Gold has compounds containing gold(1) lon or gold(II) lon. A compound of gold and chlorine was treated with a solution of silver nitrate, AGNO,, to convert the chloride lon in the compound to a precipitate of AgCl. A 1.791 mg sample of the gold compound gave 1.105 mg AgCl. cCalculate the percentage of the chlorine in the gold compound. Percentage=

If 23.9 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of CH₃OH in the resulting solution?

If 30.0 g of NaI (MM = 149.89 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of NaI in the resulting solution?

A sample of solid Mg(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Mg(OH)2 as it could hold. A 450-mL sample of this solution was withdrawn and titrated with 0.00357 M HClO4. It required 58.3 mL of the acid solution for neutralization.What is the solubility of Mg(OH)2 in water, at the experimental temperature, in grams of Mg(OH)2 per liter of solution?

A student weighs out a 3.48 g sample of manganese(II) chloride, transfers it to a 125 mL volumetric flask, adds enough water to dissolve it and then adds water to the 125 mL tic mark. What is the molarity of MnCl, in the resulting solution?

A 10.00 ml sample of a solution of acetic acid in water was titrated to the endpoint by the addition of 15.89 ml of 0.2432 M NaOH. Calculate the volume of this NaOH solution that would be required to titrate 50.00 ml of vinegar. Vinegar is 5.00% (by mass) acetic acid. Assume that the density of the vinegar solution is the same as that of water (1.00 g/ml).

A 2.85 g sample of NaCl and CaCl2 was dissolved in water, and an excess of AgNO3 was added to precipitate all of the chloride ions.The AgCl was collected and dried, and weighed to give 7.20 g of AgCl. How much NaCl and CaCl2 was in the sample? i g NaCl g CaCl2

What mass of Naz CrO4 is required to precipitate all of the silver ions from 20.0 mL of a 0.200 M solution of AgNO, ? Mass =

What mass of iron(III) hydroxide precipitate can be produced by reacting 76.0 mL of 0.290 M  iron(III) nitrate with 194 mL of 0.130 M  sodium hydroxide

A sample is a mixture of the salts and silver nitrate, copper (II) chloride, and iron (III) chloride. When a 1.000 g sample of the mixture is dissolved in water and reacted with excess silver nitrate, 1.7809 g of precipitate forms. When a separate 1.000g sample of the mixture is treated with a reducing agent, all the metal ions in the sample are reduced to pure metals. The total mass of the metals produced is 0.4684g. Calculate the percent of each salt in the original mixture.