The substance to be analyzed – is white, highly soluble in water salt. Interaction with concentrated sulfuric acid leads to evolving of reddish-brown gas with pungent odour. Addition of ammonium oxalate leads to formation of white precipitate, which is insoluble in acetic acid. Diphenylamine reaction turns color of the solution to violet. What kind of salt is this? Ca(NO3) 2 NaNO2 KBrO3 MgCl2
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- From the following data find the percentages of Na2CO3 and NaHCO3 in a mixture of these chemicals and inert constituents: a) A 0.5000 g sample required 45.50 mL 0.1050 N HCl to reach the methyl orange end point. b) 25.00 mL of 0.1000 N KOH is added to 0.2500 g of the sample; BaCl2 is added to precipitate the BaCO3 and 12.00 mL 0.1050 N HCl is required to reach the phenolphthalein end point.Of the five salts listed below, which has the highest concentrationof its cation in water? Assume that all salt solutionsare saturated and that the ions do not undergo any additionalreactions in water.(a) lead(II) chromate, Ksp = 2.8 x 10-13(b) cobalt(II) hydroxide, Ksp = 1.3x 10-15(c) cobalt(II) sulfide, Ksp = 5 x 10-22(d) chromium(III) hydroxide, Ksp = 1.6 x 10-30(e) silver sulfide, Ksp = 6 x 10-51Which salt would you expect to dissolve readily in acidic solution, calcium phosphate, Ca3(PO4)2, or calcium sulfate, CaSO4? Give an explanation.
- Compare the solubility of magnesium carbonate in each of the following aqueous solutions: Clear All 0.10 M Mg(CH3C00), More soluble than in pure water. 0.10 M (NH4)2C03 Similar solubility as in pure water. 0.10 M NACH3CO0 Less soluble than in pure water. 0.10 Μ ΚΝΟA mineral contains 6.6% (w/w) of K20. What weight of this mineral must be taken to obtain a KCIO4 precipitate weighing 0.4100 g?A 1.000-gram sample of NaOH (39.997 g/mol) which has been exposed to the air for some time (NaOH will adsorb water and CO2 from the ambient air) is dissolved in water and then diluted to 500.00 mL. 100.0 mL of this solution required 38.60 mL of 0.1062 M HCl to be titrated to the endpoint (~pH 3). A second 100.00 mL portion is treated with excess BaCl2 and then diluted to 250 mL and filtered. 200 mL of the filtrate required 29.62 mL of HCl to titrate to the (~pH 8-9) endpoint. Calculate the mass percentage of NaOH and Na2CO3 (105.9898 g/mol) in the original sample. The adsorbed CO2 is converted to Na2CO3. The Ksp for BaCO3 (s) is 2.58 x 10-9.
- 2.413 g sample contains Na2CO3, NaHCO3 and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO3 and Na CO in sample (Na CO =106.0 g/mol, NaHCO =84.02 g/mol)Which of the following salts would you predict to also produce bubbles in a chemical reaction withHCl? K2SO4,KHCO3, KCl, Ca(OH)2 and MgCO3The substance to be analyzed coloration test gives carmine red color. Interaction with concentrated sulfuric acid leads to evolving of gas with pungent odour. Interaction with weak sulfuric acid solution leads to white precipitate formation. Interaction with water solution of silver nitrate leads to formation of white curdy precipitate, which soluble in is white, highly soluble in water salt. Flame saturated ammonium carbonate solution. What kind of substance is this? SrCl, NaNO 2 MgCl, Ca(NO3) 2
- Compare the solubility of lead carbonate in each of the following aqueous solutions: Clear All 0.10 M Pb(NO3)2 More soluble than in pure water. 0.10 M K2CO3 Similar solubility as in pure water. 0.10 M ΝΗANO; Less soluble than in pure water. 0.10 M NACH3C00When 10 drops of 0.1 M Co2+ is acidified using 20 drops 6.0 M CH3COOH and a pinch of solid NaNO2 is added then placed in a warm water bath, an orange solution is observed. Write the net ionic equation associated with the formation of the orange solution and indentify which species is responsible for this color change.A solution of unknown group I ions gives a white precipitate with HCl.When treated with hot water, it gives a solution to which K2CrO4 is added, and a yellow precipitate forms.The white precipitate that remains after the hot water treatment dissolves completely in NH3. Which ions are present and which are not?