The following molecular equation represents the reaction that occurs when aqueous solutions of lead(II) nitrate and cobalt(II) bromide are combined. Pb(NO3)2(aq) + CoBr2 (aq) → PbBr2 (s) + Co(NO3)2 (aq) Write the balanced net ionic equation for the reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)

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)

Consider the following unbalanced precipitation reaction:    CuBr2 (aq) + KOH (aq) → KBr(aq) + Cu(OH)2 (s)   Provide the net ionic equation for this reaction. I will be looking for charges, subscripts, coefficients, and states. The X2 button can be used to provide superscripts and X2 button can be used to provide subscripts.

The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding silver nitrate, it is possible effectively to remove all chloride ion from the sample. Ag+(aq) + Cl-(aq) → AgCl(s) Suppose a 1.515 g sample is known to contain 27.5% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample?

Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(II) to insoluble Fe(III): $$4Fe(OH)+(aq)+4OH−(aq)+O2​(g)+2H2​O(l)4Fe(OH)3​(s)  How many grams of O2 are consumed to precipitate all of the iron in 75.0 mL of 0.0350 M Fe(II)?

Complete and balance the equation for the single displacement reaction between sodium and lead (II) nitrate. Phases are optional. Balanced equation: Na(s)+Pb(NO3)2(aq) =

How many millilitres of 0.450 mol L−1 H2SO4(aq) are required to completely neutralize 46.7 mL of 0.930 mol L−1 KOH(aq) ? Hint: Write a balanced chemical equation for the reaction.   Give your answer in mL, accurate to three significant figures. Do not include units as part of your answer.

For each of the following reactions, suggest two soluble ionic compounds that, when mixed together in water, result in the net ionic equation given: (a) 2 Ag+ (aq) + CO3²¯ (aq) → Ag₂CO3(s) (b) Mg²+ (aq) + 2 OH¯(aq) → Mg(OH)₂(s), the suspension present in milk of magnesia 3+ (c) 3 Ca³+ (aq) + 2 PO2 (aq) → Ca3(PO4)2(s), gypsum, a component of concrete

Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(II) to insoluble Fe(III): 4Fe(OH)* (aq) +40H (aq) + O₂ (g) + 2H₂O(1)→→→→→→ 4Fe(OH)3 (s) How many grams of O₂ are consumed to precipitate all of the iron in 70.0 mL of 0.0550 M Fe(II)?

Write the net ionic equation for the reaction when solutions of magnesium sulfide (MgS) and copper (1) nitrate (CUNO3) are mixed given the reaction below: Reaction: MgS (aq) + 2 CuNO3 (aq) → Mg(NO3)2(aq) + Cu₂S (s) Be sure to write out the complete ionic reaction first to find which ions are spectator ions.