An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2)...

An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2) with a 0.6400 M solution of KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 22.2 mL of the KOH solution to it. Please round your answer to 2 decimal places

Expert Solution

queen_honey_blossom answered 1 year ago

An analytical chemist is titrating 114.8mL of a 0.3100M solution of nitrous acid HNO2 with a...

An analytical chemist is titrating 114.8mL of a 0.3100M solution of nitrous acid HNO2 with a 1.000M solution of KOH . The pKa of nitrous acid is 3.35 . Calculate the pH of the acid solution after the chemist has added 12.69mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

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An analytical chemist is titrating 60.5mL of a 0.8700M solution of benzoic acid HC6H5CO2 with a 0.3600M solution of KOH . The pKa of benzoic acid is 4.20 . Calculate the pH of the acid solution after the chemist has added 172.mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 227.3mL of a 1.200M solution of propionic acid HC2H5CO2 with a...

An analytical chemist is titrating 227.3mL of a 1.200M solution of propionic acid HC2H5CO2 with a 0.5600M solution of NaOH . The pKa of propionic acid is 4.89 . Calculate the pH of the acid solution after the chemist has added 532.8mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 178.3mL of a 0.3400M solution of acetic acid HCH3CO2 with a...

An analytical chemist is titrating 178.3mL of a 0.3400M solution of acetic acid HCH3CO2 with a 0.2300M solution of NaOH . The pKa of acetic acid is 4.70 . Calculate the pH of the acid solution after the chemist has added 46.70mL of the NaOH solution to it

You are titrating 50 ml. of nitrous acid with sodium hydroxide (0.15 M). Equivalence is reached...

You are titrating 50 ml. of nitrous acid with sodium hydroxide (0.15 M). Equivalence is reached at 22.0 ml of NaOH delivered. Calculate the pH of the solution in the flask: - before the beginning of the titration - after the delivery of 5 ml. of titrant - at half$equivalence - at equivalence -after delivery of 23 ml. of titrant. -------------Give detail Show ALL WORK, UNITS and use ICE/reaction table and ML (no millimoles). Please be clear in how you...

Find the pH during the titration of 20.00 mL of 0.1000 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.1000 M nitrous acid, HNO2 (Ka = 7.1 10-4), with 0.1000 M NaOH solution after the following additions of titrant. Find at volumes of 0 mL, 10.00 mL, 15.00 mL, 20.00 mL, and 25.00 mL.

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You carry out the titration of 25.00 mL of 0.250 M Nitrous Acid (HNO2) using a 0.375 M NaOH solution Nitrous acid Ka= 4.5*10^-4 Calculate the pH at the volume of NaOH added, see table Titration point Volume of NaOH added (mL) pH 1 0 2 4.25 3 8.33 4 16.67 a. At 0 mL NaOH b. At 4.25 mL NaOH c. At 8.33 mL NaOH d. at 16.67 mL NaOH

Be sure to answer all parts. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are...

Be sure to answer all parts. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. (a) Calculate the pH for the initial solution. (b) Calculate the pH for the point at which 80.0 mL of the base has been added. (c) Calculate the pH for the equivalence point. (d) Calculate the pH for the point at which 105 mL of the base has been added.

Find the pH during the titration of 20.00 mL of 0.2300 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.2300 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.2300 M NaOH solution after the following additions of titrant. a) 0mL b)10.00mL c) 15.00mL d) 19.00mL e)19.95 mL f) 20.00mL g) 20.05mL h) 25.00mL

Find the pH during the titration of 20.00 mL of 0.1820 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.1820 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.1820 M NaOH solution after the following additions of titrant. ( a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00 mL

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