impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O

A 9.12g of KClMgCl26H2O is to be dissolved to prepare a solution in sufficient water to give 1.500L. What is the molar analytical concentration of KClMgCl2 in this solution?

A 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3.  Question: Calculate the percent by mass of Vitamin C in the Real Lemon Sample

The Kjeldahl method was used to determine the nitrogen content of a protein. A 275 µL aliquot of a 47.0 mg/mL protein solution was digested in boiling sulfuric acid. The solution was made basic and the liberated NH, was collected in 5.00 mL of 0.0512 M HCl. A volume of 7.00 mL of 0.0174 M NaOH was required to react with the excess HCl. Calculate the weight percent of nitrogen in the protein. weight percent: wt% N

15). If Ca(NO3) (aq) is slowly added to solution containing CO32– and SO42– what compound would precipitate out first given the solubility products (Ksp (CaSO4) = 2.4 x 10–5 and Ksp (CaCO3) = 8.7 x 10–9)? CaCO3 would precipitate first because it is least soluble. CaSO4 would precipitate first because it is least soluble. CaCO3 would precipitate first because it is more soluble. CaSO4 would precipitate first because it is more soluble.

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.

Ammonium sulfate is added to an unknown mixture of ions. A precipitate forms. The solution is centrifuged, and the remaining solutions is decanted. Ammonium oxalate is then added to the solution and a precipitate forms. The solution is centrifuged, and the remaining solution is decanted. Sodium monohydrogen phosphate and sodium hydroxide are added to the decanted solution, and a precipitate forms. The precipitate is centrifuged and decanted. The solid is dissolved in acid, magnesium indicator is added, then sodium hydroxide is added until the solution turns cloudy blue, which settles when centrifuged. Sodium hydroxide is added to a fresh sample of the unknown. A damp piece of litmus paper over the opening of the test tube remains red. Select the ions present.   Question 3 options:   Ba2+   Ca2+   Mg2+   NH41+