What is the OH- concentration when 20.0 mL of 0.100 M HNO2 is titrated with 20.0 mL of 0.100 M NaOH? The Ka for HNO2 is 4.5×10-4.
What is the OH- concentration when 20.0 mL of 0.100 M HNO2 is titrated with 20.0...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
. 20.0 mL of 0.100 M lactic acid solution is titrated with 0.100 M NaOH solution. Calculate the pH of the contents of the Erlenmeyer flask at each of the following points during the titration. (a) When 0.00 mL of NaOH have been added. (2) (b) After 5.00 mL of NaOH have been added. (3) (c) After 20.0 mL of NaOH have been added. (3) (d) After 10.0 mL of NaOH have been added. (1) (e) After 25.0 mL of...
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?
A volume of 50.0 mL of 0.100 M CH3COOH(aq) is titrated with 0.100 M NaOH(aq). What is the pH at the equivalence point? (Ka for CH3COOH = 1.8 × 10–5) (1) 7 (2) 5.28 (3) 8.72 (4) 6.34 (5) 4.15
50.0 mL of 0.275 M HNO2 is titrated to its equivalence point with 1.00 M NaOH. What is the pH at the equivalence point? Ka for HNO2 is 4.0x10^-4
At 25.0 mL sample of 0.100 M HClO (aq) is titrated with NaOH (aq). What is the pH of the solution after the addition of 25.00 mL of 0.100 M NaOH? Ka of HClO=3.5*10^-8. The answer might be 4.70 but I don't know. Can anyone explain this problem to me? Full explanation please.
7. Calculate the pH of the solution obtained by titrating 50.0 mL of 0.100 M HNO2(aq) with 0.150 M NaOH(aq) to the equivalence point. Take Ka = 5.6 x 10 - M for HNO2(aq).
9. 100 mL of 0.5M HNO2 (Ka = 4.5*10-4) is titrated with 0.5M KOH. What is the pH after 100mL of 0.5M KOH is titrated into the acid? (12)
4) A 40.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of NaOH: (a) 0,0 mL, (b) 20.0 mL, (c) 40,0 mL, (d) 60,0 mL. A plot of the pH of the solution as a function of the volume of added titrant is known as a pH titration curve. Using the available data points, plot the pH titration curve for the above titration,
A 42.0 mL sample of 0.120 M HNO2 is titrated with 0.214 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH.