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PLS ANSWER ASAP HUHU I ONLY HAVE 5 MINS. LEFT :(
Calculate the ionic strength of a 0.030 M Al2(CO3)3
a. 0.05
b. 0.45
c. 0.02
d. 0.54
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- Which has an acitivity coeeficient closest to 1 with ionic strength = 0.001 M? a. Lithium ion b. Magnesium ion c. Lead ion d. Aluminum ion(a) How many coulombs are required to reduce 1 mole Cr2O72- to Cr3+?(b) The conductivity of 0.001 M acetic acid is 4 × 10-5 S/m. Calculate the dissociation constant of acetic acid if [latex]\Lambda_{\mathrm{m}}^{0}[/latex],for acetic acid is 390 S cm2 mol-1.Dilution is done to commercially available acids such as HNO3, H2SO4 etc so that the strength is increased and so it will be safe to be used by students in a chemistry laboratory. Select one: True False
- In an experiment to check chemical balance, measurements of electrical conductivity (κ) were made of acid solutions in different concentrations, as shown in the table below. From these data, show that the acetic acid dissociation equilibrium constant is really a constant, that is, it has the same value for any acetic acid solution at a given temperature. The data were collected at 25 oC. The limit molar conductance of the acetic acid solution is Λ0 = 390.71 Ω^-1*cm^2 / mol. Suggestion: calculate the molar conductance (Λm = 1000 κ / c) for each concentration and then use Ostwald's Dilution Law Molarity c (mol / L) Conductivity κ (Ω^-1*cm^-1) 0.010 1.5590 x 10^-4 0.05 3.5939 x 10^-4 0.1 5.0610 x 10^-4 ANSWER: values close to 1.7 x 10^-5 I need the calculations to show how to obtain this valueSulfide ion (S2- ) is formed in wastewater by the action of an aerobic bacteria on organic matter. Sulfide can be readily protonated to form volatile, toxic H2S. In addition to the toxicity and noxious odor, sulfide and H2S cause corrosion problems because they can be easily converted to sulfuric acid when conditions change to aerobic. One common method to determine sulfide is by coulometric titration with generated silver ion.At the generator electrode, the reaction is Ag Ag+ + e-. The titration reaction is S2- + 2Ag+ Ag2S(s). (a) A digital chloridometer was used to determine the mass of sulfide in a wastewater sample. The chloridometer reads out directly in ng Cl-.In chloride determinations, the same generator reaction is used,but the titration reaction is Cl- + Ag+ AgCI(s). Derive an equation that relates the desired quantity, mass S2- (ng), to the chloridometer readout in mass Cl- (ng). (b) A particular wastewater standard gave a reading of 1689.6 ng Cl-. What total charge in coulombs was required to generate the Ag+ needed to precipitate the sulfide in this standard? (c) The following results were obtained on 20.00-mL samples containing known amounts of sulfide.17 Each standard was analyzed in triplicate and the mass of chloride recorded. Convert each of the chloride results to mass S2- (ng). (d) Determine the average mass of S2- (ng), the standard deviation, and the %RSD) of each standard. (e) Prepare a plot ofthe average mass of S2- determined (ng) versus the actual mass (ng). Determine theslope, the intercept, the standard error, and the R2 value. Comment on the fit of the data to a linear model. (f) Determine the detection limit (ng) and in parts per million using a k factor of 2 (see Equation 1-12). (g) An unknown wastewater sample gave an average reading of 893.2 ng Cl. What is the mass of sulfide (ng)? If 20.00 mL of the wastewater sample was introduced into the titration vessel, what is the concentration of S2- n parts per million?2 table spoon solution with 10% w/v were diluted to 1 quart with water, what be ratio strength (w/v) the dilution? explain easy
- In lab, we calculated the pKa for weak acids with a pH electrode and then graphing it, but we did not do so for HCl, a strong acid. Why is it?The concentration of ammonia in a water sample can be measured by electrode. Why does the pH of each sample need to be adjusted with NaOH prior to measurement? don't reject genuine expert solve i will upvoteA pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanation