A chemist titrates 30.0 mL of 0.840 M hydroxylamine, HONH2 Kb = 1.1 x 10–8 ,...

A chemist titrates 30.0 mL of 0.840 M hydroxylamine, HONH2 Kb = 1.1 x 10–8 , with 0.900 M HNO3. Calculate the pH at each of the following volumes of added titrant.

12.0 mL HNO3

14.0 mL HNO3

28.0 mL HNO3

35.0 mL HNO3

Solutions

Expert Solution

NOW PH= 14 - POH

= 14 - 7.83

= 6.17

Please check the calculations and pay attention to the unit analysis.

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A chemist titrates 210.0 mL of a 0.7560 M butanoic acid (HC3H7CO2) solution with 0.6335 M...

A chemist titrates 210.0 mL of a 0.7560 M butanoic acid (HC3H7CO2) solution with 0.6335 M KOH solution at 25 degrees celsius. Calculate the pH at equivalence. The pKa of butanoic acid is 4.82. Round your answer to 2 decimal places please

A) A chemist titrates a 25.0 mL sample of 0.191 M benzoic acid (C6H5COOH) against a...

A) A chemist titrates a 25.0 mL sample of 0.191 M benzoic acid (C6H5COOH) against a 0.100 M solution of NaOH. The overall reaction is shown by the equation below: $$C6H5COOH(aq)+NaOH(aq) C6H5COONa(aq)+H2O(l) The Ka value for benzoic acid is 6.28 × 10–5. Calculate the pH at the start of the titration, before any NaOH has been added. Give your answer correctly to two places after the decimal. B) What will the pH be when 12.0 mL of 0.100 M NaOH...

Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540)...

Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HClO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 5.3 mL pH = (c) 10.5 mL pH = (d) 15.8 mL pH = (e) 21.0 mL pH = (f) 33.6 mL pH =

Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.40e-05)...

Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.40e-05) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = _________ (b) 5.3 mL pH = __________ (c) 10.5 mL pH = ____________ (d) 15.8 mL pH = _____________ (e) 21.0 mL pH =___________ (f) 39.9 mL pH = __________

Consider the titration of 60.0 mL of 0.100 M NH3 Kb= 1.8 x 10^-5 with 0.150...

Consider the titration of 60.0 mL of 0.100 M NH3 Kb= 1.8 x 10^-5 with 0.150 M HCl. Calculate the pH after the following volumes of titrant have been added: 40.5 mL & 60.0 mL

Consider the titration of 100.0 mL of 0.130 M H2NNH2 (Kb= 3.0 x 10-6) by 0.260...

Consider the titration of 100.0 mL of 0.130 M H2NNH2 (Kb= 3.0 x 10-6) by 0.260 M HNO3. Calculate the pH of the resulting solution after the following volumes of have been added: 0.0 mL, 20.0 mL, 40 mL, 50 mL, 100 mL.

Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M...

Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M solution of hydrochloric acid. A) Write the chemical equation that occurs B) Do you expect the pH of the solution to be acidic, basic or neutral at the equivalence point? Explain. C) Calculate the pH after 20 mL of HCl solution have been added. Hint: Kb(NH3)=1.8*10-5

If 30.0 mL of 0.150 M CaCl2 is added to 35.0 mL of 0.100 M AgNO3,...

If 30.0 mL of 0.150 M CaCl2 is added to 35.0 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate?

The dissociation of hydroxylamine H2NOH in water Kb = 1.5x10-8 forms what two products. (Show ICE...

The dissociation of hydroxylamine H2NOH in water Kb = 1.5x10-8 forms what two products. (Show ICE Table). You have a 0.340 M solution of the base above. You create an ICE table and solve for x and get x = 1.45x10-6 1. What is the hydroxide concentration of your base is [x] 2. the pH of your base is [y]

Consider the titration of a 30.0 mL sample of 0.150 M CH3COOH (Ka=1.8×10−5) with 0.200 M...

Consider the titration of a 30.0 mL sample of 0.150 M CH3COOH (Ka=1.8×10−5) with 0.200 M NaOH. Determine each quantity: Part A: What is the volume of base required to reach the equivalence point? Express your answer using one decimal place. Part B: What is the pH after 10.0 mL of base have been added? Express your answer using two decimal places. Part C What is the pH at the equivalence point? Express your answer using two decimal places. Part...

Subjects