When we combine two aqueous salts with the same anion: A. PRECIPITATE B. NO REACTION When we combine two aqueous salts with the same cation: A. PRECIPITATE B. NO REACTION Generally, which cations produce precipitates? Barium Calcium Sodium Potassium Silver Generally, which anions never seem to produce precipitates? chlorides sulfates carbonates nitrates

The concentration of CO in air is determined by passing a known volume of air through a tube that contains I2O5, forming CO2and I2. The I2 is removed from the tube by distilling it into a solution that contains an excess of KI, producing I3-. The I3-is titrated with a standard solution of Na2S2O3. In a typical analysis a 4.79-L sample of air is sampled as described here, requiring 7.17 mL of 0.00329 M Na2S2O3 to reach the end point. If the air has a density of 1.23 × 10–3 g/mL, determine the parts per million CO in the air

Give detailed Solution with explanation needed..don't give Handwritten answer..

A student was given Mg, Zn, Fe, and Cu metals He put each of them in dil HCIcontained in different test tubes Identify which of them(i) will not displace 112 from dli HCI(ii) forms a pale green substance(iii) will give 112 with 5% 11N0(iv)will be displaced from its salt solution by all other metals

A sample of alfalfa meal weighing 2.0 g is analyzed by Kjeldahl method for the percentage of nitrogen. The liberated NH3 is caught in a solution of H3BO3, and 8.23 ml of HCl are required in the subsequent titration. A sample of pure (NH4)2SO4 (132.12) weighing 0.61 g is treated with excess NaOH and the liberated NH3 (17.04) is also caught in H3BO3. The resulting solution requires 20 ml of the acid for titration. Calculate the percentage of protein in the sample using 6.25 as the factor.

G.159.

The level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.

A compound is known to be Na2CO3, Na2SO4, NaOH, NaCL, NaC2H3O2 or NaNO3-. When barium nitrate solution is added to a solution containing the unknown a white precipitation forms. No precipitate is onserved when a magnesium nitrate solution is added to a solution containing the unknown. What is the identity of the unknown compound? Explain reasoning

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I need the net ionic equation for the reactions below:  -Dissolution of silver oxalate with nitric acid -Dissolution of silver chloride with aqueous ammonia -Oxidation of the iodide ion by hypochlorite solution -Precipitation of the sulfate ion with barium ion -Dissolution of barium phosphate solution with hydrochloric acid -Reaction of sodium phosphate solution with hydrochloric acid -Reaction of phosphoric acid with ammonium molybdate solution -Precipitation of the oxalate ion with calcium ion -Reaction of calcium axalate with sulfuric acid -Reaction of oxalic acid with acidic permanganate solution -Production of carbon dioxide from solid sodium carbonate and hydrochloric acid -Production of acetetic acid or ethyl acetate in sulfuric acid  Thank you