Chapter 17 Matching Questions1-5 Match the following. Drag the appropriate labels to their respective targets. Reset Help 3/4 of the way to second equivalence point of a diprotic acid/strong base titration pH = 7 equivalence point of a weak base/strong acid titration pH = pK. half-way to equivalence point of a weak acid/strong base titration pH > 7 equivalence point of a strong acid/strong base titration pH < 7 pH = pK2 equivalence point of a weak acid/strong base titration

Chapter 17 Matching Questions1-5 Match the following. Drag the appropriate labels to their respective targets. Reset Help 3/4 of the way to second equivalence point of a diprotic acid/strong base titration pH = 7 equivalence point of a weak base/strong acid titration pH = pK. half-way to equivalence point of a weak acid/strong base titration pH > 7 equivalence point of a strong acid/strong base titration pH < 7 pH = pK2 equivalence point of a weak acid/strong base titration

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter12: Spectrochemical Methods

Section: Chapter Questions

Problem 15P

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalenc
What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Please present complete solution. Express your final answers up to two (2) decimal places.
50.0 mL of 0.0500 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HI. Calculate the pH after the following volumes of titrant have been added: (d) 18.8 mLpH = (e) 25.0 mLpH = (f) 42.5 mLpH =
Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
C. When a strong acid titrant (e.g. HCl) is added to a weak base (B2-) capable of accepting two protons, the following reactions occur: (vi) B2-(aq) + H+(aq) -> HB-(aq) (vii) HB-(aq) + H+(aq) -> H2B(aq) Note: single arrow to the right rather than double arrow means the reactions go to completion 11. Which region/point (A,B,C,D,E, or F) is where the titration begins and B2- is the predominant species in solution ? ____________ 12. Which reaction (vi or vii) dominates at higher pH values? _____________ 13. Halfway through which region (A,B,C,D,E, or F) is where the pH = pKa2 ? ____________ 14. Which species (H2B, HB-, or B2-) predominates at "C", the equivalence point 1 ? _____________ 15. During the titration, which region (A,B,C,D,E or F) on the curve represents the first buffer region for the base? _____________ ? Second buffer region _____________ ?
Please help me fill out this table! Answering just one of the columns is good enough, thank you! Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration _?_mmol _____mmol Millimoles of acetic acid in sample _?_mmol ______mmol Molar concentration of acetic acid solution _?_mol/L ______mol/L
It is necessary to prepare 0.100 liters of buffer pH 4.70 with a concentration of 0.250 M, from a solution of acetic acid at 55.0% m/m (density = 1.010 g/mL) and sodium acetate of purity 97.0 %, how many g of salt do I need? (Ka = 1.78 x 10-5) (Note significant figures).
please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically greater than the moles of the analyte? post-equivalence pre-equivalence equivalence end stage
Construct a curve for the titration of 20.00 mL 0.0500 N succinic acid (HO2CCH2CH2CO2H) by 0.1000 N NaOH solution. MS Excel® can be used. Titrant volumes: 15.00 mL, 20.00 mL, and 25.00 mL. (CH2)2(CO2H)2 ⇌ (CH2)2(CO2H)(CO2)^− + H^+ Ka1 = 6.21 × 10^-5; pKa1 = 4.207 (CH2)2(CO2H)(CO2)− ⇌ (CH2)2(CO2)2^2− + H^+ Ka2 = 2.31 × 10^-6; pKa2 = 5.636