As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)−4.Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3K2CO3 and all ammonium is present as NH4Cl.NH4Cl.
A 5.075 g5.075 g soil sample was dissolved to give 0.500 L0.500 L of solution. A 100.0 mL100.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+K+ and NH+4NH4+ ions completely.
Compound | Formula mass |
---|---|
KB(C6H5)4KB(C6H5)4 | 358.33 g/mol358.33 g/mol |
NH4B(C6H5)4NH4B(C6H5)4 | 337.27 g/mol337.27 g/mol |
K2CO3K2CO3 | 138.21 g/mol138.21 g/mol |
NH4ClNH4Cl | 53.492 g/mol53.492 g/mol |
B(C6H5)−4+K+⟶KB(C6H5)4(s)B(C6H5)4−+K+⟶KB(C6H5)4(s)
B(C6H5)−4+NH+4⟶NH4B(C6H5)4(s)B(C6H5)4−+NH4+⟶NH4B(C6H5)4(s)
The resulting precipitate amounted to 0.251 g.0.251 g. A new 200.0 mL200.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH+4NH4+ as NH3.NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.149 g0.149 gof precipitate.
Find the mass percentages of NH4ClNH4Cl and K2CO3K2CO3 in the original solid.
mass percentage of NH4ClNH4Cl:
%%
mass percentage of K2CO3K2CO3:
%
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content...
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na*B(C,H,7. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non-negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4CI A 5.075 g soil sample was dissolved to give 0.500 L of solution. A 100.0...
Anion analysis
POSTLABORATORY ASSIGNMENT 1. An iodide/chloride/sulfate unknown solution gave a yellow precipitate with AgNO The supernate did not react with Ba(NO)). The yellow precipitate did not dissolve in NH, H,O. After centrifuging the supernate was acidified with HNO, and gave a white precipitate. State the ion(s) present in the unknown solution. An iodide/chloride/sulfate unknown solution plus AgNO, gave no reaction. The solution was treated with Ba(NOs)2 and produced a white precipitate. State the ion(s) present in the unknown solution....
Part A.
Use the attached flow chart of a qualitative analysis separation
and identification scheme to answer the following question.
What ion is present in solution if the following observations
were seen (enter your answer as the chemical symbol without the
charge)
Addition of HCl: no precipitate
Addition of NH3/NH4Cl: a precipitate
forms
Addition of NaOH and H2O2: no
precipitate
Heat to remove H2O2 and addition of HCl: a
colorless solid is formed
Addition of HCl, Aluminon and NH3: a...
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need help on question 2a,b,c and 3a,b,c on the post lab.
Experiment EQ-309 Post-Lab Questions Determination Of An Equilibrium Constant (To be answered in the "Analysis" section of your lab report) 1 a) Calculate the molarity of the silver nitrate solution provided. b) Calculate the molarity of the sodium chloride solution provided. 2 a) Use the data from each titration to calculate the value of K for the reaction, Ag(NH)2+ + Cl" - AgCl, + 2 NH, b) Calculate...
CHEM 101 LAB 7 PRELAB QUESTIONS B C AND D
Experiment 7 Preparation of Alum PURPOSE oF EXPERIMENT: Prepare KAI(So,)2 12H20, an aluminum alum, from aluminum metal. (Note: ExPERIMENT 8 describes the gravimetric analysis of the sulfate content in alum.) Alums have the general formula MM(So) 12HO, where M* is commonly Na". K', Tl., NH,., or Ag, and Mt''is A广, Fe". Cr". Ti". or Co. . Samples of these compounds have a variety of uses in our everyday lives. Sodium...
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only need g, h and I please
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Please help me! Thank you so much!
2. Give chemical equations for the following: a. Precipitating the silver ion by adding hydrochloric acid b. Precipitating the copper ion by adding sodium sulfide c. Dissolving the copper sulfide in concentrated nitric acid to precipitate sulfur. (The orange gas that you saw is NO, product, and sulfur precipitate can be shown as "S") d. Confirming the identity of the ion as copper by adding potassium ferricyanide. (Pote is only a spectator ion...
Analysis of Vinegar EXPERIMENT NAME SECTION DATE POSTLABORATORY ASSIGNMENT 1. A standard nitric acid solution is prepared using 0.425 g of sodium carbonate, NaCO3. Find the molarity of the acid if 33.25 mL are required to reach a permanent endpoint. 2 HNO, (aq) + Na2CO3(s) + 2 NaNO3(aq) + H2O(l) + CO2(g) 2 H OT 2. A 10.0-ml sample of household ammonia solution required 27.50 mL of 0.241 M HNO3 for neutralization. Calculate (a) the molar concentration of the ammonia...