96 . After the addition of 20.00 mL of 0.500 M standard KOH solution to a...
After the addition of 20.00 ml. of 0.500 M standard KOH solution to a 10.00 mL sample of formic acid (HCOOH, K_a = 1.8 times 10^-4), the equivalence point is reached. What is the molarity of the formic acid? What is the pH at the equivalence point?
196 3. After the addition of 20.00 mL of 0.500 M standard kon sample of formic acid (HCOOH, K = 1.8 x 10), the equivalence pom Wat is the molarity of the formic acid? What is the pH at the equivalence 00 M standard KOH solution to a 10.00 mL "), the equivalence point is reached. ? What is the pH at the equivalence point?
Calculate the hypothetical pH AFTER addition of 15.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. QUESTION 7 10 poir Calculate the hypothetical pH AFTER addition of 40.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. Calculate the hypothetical pH AFTER addition of 46.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with...
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?
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.
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...
Determine the pH during the titration of 25.5 mL of 0.455 M formic acid (Ka = 1.8×10-4) by 0.477 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 5.90 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 36.5 mL of KOH
1) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 16.0 mL of KOH.Express your answer numerically. pH=_______ 2) A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3.Express your answer numerically. pH=_______ 3) A 52.0-mL volume of 0.35 M CH3COOH (Ka = 1.8 x10-5 ) is titrated with 0.40 M NaOH. Calculate...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 15.0 mL of KOH. Express your answer numerically. pH = SubmitHintsMy AnswersGive UpReview Part Part C A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. pH = SubmitHintsMy AnswersGive UpReview Part Part D A 52.0-mL volume of 0.35 M CH3COOH...
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...