An analytical chemist is titrating 55.1 mL of a 0.8800M solution of diethylamine ((C₂H₂)₂NH) with a 0.4900M solution of HNO3. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 110.3 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

Q: A solution is prepared that is initially 0.19M in methylamine (CH3NH₂), a weak base, and 0.48M in…

A: Buffer solution is a type of solution that resists the change in its pH on adding small quantity of…

Q: An analytical chemist is titrating 189.5 mL of a 0.6500M solution of ammonia (NH,) with a 0.8000M…

A:

Q: An analytical chemist is titrating 86.6 mL of a 0.4900M solution of dimethylamine ((CH,) NH) with a…

A: Step 1:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: An analytical chemist is titrating 178.1 mL of a 1.200M solution of hydrazoic acid (HN) with a…

A: Hydrazoic acid ( HN3 ) is a weak acid.NaOH is a strong base .the volume of HN3 = 178.1 mL = 0.1781…

Q: An analytical chemist is titrating 52.7 mL of a 0.3500M solution of methylamine (CH, NH,) with a…

A:

Q: An analytical chemist is titrating 190.6 mL of a 0.3000M solution of methylamine (CH3NH₂) with a…

A:

Q: An analytical chemist is titrating 143.9 mL of a 0.6100M solution of acetic acid (HCH3CO₂) with a…

A: Given data : Concentration of HCH3CO2 = 0.6100 M Volume of HCH3CO2 = 143.9 mL Concentration of NaOH…

Q: An analytical chemist Is titrating 150.5 mL of a 0.1400M solution of aniline (CH,NH,) with a 0.4000M…

A:

Q: A chemist titrates 60.0 mL of a 0.6499 M propionic acid (HC,H,CO,) solution with 0.6233 M KOH…

A: At the equivalence point mole of acid = mole of the base. The reaction involved is as follows:

Q: An analytical chemist is titrating 215.6 mL of a 1.000M solution of hydrazoic acid (HN) with a…

A: Step 1: Step 2: Step 3: Step 4:

Q: A chemist titrates 170.0 mL of a 0.8997 M butanoic acid (HC,H,CO,) solution with 0.3845 M NAOH…

A: Given information: Molarity of butanoic acid (HC3H7CO2)= 0.8997 M Volume of butanoic acid = 170 ml…

Q: An analytical chemist is titrating 214.6 mL of a 1.200M solution of propionic acid (HC,H,CO,) with a…

A: By the reaction of Propanoic acid and KOH potassium propanoate and salt.sodium propanoate and…

Q: An analytical chemist is titrating 191.3 mL of a 0.8900M solution of hydrazoic acid (HN,) with a…

A:

Q: An analytical chemist is titrating 124.7 mL of a 0.7700M solution of piperidine (C,H, NH) with a…

A: Given,Molarity of piperidine ( C5H10NH ) = 0.7700 MVolume of  C5H10NH solution = 124.7 mLpKb of…

Q: An analytical chemist is titrating 201.0 mL of a 0.5700 M solution of piperidine (C,HNH) with a…

A: The question is based on the concept of titrations.   we are titrating  a  strong acid with a weak…

Q: An analytical chemist is titrating 136.3 mL of a 0.1300M solution of ammonia (NH3) with a 0.1800M…

A: Here we required to find the pH of the solution.

Q: the final volume equals the initial volume of the solution plus the volume of NaOH solution added. ?

A: Given, Molarity of Acid(M) = 0.4500 M Volume of Acid(V) = 78.9 mL mmol of Acid =  M × V   = 0.4500 ×…

Q: None

A: Step 1: Step 2: Step 3: Step 4:

Q: An analytical chemist is titrating 56.7 mL of a 0.4900M solution of formic acid (H,CO,) with a…

A:

Q: b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a…

A: Given: VCH3​NH2​​=136.2mL;[CH3​NH2​]=0.7100M;VHNO3​​=97.5mL;[H+]=0.4900MpKb​=3.36;pH=???Step 1:…

Q: An analytical chemist is titrating 59.1 mL of a 0.6700 M solution of ammonia (NH,) with a 0.4500 M…

A: Given : Concentration of NH3 = 0.6700 M Volume of NH3 solution = 59.1 mL = 0.0591 L…

