Use the data below for the concentrated acids and bases.Specificgravity1.050.901.19ReagentConcentration%w/w99.7Acetic acidAmmoniaHydrochloric acidHydrofluoric acidNitric acidPerchioric acidPhosphoric acidSulfuric acid29.037.249.51.151.4270.571.086.096.51.671.711.84What is the volume (in deciliter) of conc HCI needed to prepare 1000 mL of 9.89 N HCI? Molar mass of HCI is 36.458.Express answer in 2 decimal places. No need to write the unit in the answer box.

we can prepare a diluted solution from concentrated stock solution using dilution law

Answered: Use the data below for the concentrated…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 15P

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Give clear handwritten answer- Show how conductivity measurements may be used to determine the dissociation constant of a weak acid or base.
Oxalic acid (H2C2O4) is a diprotic acid with Ka1=5.6×10-1 and Ka2=1.5×10-4. Oxalate ion (C2O42-) also has two base dissociation constants, Kb(1) =6.5×10-11 and Kb2=1.8×10-14. Based on these values, deduce the formula to compute the base dissociation constants of oxalate ion in terms of Kw and Ka1 or Ka2.
Both H2PO3−H2PO3− and HS−HS− are amphoteric. Write an equation to show how H2PO3−H2PO3− can act as a base with HS−HS− acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. then Write an equation to show how H2PO3−H2PO3− can act as an acid with HS−HS− acting as a base. Express your answer as a chemical equation. Identify all of the phases in your answer.
Complete the flow chart below to describe the separation of an acid and base mixture by providing the necessary chemical structures.
Oxalic acid (H2C2O4) is a diprotic acid with Ka1 = 5.6x10-1 and Ka2 = 1.5x10-4. Oxalate ion (C2O42-) also has two base dissociation constants, Kb1 = 6.5x10-11 and Kb2 = 1.8x10-14. Based on thesevalues, deduce the formula to compute the base dissociationconstants of oxalate ion in terms of Kw and Ka1 or Ka2
Predict the Nature of the Adduct between the hard acid/base and soft acid/base with examples for each case.
Which of the following samples (acetic acid, monochloroacetic acid, acetamide, acetone, isopropyl alcohol, phenol) are classified as stated below. Support your answer by writing the structural formula and encircling the part that makes it acidic, basic or neutral as the case may be: a. Bronsted-Acid b. Bronsted-Base c. Lewis acid d. Lewis base e. Neutral
Calculation of pH and % ionization with any assumptions clearly noted. (submit all work. Include units and pay attention to significant figures 0.150 M propanoic acid (CH3CH2CH2COOH)
a. Acetic acid and monochloroacetic acid b. Acetamide and acetone c. Glycine and lysine d. Isopropyl alcohol and phenol 4. Which of the following sample above are classified as stated below. Support your answer by writing the structural formula and encircling the part that makes it acidic, basic or neutral as the case may be: a. Bronsted acid b. Bronsted base c. Lewis acid d. Lewis base
Calculate the H3O+ concentration (M) of a 0.313 solution of a triprotic acid given the acid ionization constants below. Report your answer to to the tenths place using scientific notation (e.g., 1.2e3 or 1.2e-3) and do not include units. Ka1 = 6.4 x 10-5 Ka2 = 4.3 x 10-8 Ka3 = 7.4 x 10-12
Why do acids not show acidic behavior in the absence of water?
I just need help in the Calculations EXPERIMENT: ESTIMATION OF SODIUMHYDROXIDE USING HYDROCHLORIC ACID (CONDUCTOMETRIC TIITRATION) Aim: To determine the mass of NaOH in the given solution by conductance measurement. Apparatus & Chemicals: 0.1N, 100 ml HCl , weighing balance, burette, pipette, beaker, funnel, standard flask, glass rod, distill water Theoretical Background: When sodium hydroxide is added to HCl, the highly mobile H+ ions are replaced by less mobile metallic ions. Before the alkali is added, the acid solution has a high conductance due to the highly mobile H+ ions. Observations: Volume of NaOH added (ml) Conductance Volume of NaOH added (ml) Conductance 1 5.5 13 1.3 2 5.3 14 1.0 3 5.1 15 0.7 4 4.6 16 0.4 5 4.2 17 0.1 6 3.8 18 0.5 7 3.3 19 0.9 8 2.9 20 1.2 9 2.6 21 1.7 10 2.2 22 2.2 11 1.9 23 2.5 12 1.6 24 2.9 Calculations:…

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