A chemist titrates 60.0 mL of a 0.5980M hypochlorous acid (HCIO) solution with 0.6753M NAOH solution at 25 °C. Calculate the pH at equivalence. The p K of hypochlorous acid is 7.50, 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 NaOH solution added.

Q: An analytical chemist is titrating 91.3 mL of a 0.7000M 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 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: 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: 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: 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: 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 chemist titrates 50.0 mL of a 0.2742 M ethylamine (C,H,NH,) solution with 0.5877 M HNO, solution…

A: An equivalence point during a titration is when equivalent quantities of acid and base have been…

Q: Please calculate the pH of a buffer solution

A:

Q: An analytical chemist is titrating 226.3 mL of a 0.3900M solution of hydrazoic acid (HN3) with a…

A: The objective of the question is to calculate the pH of the acid solution after the addition of .It…

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: help

A: (M2 • V2)NaOH = ( M1 • V1 )HCNO V2 = ( 0.4913molL-1 • 170.0mL / 0.2156molL-1 )  V2 = 387.4 mL…

Q: A chemist titrates 220.0 mL of a 0.0579M propionic acid (HC₂H₂CO₂) solution with 0.1972M KOH…

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

Q: Consider a buffer solution that is 0.47 M HCN and 0.47 M NaCN. (Ka(HCN) = 4.9 × 10−10) Calculate…

A: After addition of 0.20 mol of NaOH the [ HCN ] = ( 0.47 - 0.20 ) = 0.27 M And [ NaCN ] = ( 0.47 +…

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 80.0 mL of a 0.0860M hypochlorous acid (HC1O) solution with 0.6206M KOH solution…

A:

Q: Sodium benzoate, the sodium salt of benzoic acid, is used as a food preservative. A sample…

A: moles of HCl added = molarity x volume in mL                                 = 0.5 M x 50 ml = 25…

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

Q: Calculating the pH at equivalence of a titration A chemist titrates 230.0 mL of a 0.3847 M…

A: At equivalence point the number of moles (nNaOH) of NaOH is equal to the number of moles (nHCN) of…

Q: An analytical chemist is titrating 144.6 mL of a 0.6600 M solution of benzoic acid (HC,H,CO,2) with…

A: Given Benzoic acid Concentration = 0.6600 M volume = 144.6 ml KOH Concentration = 0.8400 M Volume…

Q: A chemist titrates 120.0 mL of a 0.2065 M benzoic acid (HC HCO₂) solution with 0.6703 M NaOH…

A: In this chemistry problem, we are tasked with calculating the pH at the equivalence point of a…

Q: A chemist titrates 220.0 mL of a 0.6204 M butanoic acid (HC₂H,CO₂) solution with 0.2746 M KOH…

A:

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

A:

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

A:

Q: A chemist titrates 160.0 mL of a 0.3349M cyanic acid (HCNO) solution with 0.3751 M KOH solution at…

A: Given data : Concentration of HCNO = 0.3349 M Volume of HCNO = 160.0 mL Concentration of KOH =…

Q: An analytical chemist is titrating 204.4 mL of a 0.9200 M solution of butanoic acid (HC₂H,CO₂) with…

A:

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: Calculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.1528M…

A:

Q: An analytical chemist is titrating 191.4 mL of a 0.4200M solution of benzoic acid (HC,H5CO,) with a…

A: We can approach this question by calculating the millimoles reacting. Thus we can find the…

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)

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.