Q: An analytical chemist is titrating 136.2 mL of a 0.4700M solution of propylamine (C,H,NH,) with a…

A: no of moles of C3H7NH2  = molarity * volume in L                                      =…

Q: A chemist titrates 130.0 mL of a 0.7778 M lidocaine (C, H,,NONH) solution with 0.1602 M HCI solution…

A: Given: Concentration of lidocaine, M1= 0.7778 MVolume of lidocaine, V1= 130ml =0.130LConcentration…

Q: A solution is prepared that is initially 0.095M in methylamine (CH3 NH,), a weak base, and 0.38M in…

A: we need to fill the given table and calculate pH of the solution

Q: Calculate the change in pH when 9.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution…

A: Given,

Q: An analytical chemist is titrating 74.8 mL of a 0.7500M solution of propylamine (C,H,NH,) with a…

A:

Q: An analytical chemist is titrating 221.9 mL Oof a 0.9800M solution of propionic acid (HC,H,CO,) with…

A:

Q: An analytical chemist is titrating 143.6 mL of a 0.7000M solution of piperidine (C5H10NH) with a…

A: Given, Volume of piperidne C5H10NH=143.6 mLMolarity of  piperidne C5H10NH=0.7000mPK6 =2.89Volume of…

Q: A chemist titrates 110.0 mL of a 0.3453 M methylamine (CH3NH₂) solution with 0.7011 M HCl solution…

A:

Q: the acid solution after the chemist has added 17.69 mL of the KOH solution to it. students: you may…

A: Mmol of Acid = 0.5900 × 141.4        = 83.426 mmol Mmol of Base = 0.760×17.69   = 13.44 mmol Excess…

Q: A chemist titrates 210.0 mL of a 0.3206M ammonia (NH3) solution with 0.3768M HCl solution at 25 °C.…

A:

Q: An analytical chemist is titrating 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M…

A:

Q: An analytical chemist is titrating 164.9 mL of a 0.4100M solution of hydrazoic acid (HN3) with a…

A:

Q: An analytical chemist is titrating 68.1 mL of a 0.6500M solution of propionic acid (HC,H,CO,) with a…

A: The given data is as follows: The concentration of propionic acid = 0.6500 M The volume of propionic…

Q: An analytical chemist is titrating 126.8 mL of a 0.2600M solution of diethylamine ((C₂H₂)₂NH) with a…

A: Given : Concentration of diethylamine = 0.2600 M  Volume of diethylamine = 126.8 ml  Concentration…

Q: An analytical chemist is titrating 208.8mL of a 0.7500M solution of methylamine CH3NH2 with a…

A: In this question, we want to determine the pH of the Solution after titration of weak base with…

Q: A buffer solution is prepared by combining 0.898 moles of formic acid and 0.733 moles of sodium…

A: The buffer solution is prepared by mixing with 0.898 moles of formic acid and 0.733 moles of sodium…

Q: A chemist titrates 150.0 mL of a 0.0676M dimethylamine (CH,) NH) solution with 0.4402M HBr solution…

A: Interpretation - To calculate the pH at equivalence point.     Given  molarity of dimethyl amine =…

Q: An analytical chemist is titrating 139.2 mL of a 0.2600M solution of ammonia (NH3) with a 0.5900M…

A: we have to calculate the pH of the solution

Q: An analytical chemist is titrating 99.3 mL of a 0.3300M solution of propylamine (C,H, NH₂) with a…

A:

Q: N) with a 0.7800M solution of HNO3. The pK, of trimethylamine An analytical chemist is titrating…

A: To calculate the pH of the solution after adding 86.6 mL of 0.7800 M HNO3 to 123.2 mL of 0.4600 M…

Q: An analytical chemist is titrating 239.7 mL of a 0.6100M solution of benzoic acid (HC,H,CO,) with a…

A: pH of a buffer can be determined by using Henderson equation pH = pka + log( salt/ acid)

Q: A chemist titrates 50.0 mL of a 0.1314M lidocaine (CH,2 NONH) solution with 0.3507M HNO, solution at…

A: Given  volume = 50.0mL concentration= 0.1314M (lidocaine) Concentration of HNO3 = 0.3507M  pKb od…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.