ebration of 20.00 mL of 0.5 M Nibous acid CHND 4.00x 10) aith whon 60.D0mL NaDH...
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...
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
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...
OL 20.00 1 C2 =.936 M 45. 7.00 mL of acetic acid is titrated with NaOH. If 19.2 mL of 0.200 M NaOH is nec equivalence point, what is the concentration of the acid? Macid & Vaida Mo NaOH 19.2 mL = .0192 L 7.00mL needed HC 2 H ₃ Oz NaOH Na C2 H₂O2 + H₂O. 200M HC₂ H₂ O2 + NaOH 2oom ,200 ni 290X 7.0 Mb 7.oom you 19 1. f 450 mL is completely neutralized
Calculate the pH during the titration of 20.00 mL of 0.1000 M HBrO(aq) with 0.2000 M NaOH(aq) after 2 mL of the base have been added. Ka of hypobromous acid = 2.3 x 10-9.
A 250 mL flask contains a 8.0% (m/v) nitric acid solution. Which TWO of the following ratios are NOT equivalent to the concentration? Select one or more: 8g HNO/100 mL soln 20 g HNO3/250 mL soln 80 g HNO/1 L soln 40 g HNO,/0.50 L soln 8 g HNO/1 mL soln 80 mg HN0/1 mL soln 0.08 g HNO/1 mL soln 8 g HNO3/1 L soln
Calculate the pH during the titration of 20.00 mL of 0.1000 M HNO2(aq) with 0.2000 M NaOH(aq) after 6.5 mL of the base have been added. Ka of nitrous acid = 7.1 x 10-4. Show with ICE table and equations
Copy of Calculate the pH during the titration of 20.00 mL of 0.1000 M HNO2(aq) with 0.2000 M NaOH(aq) after 7 mL of the base have been added. Ka of nitrous acid = 7.1 x 10-4.
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
A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 2,421 mL. What is the molarity of nitric acid in the final solution?