A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution. This solution is then added to 165 mL of 0.015 M aqueous Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the solution via precipitation as insoluble PbBr2(s).
The precipitation reaction that occurs is: Pb2+ (aq) + 2 Br (aq) ---> PbBr2 (s)
At the end of the reaction, what is the concentration (in molarity) of nitrate ions in the solution?
Note: potassium ions would be present, because both K+ and NO3- are spectator ions, but you have only been asked about the NO3-.
The solution of question is not as trivial as the question itself.The solution just involves the calculation of Molarity of NO3- which involves the calculation of new molarity of aq lead(2) nitrate in increased volume of solution though the no of moles remain same.
A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution....
A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution. This solution is then added to 165 mL of 0.015 M aqueous Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the solution via precipitation as insoluble PbBr2(s). The precipitation reaction that occurs is: PB2+(aq) + 2Br(aq) --> PbBr2(s) What is the maximum mass of product that could be isolated by filtration after the reaction occurs?
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1. When 0.100 L of a solution containing 0.15 M KBr is added to 0.100 L of a solution containing 0.15 M Pb(NO3)2, what precipitate will form? PbBr2 PbBr Pb(NO3)2 KNO3 K(NO3)2 PbK KBr 2. What is the driving force for the reaction described in Q1 above? The formation of a new insoluble ionic compound The formation of a gas the formation of water molecules the formation of new ions the formation of a new soluble ionic compound 3. Write...
You mix a 25.0 mL sample of a 20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) ® PbCl2 (s) + 2KNO3 (aq) You mix a 25.0 mL sample of a 20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) ® PbCl2 (s) +...
23. Lead (II) bromide is prepared using the following reaction: Pb(NO3)2 (aq) + KBr (aq) → PbBra(s) + KNO3(aq) (unbalanced) How many milliliters of 1.5M Lead (II) nitrate Pb (NO3), are needed to prepare 150 grams of PbBr2 in excess potassium bromide solution. Assume you have 100% yield. Fill in the stoichiometric pathway for this problem: (2 points) Show the dimensional analysis calculation required for this problem: (3 points)
A 29.3-mL sample of a 1.22 M potassium chloride solution is mixed with 14.5 mL of a 0.860 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq)+Pb(NO3)2(aq)→PbCl2(s)+2KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.46 g. Determine the limiting reactant, the theoretical yield, and the percent yield.
You mix a 25.0 mL sample of a 1.20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) → PbCl2 (s) + 2KNO3 (aq) You collect and dry the solid PbCl2 and find that it has a mass of 3.45 g. Determine the limiting reactant, and the percent yield? How many grams of excess reactant will remain when the reaction is complete?
1. When 5.0 g CaCl2 is dissolved in enough water to make a 0.500 L solution, what is the molarity of ions in solution? 2. How many formula units are in 0.25 mole of Na2O? 3. How many nitrate ions are present in 0.200 mol of Zn(NO3)2?
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
A 29.3 mL sample of a 1.46 M potassium chloride solution is mixed with 14.6 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq) + Pb(NO3)2(aq) + PbCl2 (s) + 2KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.64 g. Determine the limiting reactant, the theoretical yield, and the percent yield. Part B Determine the theoretical yield of PbCl2. Express your answer in grams to three significant figures. ΑΣΦ...