For the following question please show all work. For the titration of 20.00 mL of 0.150M NaOH with 0.250 M HF. (Ka for HF is 6.8 x 10-4) Write the molecular equation with state symbols Calculate the initial pH. Indicate species present Calculate the pH after 5.00 mL of HF has been added. Indicate species present Calculate pH at equivalence point. Indicate species present Calculate the pH after 6.00 mL extra of HF has been added. Indicate species present

For the following question please show all work. For the titration of 20.00 mL of 0.150M NaOH with 0.250 M HF. (Ka for HF is 6.8 x 10-4) Write the molecular equation with state symbols Calculate the initial pH. Indicate species present Calculate the pH after 5.00 mL of HF has been added. Indicate species present Calculate pH at equivalence point. Indicate species present Calculate the pH after 6.00 mL extra of HF has been added. Indicate species present

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

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A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated
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What is the best way to calculate the following titration: 100 ml water and 100 ml of solution with citric acid with pH2 is mixed togeather so the total volume is 200 ml. Then i titrate with NaHCO3 with the following grams. 0.62 gr , 1.82 gr , 2.40 gr What is the pH after each addition of NaHCO3. Please show details, along with the pKa and how it is used as I am very stuck on this and getting it wrong
I have contacted Bartleby customer support and they said this question is valid to be asked! They have said if someone denys again, i can contact them back and they will know who has declined and have a talk with them! Dont cause any issues! Use acid-base titration to determine theconcentration of:– A weak acid: CH3COOH 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10
Q2 (a) Compare between redox titration and Acid-base titration. (b) A 0.12 N HNO3 solution is titrated with potassium hydroxide. 20 ml ofunknown KOH solution consume 15 ml of above HNO3. Calculateamount of KOH present in the solution in terms of g/lit. (c) Identify any three requirements of primary standard and give suitablejustification for the above selected points.
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Determine the [H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2H (HAc), is 4.745. To enter exponential values, use the format 1.0e-5. Someone else on Bartleby posted the answers for the first 3 questions, however, their solution is not clear and thats why I could not finish the remaider of these questions.