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please show work 9.45.0 mL of 1.023 M HCOOH is titrated with 0.740 M LIOH. What...
9.45.0 mL of 1,023 M HCOOH is titrated with 0.740 M LIOH. What is the pH after 30.0 mL of LiOH has been added? The K. of HCOOH is 1.80 x 10-4 (11 points)
8.15.0 mL of 0.475 M CH3COOH is titrated with 0.450 M ROOH. What is the pH after 18.0 mL of RbOH has been added? The K, of CH3COOH is 1.80 x 109. (10 points)
8. 15.0 mL of 0.475 M CH3COOH is titrated with 0.450 M ROOH. What is the pH after 18.0 mL of RbOH has been added? The K, of CH3COOH is 1.80 x 10-9. (10 points)
A 50.0 mL sample of 0.25 M formic acid (HCOOH) aqueous solution is titrated with 0.125 M NaOH solution. Ka of HCOOH = 1.7 x 10−4. a. Calculate the pH of the solution after 50 mL of NaOH solution has been added. b. How many mL of 0.125 M NaOH need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?
3) (10 points total) A 25.0-mL sample of 0.35 M HCOOH (formic acid) is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka-1.77 x 10 a) (4 points) What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ks-1.77 x 10 C 2-l04Co1s5 b) (6 points) Calculate at least nine (9) more titration points, build a table...
20.00 mL of 3.000 M butanoic acid(C4H2O2)is titrated with 0.7000 M LIOH. Find the pH of the solution of the following points in the titration: Kabutanoic acid = 1.5 X 10-5 A. Before any base is added: B. When half the butanoic acid has been neutralized:
. A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution at the following conditions below: a. before the addition of any LiOH. b. after the addition of 30.0 mL of LiOH. c. after the addition of 50.0 mL of LiOH. d. after the addition of 66.67 mL of LiOH e. after the addition of 75.0 mL of LiOH. f. after the addition of 100.0 mL of LiOH.
X and Y ,000 wu A 30.0-ml sample of 0.20 M HCOOH was titrated with 0.20 M NaOH. The following data were collected during the titration ml NaOH 5.00 10.00 15.00 20.00 25.00 added pH 13.07 4.77 3.47 3.77 029 X. OME.006 mole HTOOT What is the Ka for HCOOH? 20 X. DUS = .00+ mol Nao 4.07 loot A B. C. D. 1.1 x 10-7 005 1.7 x 104 1.2 x 10-8 4.9 x 10-11 None of these choices...
A 74.0 mL sample of 0.0400 M HNO3 is titrated with 0.0800 M LiOH solution. Calculate the pH after the following volumes of base have been added. (a) 11.8 mL pH = (b) 36.3 mL pH = (c) 37.0 mL pH = (d) 38.9 mL pH = (e) 59.2 mL pH =
A 25.00 mL sample of 0.280 M LiOH is titrated with 0.750 M HI at 25 °C. Calculate the initial pH before any titrant is added. pH = Calculate the pH of the solution after 5.00 mL of the titrant is added. pH =