[Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is 0.337 M in H₂S and 0.280 M in NaHS. If Kal for H₂S is 1.0 x 10-7, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group No more group attempts remain
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- Buffer solution of 0.5 M acetic acid and 0.4 M sodium acetate (Ka = 1.7e-5) 0.4 0.5 0.8 4.67 4.77 1.7e^(-5) 2.1e^(-5) 4.7e^(-10) 5.9e^(-10) 9.23 9.33 None Give the value of these examples Conjugate Acid, Conjugate base, Molar Ratio, pOH, Salt, [H+], [OH-], pKa, and the acid (there answers are given above)Which of the following solutions represent(s) a buffer solution? Explain.(a) 15 cm3 of 0,1 mol.dm–3 NaOH(b) 15 cm3 of 0,1 mol.dm–3 HC2H3O2(c) 30 cm3 of 0,1 mol.dm–3 NaOH and 30 cm3 of 0,1 mol.dm–3 HC2H3O2(d) 30 cm3 of 0,1 mol.dm–3 NaOH and 60 cm3 of 0,1 mol.dm–3 HC2H3O2How to answer for Ka/ Kb and calculated pH of a solution?I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Given: In a 10.0 mL 0.10 M CH3COOH solution, a 15 mL 1.00 M HCl solution was added. Compute for it's ka/kb and pH.
- Calculate [OH⁻] in a solution obtained by adding 1.50 g solid KOH to 1.00 L of 10.0 M NH₃. (Kb of NH₃ is 1.80 × 10⁻⁵). (do not provide AI based content otherwise i dislike)Which of the following, if dissolved in 1.0 L of pure water, will produce a buffer solution? 0.1 mole HCL + 0.1 mole KCl 0.1 mole NaH2PO4 + 0.1 mole Na2HPO4 0.1 mole NaCl + 0.1 mole KCl 0.1 mole of H3O+ + 0.1 mole OH- I am guessing option 2, but need clarification please!Good evenig, Earlier I submitted this problem to try and receive some help with understanding the correct way to answer, but it wasn't correct, and I still lack understanding of how to execute this problem. Would you be able to help me? Thank you. Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq) with 0.200 M KOH(aq). Use the ionization constant for HClO. What is the pH before addition of any KOH? pH= What is the pH after addition of 25.0 mL KOH? pH= What is the pH after addition of 40.0 mL KOH? pH= What is the pH after addition of 50.0 mL KOH? pH= What is the pH after addition of 60.0 mL KOH? pH=
- Really hoping for solutions since I’m having a hard time with this. Pls. skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced. A. What mass of NaCH3COO should be added to 1.00 L of 0.100 M CH3COOH to produce a solution with pH = 5.00? Assume that the volume remains 1.00 L. Include your analysis of the problem and assumptions if any. Make sure your final answer has correct significant figures. B. For another experiment, you will need a buffer at pH 5.2. Outline steps you will do to adjust the pH of the buffer you made in A to pH 5.2. Show your calculations.calculate the amount of NaH2PO4 needed for a 100mL buffer solution with a pH of 7.33 and a concentration of sodium phosphate monobasic of 0.014Please Calculate the mass of sodium acetate trihydrate (CH3COONa●3H2O) solid and thevolume of 1.00 M acetic acid (CH3COOH) required to make 250.0 mL of 0.100 M buffer, pH 5.00 Thank you!
- Give good explanation Asap Thanks You have a 0.10 M aqueous NH3 solution. Calculate a) the number of moles and b) the number of grams of NH4Cl that must be added to 500 ml. of this solution to obtain a buffer solution of pH = 9.15 Neglect the volume change from the addition of solid NHCl.enumerate the steps necessary to create a Phosphate Buffer NaH2PO4 - K2HPO4 with a final volume of 500 mL, a concentration of 0.10M, and a pH of 7.20 using 0.20 M NaH2PO4 and solid K2HPO4. Nota bene: Ka equals 6.3 x 10-8. (show computation as well) For solid K2HPO4, calculate for the mass (based from calculated moles of salt) rather than the volume since this is a solid substance.H8. Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion