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17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH...
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M NaOH is performed. Given that K, for nitrous acid is 4.5 x 104, the pH at 30.00 mL of NaOH added is (a) 1.94 (b) 7.00 (c) 3.35...
2) How many grams of Nat would have to be added to 2.00 Lof 0.100 MHF to yield a solution with a phi 4.00? Assume the volume of the solution remains at 2.00 Lufter the Naf is added. (a) 300 (b) 368 (c) 0.84 (d) 6.98 (e) 60. G 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M N OH is performed. Given that Ka for nitrous acid is 4.5 x 10-4, the pH...
17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. How many grams of HNO3 are in 1 mL of nitric acid? a) 0.99g b) 99g c) 2.1g d) 0.021 g e) 0.49g
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...
10.00 mL Nitric acid was titrated with NaOH of 0.100 molarity until the equivalence was reached. 15.2 mL of NaOH were required. Find: A) Concentration of nitric acid before titration B) pH of solution before titration C) pH of solution after 15.1 mL of sodium hydroxide is added D) pH of solution after 15.3 mL of sodium hydroxide is added
A 25 mL solution of nitric acid, HNO3, required 31.1 mL of 0.1459 M NaOH to reach a bromthymol blue end point. What is the concentration of the nitric acid solution?
A titration is performed between 10.0 mL of 0.100 M of acetic acid and 0.0500 M NaOH. Calculate the pH at the following volumes of added NaOH: 20.00 mL and 25.00 mL. The answers my professor provided are: 8.640, abd 11.854 respectively.
Find the pH during the titration of 20.00 mL of 0.2320 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.2320 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00 mL
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
Consider a titration of 50.0mL sample of 0.500 M HC2H3O2 (a weak acid, which contains 0.0250 moles H3O+) with 0.400 M NaOH (a strong base). Determine the pH of the solution after 15.0 mL of NaOH (0.00600 moles of OH-) is added.