A 0.660 g sample of a mixture containing only NaBr and CaBr, is dissolved in water. An excess of an aqueous solution of Pb(NO₂), is added. The PbBr, that forms is filtered, dried, and weighed. The mass of PbBr, is found to be 1.20 g. What is the mass of Br ions in the sample?

What volume (in mL) of water must you add to 50.0 mL of a 0.600 M LiBr solution to produce a 0.185 M solution? Assume the volumes are additive.

a) What is the maximum amount of salt (in molecules) that can be produced when 35 mL of 0.102 M of strontium hydroxide reacts with 12 mL of 0.321 M nitrous acid?         Does the reaction result in a basic, neutral or acidic solution?

1. If 30.4 g of Nal (MM=149.89g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of Nal in the resulting solution? 2. What volume (in L) of 1.1 M FeCl3 would be required to obtain 0.59 moles of Cl- ions?

if 38.0 g of KCl (MM=74.55 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KCi in the resulting solution?

3. A student followed the procedure of this experiment to determine the percent NaOCl in a commercial bleaching solution that was found in the basement of an abandoned house. The student diluted 50.00 mL of the commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mL aliquot of the diluted bleaching solution. The titration required 35.46 mL of 0.1052M Na,5203 solution. A faded price label on the gallon bottle read S0.79. The density of the bleaching solution was 1.10 g mL-? h. Calculate the mass of one gallon of the commercial bleaching solution. i. Calculate the cost of 100 g of the commercial bleaching solution. j. Determine the cost of the amount of commercial bleaching solution required to supply 100 g of NaOCl.

Assume the given amount of RbF fully dissociates in water. Calculate the molarity of a solution if 145.20 g of RbF are dissolved into a solution of water that has a final volume of 2.00 L.

14.4 g of magnesium nitrate is dissolved in 1.20 L of water. 25 mL of this solution is taken and diluted to 175 mL with water. What is the final concentration of the nitrate ion?

b) The solubility rules provide a qualitative assessment of what combination of ions will form a precipitate when mixed in water. However, what general statement can be made regarding the solubility of all ionic compounds? Why? c) Explain why gases dissolve less in solution when the solution is heated?

A precipitation reaction involves the formation of a precipitate when aqueous solutions are mixed. Not all combinations of aqueous solutions produce precipitates, and it is important to be able to predict the ones that do. A) Complete and balance the molecular equation for the reaction between aqueous solutions of lithium fluoride and potassium chloride, and use the states of matter to show if a precipitate forms. B) Write the complete ionic equation for the reaction that takes place when aqueous solutions of lithium fluoride and potassium chloride are mixed.   C) Write the net ionic equation for the precipitation reaction, if any, that may occur when aqueous solutions of lithium fluoride and potassium chloride are mixed. If there is no net ionic equation, simply write "none."