A chemist titrates 70.0 mL of a 0.4298 M propionic acid (HC,H,CO,) solution with 0.2267 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK, of propionic acid is 4.89. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added.

Q: A chemist titrates 170.0 mL of a 0.2489M nitrous acid (HNO₂) solution with 0.7980 M NaOH solution at…

A: Given,molarity of HNO2 = 0.2489 Mvolume of HNO2 = 170.0 mL = 0.1700 LTherefore, number of moles of…

Q: A chemist titrates 50.0 mL of a 0.8655M ethylamine (C,H,NH,) solution with 0.1833M HBr solution at…

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

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Q: A chemist titrates 250.0 mL of a 0.8167M carbonic acid (H,CO3) solution with 0.1388M NaOH solution…

A: Answer is explained below. Given, volume of H2CO3 is 250 ml and its concentration is 0.8167 M. &…

Q: A chemist titrates 110.0 mL of a 0.3936M dimethylamine ((CH3), NH) solution with 0.7244M HNO,…

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Q: An analytical chemist is titrating 161.1 ml. of a 0.6100M solution of formic acid (H,CO,) with a…

A: Given data,Molarity of HCOOH=0.61MVolume of HCOOH=161.1mL=0.1611LMolarity of NaOH=0.46MVolume of…

Q: A chemist titrates 110.0 mL of a 0.5082 M carbonic acid (H,CO,) solution with 0.5000M NaOH solution…

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Q: A chemist titrates 200.0 mL of a 0.3926M benzoic acid (HC H,CO,) solution with 0.4808 M KOH solution…

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

Q: A chemist titrates 190.0 mL of a 0.5697 M carbonic acid (H, CO,) solution with 0.1442 M KOH solution…

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

Q: A buffer system is prepared by combining 0.406 moles of ammonium chloride (NH4CI) and 0.525 moles of…

A: Moles of base (NH3 ) = 0.525 mol  Moles of conjugate acid (NH4+ ) = 0.406 mol Moles of nitric acid…

Q: A chemist titrates 250.0 mL of a 0.8118 M pyridine (C,H,N) solution with 0.3729M HBr solution at 25…

A: Given,  [C5H5N] = 0.8118 M  Volume of C5H5N in mL = 250.0 mL  [HBr] = 0.3729 M  pKb of C5H5N = 8.77…

Q: A chemist titrates 60.0 ml. of a 0.4812 M cyanic acid (HCNO) solution with 0.7227 M NaOH solution at…

A: Question about titration of weak acid cyanic acid with NaOH. We have to calculate the pH at…

Q: A chemist titrates 210.0 mL of a 0.2223M pyridine (C,H,N) solution with 0.3895M HNO, solution at 25…

A: Given: Volume of C5H5N = 0.2223 M Volume of C5H5N solution = 210.0 mL = 0.210 L…

Q: A chemist titrates 250.0 mL of a 0.8331 M butanoic acid (HC,H,CO,) solution with 0.5749 M NaOH…

A: Molarity dilution equation: Given data: Concentration of butanoic acid=0.8331M. Volume of butanoic…

Q: A chemist titrates 120.0 mL of a 0.7631 M acetic acid (HCH C0,) solution with 0.0959M KOH solution…

A:

Q: A chemist titrates 120.0 mL of a 0.2898M carbonic acid (H₂CO,) solution with 0.8540M KOH solution at…

A: pH value at equivalence point can be calculated by considering the equilibrium reaction of HCO3-

Q: A chemist titrates 130.0 mL of a 0.8034M pyridine (C,HşN) solution with 0.2958M HCl solution at 25…

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Q: An analytical chemist is titrating 130.6 ml. of a 0.6000 M solution of piperidine (C,HNH) with a…

A: Given, Volume of piperidine (C5H10NH) = 130.6 mL Concentration of piperidine (C5H10NH) = 0.6000 M…

Q: A chemist titrates 60.0 mL of a 0.4543 M aniline (C,H;NH,) solution with 0.7673M HNO, solution at 25…

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Q: A chemist titrates 250.0 mL of a 0.2448 M butanoic acid (HC,H,CO,) solution with 0.1225 M KOH…

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Q: An analytical chemist is titrating 243.9 mL of a 0.3300M solution of ammonia (NH,) with a 0.8900M…

A: The above-given problem can be solved using the Henderson-Hesselbalch equation. Given,pKb of ammonia…

Q: Calculate the pH at equivalence. The p K of nitrous acid is 3.35.

