An analytical chemist is titrating 150.4 mL of a 0.5000M solution of benzoic acid (HC H-CO₂) with a 0.9800M solution of NaOH. The p K of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 31.50 mL 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.

Q: A chemist titrates 220.0 mL of a 0.6779M acetic acid (HCH3CO₂) solution with 0.3134M KOH solution at…

A: At equivalence point, all the acid are consumed by the added acid. Here the moles of acid reacted…

Q: An analytical chemist is titrating 242.9 mL of a 0.7800M solution of cyanic acid (HCNO) with a…

A: pH of resulting solution can be determine by the compound formed and the remaining or excess…

Q: An analytical chemist is titrating 185.4 mL of a 0.3800M solution of propionic acid (HC₂H5CO₂) with…

A: Given,  Molarity of propionic acid (HC2H5CO2 ) = 0.3800 M.  Volume of propionic acid (HC2H5CO2 ) =…

Q: An analytical chemist is titrating 247.8 mL of a 1.100M solution of acetic acid (HCH, CO₂) with a…

A:

Q: An analytical chemist is titrating 73.6 mL of a 0.8200M solution of benzoic acid (HC H, CO₂) with a…

A:

Q: An analytical chemist is titrating 228.8 mL of a 0.6100M solution of hydrazoic acid (HN3) with a…

A:

Q: An analytical chemist is titrating 196.9 mL of a 0.5300M solution of butanoic acid (HC3H,CO₂) with a…

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

Q: An analytical chemist is titrating 158.1 mL of a 1.100M solution of benzoic acid (HC6H₂CO₂) with a…

A: The volume of the benzoic acid solution = The concentration of the benzoic acid solution = The…

Q: An analytical chemist is titrating 200.5 mL of a 0.3400M solution of hydrazoic acid (HN,) with a…

A: Here we use the Henderson Hasselbach equation,pH = pKa + log [Salt]/[Acid] Initial Acid = 200.5 x…

Q: A chemist titrates 220.0 mL of a 0.4703M benzoic acid (HCH₂CO₂) solution with 0.0972M NaOH solution…

A: We  have to calculate the pH at equivalence point

Q: If you are titrating 10.00 mL of 0.150 M HCl with an unknown solution of NaOH, and it takes 15.70…

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

Q: A chemist titrates 170.0 mL of a 0.6288 M hydrocyanic acid (HCN) solution with 0.6937M KOH solution…

A: The reaction between the weak acid HCN and the strong base KOH can be represented as:HCN + OH-…

Q: An analytical chemist is titrating 1/8.6 mL of a 0.7500M solution of ammonia (NH3) with a 0.4800M…

A: Given -> Volume of NH3 = 178.6 ml Molarity of NH3 = 0.7500 M Volume of HNO3 = 142.1 ml Molarity…

Q: An analytical chemist is titrating 169.6 mL of a 0.4900M solution of acetic acid (HCH3CO₂) with a…

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

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: An analytical chemist is titrating 152.2 mL of a 0.2200M solution of propionic acid (HC₂H₂CO₂) with…

A: The balanced equation for the reaction is HC2H5CO2 (aq) + KOH (aq) -----> KC2H5CO2 (aq) + H2O (l)

Q: A 1.31 L buffer solution consists of 0.191 M butanoic acid and 0.288 M sodium butanoate. Calculate…

A: By using Henderson-Hesselbalch's equation, pH of a buffer solution can be calculated. pH of a buffer…

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: A chemist titrates 220.0 mL of a 0.6099M trimethylamine ((CH3)N) solution with 0.2791 M HCl solution…

A:

Q: A chemist titrates 180.0 mL of a 0.5682 M methylamine (CH3NH₂) solution with 0.8472 M HNO3 solution…

A: we have to calculate the pH of the solution at equivalence point

Q: An analytical chemist is titrating 114.8 mL of a 0.3700M solution of benzoic acid (HC6H5CO2) with a…

A: First, we need to calculate the number of moles of benzoic acid and KOH. The number of moles is…

Q: A chemist titrates 240.0 mL of a 0.3461M hydrocyanic acid (HCN) solution with 0.0793M NaOH solution…

A:

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

A:

Q: An analytical chemist is titrating 76.5 mL of a 0.4500M solution of propionic acid (HC₂H₂CO₂) with a…

A:

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 152.0 mL of a 0.2100 M solution of benzoic acid (HC,H,CO,) with a…

A: Given: Concentration of HC6H5CO2 = 0.2100 M Volume of HC6H5CO2 = 152.0 mL Concentration of NaOH =…

Q: An analytical chemist is titrating 145.8 mL of a 0.7500 M solution of propionic acid (HC₂H₂CO₂) with…

A:

Q: Briefly explain the most likely reason the student obtained the results of the pH paper turning blue…

A: Explationation of above question is given below.

Q: An analytical chemist is titrating 167.1 mL of a 0.6100M solution of butanoic acid (HC,H,CO₂) with a…

A: From the amount of NaOH added to butanoic acid we can figure out the pH of resulting solution.

Q: An analytical chemist is titrating 60.6 mL of a 0.3000 M solution of butanoic acid (HC,H,Co,) with a…

A: Given : Concentration of HC3H7CO2 = 0.3000 M Volume of HC3H7CO2 solution = 60.6 mL = 0.0606 L…

Q: An analytical chemist is titrating 232.9 mL of a 0.2400M solution of cyanic acid (HCNO) with a 1.200…

A: Given titration is between weak acid, cyanic acid and strong base, KOH. Based on the moles of excess…

Q: A chemist titrates 230.0 mL of a 0.5410 M aniline (CH,NH,) solution with 0.4431 M HBr solution at 25…

A: Given: volume of aniline = 230 mL molarity of aniline = 0.5410 M molarity of HBr = 0.4431 M pKb of…

Q: An analytical chemist is titrating 68.6 mL of a 0.4000M solution of acetic acid (HCH 2 CO2) with a…

A:

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 85.5 mL of a 0.4000M solution of formic acid (H₂CO₂) with a…

A: Given A solution is prepared using formic acid = 0.4000M x 85.5 ml        = 213.75 mmol NaOH =…

Q: A chemist titrates 130.0 mL of a 0.6533 M cyanic acid (HCNO) solution with 0.5467 M KOH solution at…

A: Concentration of cyanic acid = 0.6533 M Volume of cyanic acid = 130 ml or 0.13 L Number of moles of…

Q: A chemist titrates 130.0 mL of a 0.8883 M ammonia (NH2) solution with 0.0816 M HC1 solution at 25…

A: Given: The volume of ammonia solution (NH3) (V1) is 130.0 mL The molarity of ammonia solution (NH3)…

Q: A chemist titrates 110.0 mL of a 0.3060 M acetic acid (HCH3CO₂) solution with 0.8835 M KOH solution…

A: pKa = 4.76 Molarity of acid = 0.3060 M Volume of acid = 110.0 ml Molarity of base = 0.8835 M

Q: pH =

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Does the concentration of HC, H,O, increase or decrease when OH is added? O increase O decrease Does…

A: HC7H5O2  +  H2O  ⇌    H3O+   +  C7H5O2-     According to Le-chatelier's principle :  On addition OH-…

Q: An analytical chemist is titrating 87.3 mL of a 0.9000M solution of butanoic acid (HC3H,CO₂) with a…

A: Answer: When base is added in the acid solution, salt and water will form and lots of heat gets…

Q: An analytical chemist is titrating 102.0 mL of a 0.8400M solution of cyanic acid (HCNO) with a…

A: pka of cyanic acid = 3.46

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.