A solution of calcium chloride (100.0 mL, 1.00 M) is mixed with ammonium phosphate (100.0 mL, 1.00 M). Calculate the concentration of all ions in solution (assume 200.0 mL total volume) and determine the mass of precipitate formed in the reaction.

Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of manganese(II) sulfate and ammonium carbonate are combined. Do not include states such as (s) or (aq). It is not necessarry for you to indicate which of the products is the precipitate.

Suppose 31.0 mL of 0.510 M CoCl2   solution is added to 72.0 mL of 0.180 M NiCl2 solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive. Concentration of Co2+ =  mol/L Concentration of  Ni2+=  mol/L Concentration of Cl- =  mol/L

4. When a solutions of aluminum sulfate and potassium hydroxide are mixed, a precipitate forms. a. Write a balanced net ionic equation for the reaction. b. Calculate the mass of the precipitate when 3.89 g of aluminum sulfate in 100mL of solution is combined with 50 mL of the o.300 M KOH. c. What is the molarity of the ion in excess? (Ignore the spectator ions and assume that volumes are additive)

1. Observe the physical properties of sulfur and antimony at room temperature. Note their physical state, color and solubility in carbon disulfide. The solubility may be observed qualitatively by dissolving a pinch of the powdered samples in about 3 ml of carbon disulfide and stirring until the solid sample has dissolved. Record your observations in the table below. Solubility in CS, Classification of the sample (Element/Compound) Sample Physical Color State Sulfur Antimony a. Was the system formed by the addition of sulfur to CS,, homogeneous or heterogeneous? b. Could its composition be varied or not? c. Explain your answer in la. d. Was the system formed by the addition of antimony to CS, homogeneous or heterogeneous? e. Explain your answer in 1d.

If 50.0 mL of 0.150 M CaCl 2 is added to 35.0 mL of 0.100 M AgNO 3, what is the mass in grams of AgCl precipitate?

3) When excess sliver nitrate was added to 25.00 ml of barium chloride, a precipitate of sliver chloride formed at the bottom of the beaker. If the mass of the precipitate was 4.30g, calculate the initial concentration of barium chloride.

An experiment was carried out as follows: 1.5766 g of an ammonium salt was placed in a beaker and 60 mL of 1.182 M sodium hydroxide was added. The resulting mixture was heated for about an hour and then left to cool to room temperature. The reaction mixture was then titrated with sulfuric acid and required 18.35 mL of the acid for complete neutralization. Given that the percentage by mass of ammonium in the salt was 37.5%, calculate the molarity of the sulfuric acid used in the titration.

A 0.7011-g mixture of sodium chloride and sodium nitrate is completely dissolved in water. When silver nitrate is added to the solution, 0.9805 g of solid precipitate. What is the percent by mass of chloride in the initial mixture? 65.41 % 71.50 % 34.59 % 13.99 % 28.50 %

A student performs the titration of hydrochloric acid with sodium hydroxide.  A 20.00 mL aliquot of the HCl solution required 30.50 mL of a 0.150 mol L-1 NaOH solution to reach the end point in the titration using a phenolphthalein indicator.  Write the balanced molecular equation for this reaction AND determine the concentration of the original hydrochloric acid solution. Give your answer to the correct number of significant figures.