what titrant will you use in preparing a substance with a pH of 7(green) whereupon the addition of bromothymol blue, has turned yellow instead?
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what titrant will you use in preparing a substance with a pH of 7(green) whereupon the addition of bromothymol blue, has turned yellow instead?
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- 5) Determine the ratio in which sodium acetate and acetic acid must be mixed to give a solution that is buffered at pH 6.500.Write net ionic equations for the reactions responsible for the observed pH value for each of the following solutions. For each of the four solutions, explain why the observed color change with bromcresol green reasonable given the pH. NaCl; pH=7 Na2CO3; pH =10.8 NaC2H3O2; pH=8.9 NaHSO4; pH=1.5Which of the following would be the best choice of a buffering system at pH 6.0? (a) H2SO4/HSO4-(b) Lactic Acid/Lactate(c) Carbonic Acid/Carbonate (d) Ammonium/ammonia
- A buffer is made with sodium acetate (CH3COONa) andacetic acid (CH3COOH); the Ka for acetic acid is 1.80 x 10-5.The pH of the buffer is 3.98. What is the ratio of the equilibriumconcentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informationis given to answer this question.8. (a) How many grams of ammonium bromide would have to be added to exactly 500 cm³ of 0.10 M NH3 solution to have a pH of 8.5. I (a) How many grams of sodium acetate must be added to 0.100 dm³ of 0.2 M acetic acid to give a pH of 4.0?Which of the following pairs of solution would you use to prepare a buffer with pH = 7.45? (A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5) (B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8) (C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5) (D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)
- 8-39. (a) Write the chemical reactions whose equilibrium constants are K and K for imidazole and imidazole hydrochloride, respectively. (b) Calculate the pH of a solution prepared by mixing 1.00 g of imida- zole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. (c) Calculate the pH of the solution if 2.30 mL of 1.07 M HC1O4 are added.When 1.40 moles of Br2 are put in a 0.960−L flask, 1.10 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.O7) what is the pH at the equivalent point in the titration of 5 mmol Potassium acid phthalate dissolved in 100 d of water and titrated with o.1M NaOH 9 K,= 4 +r06 Ans.: 8.96
- An analytical chemest is titrating 150.6 ml. of a 0.6600 M solution of dhethylamine (C,H,) NH) wth a 0.1500M solution of HIO, The p K, of dethylamine is 2.89. Cakculate the pH of the base solution after the chemest has added 7773 ml. of the HIO, sohuton to . Note for advanced students: you may assume the fnal vokume equals the intal volume of the solution plas the volume of HIO, sokaton added. Round your answer to 2 decimal places please explain and solvelIn a titration of 50.00 mL of 0.1000 M ethylamine with 0.1000 M HClO4, the titration error must be no more than 0.05 mL. What indicator can be chosen to realize this goal?The reaction Cu(s) + HNO3(ag) Cu(NOsh(ag) + 2 NO:) +2 H;O() is used to dissolve the copper metal Ifa 1.000 g sample of copper is used, and instructions say to use four times as much acid as the required amount, how many mL (to the nearest mL) of 15.0 M nitric acid would be used in the procedure for this sample? Select one: O a 10mL Ob 17ml O c.4mL O d 25ml O e 5mL