Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+ (aq) + 2I- (aq)  →  PbI2 (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing  45.0 g of  Pb(NO3)2 (aq) to completely precipitate the lead?

Apply the concepts of stoichiometry and solution concentration in this section.  Potassium iodide reacts with lead (II) nitrate in the following precipitation reaction 2 KI (aq)  + Pb(NO3)2 (aq)       KNO3 (aq)    +  PbI2 (s). What volume of 0.200 M KI solution is required to completely precipitate all of the lead in 255mL of a 0.312 M Pb(NO3)2 solution?           An solution is made by dissolving 28.4 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 378 mL. Calculate the molarity, molality, mole fraction, mole percent and mass percent of the solution,                          Hydrochloric acid is usually purchased in a concentrated form that is 37.0 % HCl by mass and has a density of 1.20 g/mL. Describe exactly how to prepare 2.85 L of a 0.500 M HCl to be used in Dr. Henary’s CHEM1211K lab from the concentrated solution. Hint (Find molarity of concentrated solution and use dilution equation. This is how your solution are prepared)

A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)₂(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 18.46 g PbCl₂ (s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)₂(aq) solution. concentration: M Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books

5.00 mL of 2.5 M NaCl(aq) is diluted with water to the calibration line in a 100.00 mL volumetric flask. What is the concentration of the new solution?

Calculate the number of milliliters of 0.587 M KOH required to precipitate all of the Mg²+ ions in 102 mL of 0.753 M MgCl₂ solution as Mg(OH)2. The equation for the reaction is: MgCl₂ (aq) + 2KOH(aq) → Mg(OH)2 (s) + 2KCl(aq) Volume = mL

If 33.0 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₂), how many grams of Ni(OH), will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO₂)₂(aq) → Ni(OH)₂ (s) + 2 NaNO, (aq)

In a laboratory experiment, a 19.0 −mL−mL sample of KClKCl solution is poured into an evaporating dish with a mass of 24.60 gg . The combined mass of the evaporating dish and KClKCl solution is 43.50 gg . After heating, the evaporating dish and dry KClKCl have a combined mass of 29.93 g   What is the molarity (M) of the KCl solution?

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.390M silver nitrate (AgNO,) solution to a 45.0 g sample of the fluid and collects the solid silver chloride (AgCl) product. When no more AgCl is produced, she filters, washes and weighs it, and finds that 1.8 g has been produced. The balanced chemical equation for the reaction is: Cl(aq) + AgNO, (aq) What kind of reaction is this? AgCl(s) + NO, (aq) If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has 2 significant digits. precipitation O acid-base O redox 0 0 0 0% 0° 0 0..9 X 5 A

Suppose you took a 3.00 mL sample of HNO3 (aq) of an unknown concentration, and find that you have to add 20.30 mL of 0.106 M NaOH from your buret to neutralize the acid.  How many moles of OH- Ions are neutralized in this reaction?

A 28.00 mL sample of an unknown HClO4 solution requires titration with 20.42 mL of 0.2100 MNaOH to reach the equivalence point. What is the concentration of the unknown HClO4  solution? The neutralization reaction is HClO4(aq)+NaOH(aq)→H2O(l)+NaClO4(aq) Express your answer using four significant figures.