Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH,PO4(s) and 28.0 g of Na, HPO4(s) in water and then diluting to 1.00 L. 2.82 pH = Incorrect Answer
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- Hh.83.H2SO4+ 2 NAOH 2 H2O + Na2SO4 If you require 33.35 mL of 0.541 M NaOH solution to titrate 210.1 mL of H,SO4 solution, what is the concentration of the H2SO4 solution? Type answer:Solve #4 please 65 mL of 0.65 M benzoic acid (Ka = 6.4×10-5) is titrated by 0.05 M NaOH. 1)Calculate the pH of the acid solution before any titrant is added. pH = 2.190 2)Calculate the pH after 795.9 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. pH = 12.6603 3)Calculate the pH after 845 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. pH = 12.6625 4)Calculate the pH after 1.58 x 10^3 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. pH = ?
- Q1Question 4 Part A Calculate the pH of a buffer solution that contains 0.750 M CH₂NH₂ and 0.850 M CH₂NH₂Cl. (K. = 4.4x10-4). pH of buffer= Part B 75.0 mL of 1.15 M NaOH is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the NaOH(aq) is added? pH after NaOH added = Part C 80.0 mL of 1.20 M HNO is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the HNO, is added? pH after HNO₂ added: =Which of the following chemicals would be the best buffer for a pH 9.00 solution: NH3 (Kb = 1.75x10-5), C6H5NH2 (Kb = 3.99x10-10), H2NNH2 (Kb = 3.00x10-6), C5H5N (Kb = 1.69x10-9)? Group of answer choices C5H5N H2NNH2 C6H5NH2 NH3
- TUTOR Calculate the Ratio of Acid and Base in a Buffer A buffer containing acetic acid and sodium acetate has a pH of 5.05. The Ka value for CH₂CO₂H is 1.80 x 105. What is the ratio of the concentration of CH3CO₂H to CH3CO₂? [CH3CO₂H]/[ CH3CO₂"]= Submit Submit Answer Show Approach Show Tutor Steps Try Another Version 9 item attempts remainingAn aqueous solution contains 0.414 M ethylamine (C2H5NH2).How many mL of 0.214 M nitric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.500? Answer:_____Consider the following titration curves. The solution in the buret is 0.1 M. The solution in the beaker has a volume of 50.0 mL. Answer the following questions. (a) Is the titrating agent (solution in the buret) an acid or a base? (b) Which curve shows the titration of the weakest base? (c) What is the Ka of the conjugate acid of the base titrated in curve B? (d) What is the molarity of the solution in the beaker for curve C? (e) What is the pH at the equivalence point for curve A?