A sample of `NaClO_(3)` is converted by heat to `NaCl` with a loss of `0.16g`of oxygen. The residue is dissolved in water and precipitated as `AgCl`. The mas of `AgCl` (in g) obtained will be: (Given : Molar mass of `AgCl = 143.5 g mol^(-1)`)

Solubility product of AgCl is 1.8 xx 10^(-10) . Calculate its molar solubility and solubility in g/L. Molar mass of AgCl is143.5 g mol^(-1) .

The specific conductance of saturated solution os silver chloride is k(ohm^(-1)cm^(-1)) . The limiting ionic conductance of Ag^(+) and Cl^(-) ions are x and y respectively. The solubility of AgCl in "gram liter"^(-1) is : (Molar mass of AgCl=143.5"g mol"^(-1) )

The specific conductance of saturated solution os silver chloride is k(ohm^(-1)cm^(-1)) . The limiting ionic conductance of Ag^(+) and Cl^(-) ions are x and y respectively. The solubility of AgCl in "gram liter"^(-1) is : (Molar mass of AgCl=143.5"g mol"^(-1) )

5.85 g NaCl is dissolved in 500 ml of water. The molarity is

14.625mg of NaCl is treated with AgNO_(3)(aq) .The mass of AgCl obtained as ppt is ( Ag=108g//mol )

A 1.0g sample of a pure organic compound cotaining chlorine is fused with Na_(2)O_(2) to convert chlorine to NaCl. The sample is then dissolved in water, and the chloride precipitated with AgNO_(3) , giving 1.96 g of AgCl. If the molecular mass of organic compound is 147, how many chlorine does each molecule contain ?

A 1.0g sample of a pure organic compound cotaining chlorine is fused with Na_(2)O_(2) to convert chlorine to NaCl. The sample is then dissolved in water, and the chloride precipitated with AgNO_(3) , giving 1.96 g of AgCl. If the molecular mass of organic compound is 147, how many chlorine does each molecule contain ?

A 1.0g sample of a pure organic compound cotaining chlorine is fused with Na_(2)O_(2) to convert chlorine to NaCl. The sample is then dissolved in water, and the chloride precipitated with AgNO_(3) , giving 1.96 g of AgCl. If the molecular mass of organic compound is 147, how many chlorine does each molecule contain ?