A:

Q: An analytical chemist is titrating 88.8 ml. of a 0.4900 M solution of piperidine (C,HNH) with a…

A: When a strong base is added to a weak acid solution or a strong acid is added to a weak base, then…

Q: A chemist titrates 240.0 mL of a 0.0903 M acetic acid (HCH, CO₂) solution with 0.3931 M KOH solution…

A: Given : molarity of acetic acid = 0.0903 M volume of acetic acid = 240.0 mL molarity of KOH = 0.3931…

Q: E pat equivalence of a sitration A chemist titrates 200.0 ml. of a 0.4797 M hypochlorous acid (HCIO)…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

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: A chemist titrates 60.0 mL of a 0.1125 M hypochlorous acid (HCIO) solution with 0.7761 M KOH…

A: HClO is a weak acid and KOH is strong base   Calculating moles of HClO Volume in L x M = Moles…

Q: An analytical chemist is titrating 205.8 mL of a 0.09100M solution of propylamine (C,H,NH,) with a…

A:

Q: A chemist titrates 150.0 mL of a 0.5341M carbonic acid (H,CO,) solution with 0.2213M KOH solution at…

A: We have 150 mL 0.5341 M of carbonic acid and 0.2213 M of KOH . We have to calculate the pH at…

Q: A chemist titrates 50.0 mL. of a 0.6803 M benzoic acid (HC,H, CO₂) solution with 0.2885 M NaOH…

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: A chemist titrates 80.0 mL of a 0.0860M hypochlorous acid (HC1O) solution with 0.6206M KOH solution…

A:

Q: A chemist titrates 50.0 mL of a 0.1365M methylamine (CH, NH,) solution with 0.7300M HNO, solution at…

A: Given :

Q: A chemist titrates 170.0 mL of a 0.1735M pyridine (C,H,N) solution with 0.3504M HBr solution at 25…

A:

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: An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH,)…

A: Given that : The volume of isopropylamine = 83.7 mL The molarity of isopropylamine = 0.3300 M The…

Q: The pH of a bicarbonate-carbonic acid buffer is 5.63. Calculate the ratio of the concentration of…

A: pH = 5.63 NOTE: please note as pKa value is not provided , I have used standard value.  if your…

Q: Calculating the Valence of a titration A chemist titrates 60.0 mL of a 0.0694M butanolc acid…

A:

Q: An analytical chemist is titrating 149.7 mL of a 0.5500 M solution of benzoic acid (HC H.CO,) with a…

A: The reaction taking place between benzoic acid and NaOH is- C6H5COOH + NaOH →C6H5COONa + H2O

Q: An analytical chemist is titrating 88.2 mL of a 0.2300M solution of nitrous acid (HNO₂) with a…

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Q: An analytical chemist is titrating 146.1 mL of a 0.4500M solution of ammonia (NH;) with a 0.4400M…

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Q: An analytical chemist is titrating 231.8 mL of a 0.9900M solution of acetic acid (HCH,CO,) with a…

A:

Q: An analytical chemist is titrating 70.4 mL of a 0.3700M solution of cyanic acid (HCNO) with a…

A: Given that, Volume of cyanic acid = 70.4 mL Volume of KOH = 55.9 mL Molarity of cyanic acid = 0.3700…

Q: A chemist titrates 230.0 mL of a 0.1072M ethylamine (C,H,NH, solution with 0.5758M HC1 solution at…

A: Answer :-  pH =  5.93 ---------------------------------

Q: An analytical chemist is titrating 147.3 mL of a 0.3200M solution of ammonia (NH,) with a 0.8200M…

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Q: Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H5OOH and 0.252…

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Q: A chemist titrates 160.0 mL of a 0.3445 M pyridine (C-H5N) solution with 0.8552M HNO3 solution at 25…

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Q: A chemist titrates 240.0 mL of a 0.0890M aniline (C,H,NH,) solution with 0.6621M HNO, solution at 25…

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Q: An analytical chemist is titrating 219.9 mL of a 0.5100 M solution of aniline (CH,NH,) with a 0.1800…

A: Given: Concentration of aniline = [C­6H5NH2] = 0.5100 M Volume of C­6H5NH2 = 219.9 mL pKb for…

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.