Assume that you mix equal volumes of the two solutions listed. Select all of the following buffer solutions that have a greater buffering capacity to absorb strong acid than to absorb strong base.
0.10 M HF and 0.10 M NaF
0.10 M HNO2 and 0.040 M KOH
0.20 M CH3NH2 and 0.08 M HCl
0.15 M HBr and 0.35 M NaF
0.20 M HClO and 0.30 M NaClO
0.050 M HCN and 0.020 magnesium hydroxide
0.10 M C6H5NH2 and 0.03 M HCl
Assume that you mix equal volumes of the two solutions listed. Select all of the following...
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
chans the 7. Determine the pH of the following solutions a. 0.040 M HCL ne b. 0.040 M KOH C. 0.0087 M HClO2 d. 0.010 M CH3NH2 (methylamine) e. 0.018 M NaF 0.10
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
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 solutions would have the lowest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A. A) HF, 3.5 × 10-6 B. B) HCN, 4.9 × 10-10 C. C) HNO2, 4.6 × 10-5 D. D) HCHO2, 1.8 × 10-4 E. E) HClO2, 1.1 × 10-2 F. F) none of these
please help!! calculate pH of solutions on second page a-c!! 1. (4 points) A buffer solution is created with C;H,NH, and 0.012 M C;HsNH2. The K, for C,H,NH2 is 4.7 х 104. What is the concentration of C,HNH, in the buffer solution that has a pH of 11.50? а. What is the concentration of the buffer solution if 0.0011 M HC is added to the buffer in part a.? b. Why is the buffer a basic solution? Could this weak...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
Numbers 9-14 are predominant species problems! Explain your answer. Which of the following best describes the composition of a solution labeled "0.10 M H,So"? 9. [H2SO] = 0.10M b. [H]>0.10 M, (So21 -0.10 M c. [H']= 0.20 M, [SO10.10 M d. [H']>0.10 M, [HSO.] <0.10 M e. [H'] 0.10 M, [HSO4] = 0.10 M a. 10. Which of the following best describes the composition of a solution labeled "O.10 M HCI"? [HCI) 0.10 M b. [H]<0.10 M, [CI]< 0.10 M...
36) Which one of the following is not a strong acid? (or a weak electrolyte?) a) HNO )HCI HI )HF e) HCIO Answer: 37) The is the conjugate species that remains after an acid donates a proton is called its conjugate base. What base of the hydronium ion, HO? B)HO C)HO D)H E HO'has no conjugate base. Answer: acid-base pair? 38) For the reaction shown below, which of the following is a conjugate acid A)CHsN, H:0 B) CsH,N, CsH,NH' C)...
Explain why some electrolyte solutions are strongly conducting, whereas others are weakly conducting. 4.2. Def fine the terms strong electrolyte and weak electrolyte. Give an example of each 4.3. Ex plain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound. 4.4. What are the advantages and disadvantages of using a molecular equation to represent an i reaction? 4.5. What is a spectator ion? IlIlustrate with a complete ionic reaction 4.6. What...