A precipitate of `AgCl` and `AgBr` weighs `0.4066g`. On heating in a current of chlorine, the `AgBr` is converted to `AgCl` and the mixutre loses `0.0725 g` in weight. Find the `%` of `Cl` in original mixture.

A mixture of CaCO_(3) and MgCO_(3) weighing 1.84 g on heating left a residue weighing 0.96 g . Calculate the percentage of each in the mixture.

A mixture of CaCO_(3) and MgCO_(3) weighing 1.84 g on heating left a residue weighing 0.96 g . Calculate the percentage of each in the mixture.

A mixture of CaCO_(3) and MgCO_(3) weighing 1.84 g on heating left a residue weighing 0.96 g . Calculate the percentage of each in the mixture.

A mixture of CaCO_(3) and MgCO_(3) weighing 1.84 g on heating left a residue weighing 0.96 g . Calculate the percentage of each in the mixture.

A" " 0.2g sample , which is mixture of NaCl, NaBr and NaI was dissolved in water and excess of AgNO_(3) was added. The precipitate containing AgCl,AgBr and AgI was filtered, dried and weighed to be 0.412g . The solid was placed in water and treated with excess of NaBr , which converted all AgCl into AgBr . The precipitate was then weighed to be 0.4881 g . It was then placed into water and treated with excess of NaI , which converted all AgBr into AgI . The precipitate was then weighed to be 0.5868 g . What was the percentage of NaCl, NaBr and NaI in the original mixture :

In the Carius method of estimation of halogen, 0.0811 g of an organic compound gave 0.2368 g of AgCl . Find the percentage of chlorive in the compound. Strategy: Find the molar mass of AgCl to calculate the moles of AgCl which is also equal to the moles of Cl , according to the formula. Using molar mass of Cl , find its mass to calculate its percentage.