Q3: Calculate the molarity of Hydrofluoric acid in a titration of Hydrofluoricacid against Sodium hydroxide as shown in figure below?-utel Hading (17 ml. of HF)BuretieClamphurette-Fnat Roading (4 ml. of HF)Analyte (unknown concentration)(HF acid)StandIndicator (pink)Titrant (known concentration)(N3OH 26 ml & 0.3 M)

For Hydrofluoric acid (HF) : Initial reading of HF =17ml Final reading of HF = 4ml For Sodium…

Q3: Calculate the molarity of Hydrofluoric acid in a titration of Hydrofluoric acid against Sodium hydroxide as shown in figure below? tel Hading (17 ml. of HF) Buretie Clamp hurette -Fnat Roading (4 ml. of HF) Analyte (unknown concentration) (HF acid) Stand Indicator (pink) Titrant (known concentration) (NaOH 26 ml & 0.3 M)

Q3: Calculate the molarity of Hydrofluoric acid in a titration of Hydrofluoric acid against Sodium hydroxide as shown in figure below? tel Hading (17 ml. of HF) Buretie Clamp hurette -Fnat Roading (4 ml. of HF) Analyte (unknown concentration) (HF acid) Stand Indicator (pink) Titrant (known concentration) (NaOH 26 ml & 0.3 M)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

See similar textbooks

Similar questions

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
Volume of acetic acid (HC2H3O2) in the first titration (L) 10 mL Volume of acetic acid (HC2H3O2) in the second titration (L) 10 mL Normality of sodium hydroxide (NaOH) (N) 0.1 N Volume of sodium hydroxide (NaOH) in the first titration (L) 10 mL = ……..L Volume of sodium hydroxide (NaOH) in the second titration (L) 10 mL = ……..L Normality of acetic acid (HC2H3O2) in the first titration (N) Normality of acetic acid (HC2H3O2) in the secondtitration (N) Average normality of acetic acid (HC2H3O2) (N) Mass % of acetic acid (HC2H3O2) (%)
Part A A beaker with 1.40x10? mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this butfer is 0.100 mol L-, A student adds 4.90 mL of a 0.480 mol L- HCl solution to the beaker. How much will the pH change? The pK, of acetic acid is 4,760. Express your answer numerically to two decimal places. Use a minus (-) sign if the pH has decreased. > View Available Hint(o) ? ApH =
What volume of 0.85 M NaOH (in mL) is needed to reach the equivalence point in a titration of 83.0 mL of 0.90 M HCIO4? Your Answer: Answer units
Q2 A 50.0 ml 0.100 M of a diprotic acid acid (H2M) solution is titrated with 0.200M NaOH. a) How many end points do you expect at which volumes? Calculate the pH values at the endpoints. b) What is the pH after 12.5ml, 32.0ml, 37.5ml,55.0ml? c) (Bonus)How many endpoints would you expect if the initial solution was 0.100M H2M and 0.010M Ethanol? Oxalic acid(H2M) Ka1= 1.0 x 102 Ka2=5.0x105 Ethanol(CH3CH2OH) K, = 3.16 x 1016
5 6 7 8 Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K, of hypobromous acid is 2.8 x 10¹⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)? (Two decimal places) Type your answer... Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K, of hypobromous acid is 2.8 x 10¹⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What volume (in mL) of titrant will have been added at the half-equivalence point? (One decimal place) Type your answer... Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid is 2.8 x 10.⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide…
View Policies Current Attempt in Progress Suppose we titrate 20.0 mL of 0.100M HCHO2 (K, = 1.8 × 10-4) with 0.100 M NaOH. Calculate the pH. Before any base is added: pH = i When half of the HCHO, has been neutralized: pH = After a total of 15.0 mL of base has been added: pH = At the equivalence point: pH =