. d. Mixing 50.0 mL of 0.100 M HCl with...
12.59 Place the following solutions in order of increasing [H3O+]. Please explain your reasoning. 0.10 M HF, 0.10 M NH3, 0.10 M HNO3 0.10 M HCN, 0.20 M HCN, 0.20 M HClO4 0.10 M NH3, 0.10 M NaOH, 0.10 M Ca(OH)2
Question 3 4 pts Which of the following mixtures would result in a buffer situation. Select ALL correct answers. 100 mL 0.1 M HNO3 mixed with 50 mL 0.1 M NH3 100 mL 0.1 MHCIO4 mixed with 50 mL 0.1 M NH4CI 100 mL 0.1 MHCI mixed with 50 mL 0.1 M NH3 100 mL 0.1 MHF mixed with 50 mL 0.1 M NaOH 50 mL 0.05 M KOH mixed with 50 mL 0.1 M NH4Br 100 mL 0.2 MHCIO2...
Can someone please help me solve these, please show
work/explanation and answer!
The directions say that they are predominant species and that
I must explain my answer.
11. Which of the following best describes the composition of a solution labeled "0.10 M NaOH"? a. (NaOH) = 0.10 M b. [Na] < 0.10 M, [OH-] <0.10 M C. (Na+) = 0.10 M, [OH-] = 0.10 M d. [Na+] = 0.10 M, [H] = 0.10 M, [02] = 0.10 M e. [Na]...
Which of the following combinations would make a buffer with pH close to 3.0? HClO2 Ka = 1.1 × 10-2 NH3 Kb = 1.8 × 10-5 HNO2 Ka = 7.2 × 10-4 C5H5N Kb = 1.5 × 10-9 Equal volumes of 0.10 M NH4Cl and 0.10 M NH3 Equal volumes of 0.10 M HClO2 and 0.10 M NaClO2 Equal volumes of 0.10 M HNO2 and 0.10 M NaNO2 Equal volumes of 0.10 M HCl and 0.10 M NaCl Equal volumes...