Hydrofluoric acid has a Ka of 6.8 x 10-4. In this titration, 20.00 mL of 0.120...
of Hydrofluoric acid (Ka-6.6 x 10") solution is titrated with f NaOH. Draw a titration curve, labeling the initial pH (when no sodium 40. 100 ml ofa 0.3 M olution 0.3 M solution hydroxide has been added), the pH at the mid-point of the titration, and the pH at the equivalence point (16 points). of Hydrofluoric acid (Ka-6.6 x 10") solution is titrated with f NaOH. Draw a titration curve, labeling the initial pH (when no sodium 40. 100 ml...
A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)
When 10.00 mL of 0.240 M HX (Ka = 2.29 x 10') is titrated with 0.120 M KOH, the pH will increase. Calculate the pH of the solution at each point in the titration. The pkw is 14.000 at this temperature. pH Volume of KOH (mL) 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 26.00 28.00
1. 50.00 mL of 0.1000 M propanoic acid (CH3CH2COOH – Ka = 1.34 X 10-5) is titrated with 0.2000 M KOH. Calculate the pH at the following points in the titration: 1) Initial pH – no KOH has been added. 2) 5.00 mL of KOH has been added. 3) 12.50 mL of KOH has been added. 4) At the equivalence point. (Calculate the volume of KOH to reach the equivalence point & identify a good indicator.) 5) Provide a sketch...
When 10.00 mL of 0.240 M HX (Ka = 4.31 10-5) is titrated with 0.120 M KOH, the pH will increase. Calculate the pH of the solution at each point in the titration. The pKw is 14.000 at this temperature. Volume of KOH (mL) pH 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 26.00 28.00
A 15 mL sample of hydrofluoric acid, Ka=6.8x10^-4 was titrated with .475 M KOH. The equivalence point was reached after addition of 19.35 mL of base. Determine the molar concentration of the original hydrofluoric acid solution, and find the pH of the solution.
Consider a titration of 100-mL of .25 M formic acid (Ka-1.8 x 10^-4) with .2 M KOH What is the pH after 100 mL of base has been added?
(3) 30.00 mL of 0.085 M Hydrofluoric acid (HF) is titrated with 0.10 M NaOH. What is the pH of the acid solution before any base is added? (Ans: pH = 2.11) What is the pH of the titration mixture at half the equivalence point? (Ans: pH = 3.35) What is the pH of the titration mixture at the equivalence point? (Ans: pH = 7.92) What is the pH of the mixture after 40.00 mL of base are added? (Ans:...
IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10) solution is titrated with 0.200 M NaOH. Find the pH before titration and after 25 mL, 50 mL, and 60 mL of NaOH has been added.
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...