In this experiment, you will titrate 2.00 mL of 0.0100 M KMnO4 in base with 0.0200 M NaHSO3. Using the redox equation below, calculate the volume of titrant NaHSO3 you expect to require for a complete reaction. 2MnO4-(aq) + HSO3-(aq) + 3OH-(aq)  ⇌ 2MnO42-(aq) + SO42-(aq) + 2H2O(l)

Q: An analytical chemist is titrating 83.1 mL of a 0.2800M solution of piperidine (C5H₁0NH) with a…

A: pH= -log [H+]

Q: An analytical chemist is titrating 109.1 mL of a 0.8800M solution of piperidine (C5H₁NH) with a…

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

Q: An analytical chemist is titrating 170.2 mL of a 0.7700M solution of aniline (C,H,NH,) with a…

A: Weak base when titrated with strong acid below equivalence point acts as buffer solution as there…

Q: Calculate the molarity of the acid using the titration data. b) If we assume that the titrated…

A: We are given two methods titration method and pH method  We have to find molarity of acid, pH if…

Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 319 mL 0.0439 M…

A: pH of the solution can be calculated using the following equation: pH = pKa + log ([salt]/[acid])

Q: Calculate the pH for each of the cases in the titration of 35.0 mL of 0.230 M NaOH(aq) with 0.230 M…

A:

Q: A chemist titrates 60.0 mL of a 0.0919 M lidocaine (C4H,NONH) solution with 0.8547 M HBr solution at…

A:

Q: (b) If the titrant has a molarity of 0.1500 M and there are 40.00 mL of analyte present, what is the…

A: A titration curve of pH v/s volume of titrant added is provided.A diprotic acid say H2A is the…

Q: phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the…

A:

Q: Given 1.00 L of a solution that is 0.100 M in sodium propionate (NaC3H5O2) and 0.300 M in propionic…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

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: If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00250 M , determine the…

A: Given, H2CO3(aq)  ⇌  HCO3-(aq) + H+(aq) pH of blood = 7.45 Acid dissociation constant (Ka) = 4.3 ×…

Q: Using only the Henderson-Hasselbalch equation, what is the pH of a solution that is 0.22M phenol,…

A: Given: Molarity of phenol = 0.22 M Molarity of sodium phenoxide = 0.29 M Ka of phenol = 1.3×10-8

Q: Calculate the ratio of ammonium chloride to ammonia that is required to make a buffer solution with…

A: Given data,pH=9.0Ka=5.6×10-10we know,pKa=-logKa=-log(5.6×10-10)=9.25

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

A:

Q: You were asked to estimate the pH of a 15mL of 0.09N of HCl when 16.9mL of 0.085N NaOH is added to a…

A:

Q: Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M…

A: 4-chlorobenzoic acid is a weak acid. The chemical equation for the given question may be written as:…

Q: A chemist titrates 160.0 mL of a 0.3272M nitrous acid (HNO₂) solution with 0.3027M KOH solution at…

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

Q: An analytical chemist weighs out 0.118 g of an unknown triprotic acid into a 250 mL volumetric flask…

A: Mass of the triprotic acid = 0.118 g Volume = 250 mL Molarity of NaOH = 0.1100 M Volume of NaOH…

Q: solutions.  BB- is  basic form of the indicator.             HBB    +     H2O          H3O+      +…

A:

Q: what is the pH of a solution prepared by mixing 50.0 mL of 0.125 M amonia and 25.0 mL of 0.100 M…

A:

Q: An analytical chemist is titrating 120.4 mL of a 0.5800M solution of piperidine (C5H₁0NH) with a…

A: Volume of piperidine= 120.4 mL  Volume of piperidine=0.5800M  Concentration of HNO3=0.7600M  Volume…

Q: Given 1.00 L of a solution that is 0.100 M in sodium propionate (NaC3H5O2 ) and 0.300 M in propionic…

A:

Q: Calculate the pH of a 1.00L solution containing 0.52M sodium acetate and 0.48M acetic acid after the…

A: Given that, concentration of CH3COONa in 1 L solution = 0.52 M = 0.52 mole L-1 and concentration of…

Q: Calculate the pH for each of the cases in the titration of 25.0 mL of 1.50 M pyridine, C5H5N(aq)…

A: Given,Molarity of C5H5N = 1.50 Mvolume of  C5H5N = 25.0 mLMolarity of HBr = 0.500 Mvolumes of HBr…

Q: KHP(aq) + NaOH(aq) -> H2O (l) + KNaP(aq) 1. If we forgot to add the phenolphthalein indicator, why…

A: 1. If we forgot to add the phenolphthalein indicator, we will be unable to determine the NaOH…

Q: NOTE: The following 4 questions involve the titration of a 50.00 mL sample of 0.200 M chlorous acid,…

A: Weak acid is one that does not dissociates completely in aqueous solution rather it maintains an…

Q: A chemist titrates 80.0 mL of a 0.0754M aniline (CH, NH,) solution with 0.5961M HBr solution at 25…

A: At equilibrium point acid and base are neutralized completely to give salt. So moles of salt formed…

Q: after titrating

A: Mmol of Acid = 0.10 × 40    = 4.0 mmol Mmol of KOH = 20 ×0.20   = 4.0 mmol It forms Amphoteric salt,…

Q: Suppose in the following reaction we begin with 0.250M of HCN. What is the pH at equilibrium. Note…

A: HCN is a weak acid. It is dissociated as H+ ions and CN- ions.

Q: calculated after 12.5 mL of titrant is added? Group of answer choices The pH is based on the…

A: reaction after adding HCl, F- + H+ ---> HF  Mmol of F- = M × V . = 25 ×0.1 = 2.5 mmol Mmol of…

Q: Say I am titrating 10 mL of H3PO4 with NaOH. It took 5 mL of NaOH to reach the first equivalence…

A: The objective of this question is to calculate the concentration of the weak acid, H3PO4, at the…

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:

Q: 51.8 mL of 0.1025 M methylamine (CH3NH2) is titrated with 0.0546 M HI. Determine the pH of the…

A: Given that, Volume of 0.1025 M methylamine, CH3NH2  = 51.8 mL = 0.0518 L Moles of methylamine in…

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…

A: Acid-base titration is an analytical technique utilized to determine the unknown concentration of an…

Q: A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN =…

A:

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.