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) 1. What is the ratio of the Pb²+ to Br- concentrations (i.e., Pb²+ : Br¯) present after mixing the two solutions but before the ions start reacting? a) 1.00 : 3.54 b) 1.00 : 2.00 c) 3.73 : 1.00 d) 1.06 : 1.00 2. What is the maximum mass of product that could be isolated by filtration after the reaction occurs? a) 0.513 g b) 0.908 g c) 1.10 g d) 3.21 g At the end of the reaction, what is the concentration (in molarity) of nitrate ions in the solution? Note: there are other ions present too, but you are only asked to think about the NO3 ions here. 3. a) 0.00773 mol·L-1 b) 0.00495 mol·L-1 c) 0.0300 mol·L·1 d) 0.0155 mol·L-1

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) 1. What is the ratio of the Pb²+ to Br- concentrations (i.e., Pb²+ : Br¯) present after mixing the two solutions but before the ions start reacting? a) 1.00 : 3.54 b) 1.00 : 2.00 c) 3.73 : 1.00 d) 1.06 : 1.00 2. What is the maximum mass of product that could be isolated by filtration after the reaction occurs? a) 0.513 g b) 0.908 g c) 1.10 g d) 3.21 g At the end of the reaction, what is the concentration (in molarity) of nitrate ions in the solution? Note: there are other ions present too, but you are only asked to think about the NO3 ions here. 3. a) 0.00773 mol·L-1 b) 0.00495 mol·L-1 c) 0.0300 mol·L·1 d) 0.0155 mol·L-1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

45.02 mL of a saturated solution of iron (III) hydroxide are titrated with 0.253 M HCl. If 3.36 mL of the acid are required, what is Ksp for iron (III) hydroxide? Iron (III) hydroxide reacts with HCl according to the following balanced equation: Fe(OH)3(aq) + 3HCl(aq) → FeCl3(aq) + 3H2O(l)
Some wastewater stream contains 0.015 M Hg22+. Some chemical engineer decides to remove it by precipitating it as Hg2CO3(s). He mixes 100.00 ml of the wasterwater with 100.00 ml of a 2.00 M solution of Na2CO3 and filters the result to remove the solid. How much residual Hg22+ should he expect to find still in the water? (Hint: it should not be 0) Ksp of. Hg2CO3 = 9.0 x 10-15. Also keep in mind that Hg+ is the only ion that exists in solutions as a dimer, i.e. Hg22+, not 2 Hg+ (Hg2CO3→ Hg22+ + CO32-)
You have a solution that is either CuCl2 (aq) or Cu(NO3)2 (aq). You add some KOH (aq) and a solid precipitate is formed. Does this test allow you to determine the contents of your solution? If so, how? If not, what other test could you perform that would give you the information that you need? Please explain.
In one experiment, an 80.0-mL sample of hydrocyanic cid (HCN) was titrated with 20.0 mL of triiodide (I3-) in the reaction: HCN (aq) + I3- (aq) --> ICN (aq) + 2 I- (aq) + H+ (aq) 40.0 mL of the same triiodide solution were required to titrate 0.200 mol of H3AsO3 (aq) in the reaction: H3AsO3 (aq) + I3- (aq) + H2O (l) --> H3AsO4 (aq) + 3 I- (aq) + 2H+ (aq) What is the molar concentration of HCN (aq)? (Answer in sig figs)
Copper(I) ions in aqueous solution react with NH3(aq) according to Cu+(aq)+2NH3(aq)⟶Cu(NH3)+2(aq) ?f=6.3×10^10 Calculate the solubility (in g·L−1) of CuBr(s) (?sp=6.3×10^−9) in 0.47 M NH3(aq). solubility of CuBr(s): g/L
Consider the reaction: Ag* (aq) + Cl(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag* ions from 2.900 x 102 mL of a 0.0115 M AgNO3 solution? The molar mass of NaCl is 58.44 g/ mol. Tap here or pull up for additional resources
Calculate the maximum solubility of calcium fluoride, CaF2 in g/L when in the presence of 0.077 M Ca(NO3)2. The solubility product of CaF2 is 4.2x1011 and CaF2 has a molar mass of 78.08 g/mol. Express your answer to the correct number of significant figures, in scientific notation and include the unit with your answer.
A student is given 1.4571 g of pure CuO. To recover the Cu present in the compound, the dark powdery solid was dissolved in 15.0 mL of 6 M HCl and the solution was diluted to 50.0 mL with water. How many grams of Mg is needed to displace all of the copper (II) ions from the solution? Mg(s) + Cu2+(aq) --> Cu(s) + Mg2+(aq)
2. Each of the following salts can be prepared from an acid and a base. Write the balanced molecular equation and the net ionic equation for the preparation of each. Indicate states of the reactants and products [(aq), (s), (1)]. Review solubility rules if necessary to determine the solubility of the reactants. (c) Al(NO3)3 (aq) (a) BaCl₂ (aq) (b) CsCH3CO₂ (aq)
Solid potassium hydroxide is slowly added to 150 mL of a 0.0538 M iron(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is M.
When 50.0 mL of a 0.3000 M AgNO3 solution is added to (4.65x10^1) mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of (1.2x10^-1) g. what was the concentration in molarity of chloride ions in the original MgCl₂ solution? 2AgNO3(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO3)2(aq) Use the correct number of significant figures and type in the unit abbreviation for the answer. Answer: 8.0x10^-1 M.
Part 1 Solution A is a 5.0 L aqueous sodium iodide (Nal) solution, and I want to determine the concentration of iodide ions, I- (aq). I'm going to do this with a precipitation titration, taking advantage of the insolubility of Agl (s). To a 20.0 mL sample of Solution A, I add 0.0740 M AgNO3 aqueous solution until adding AgNO3 no longer causes more precipitate to form. I see no more visible precipitate after adding 6.00 mL of AgNO3 solution. Based on this information, what is the concentration (in mM) of iodide anions in Solution A? Part 2 mM I It's hard to precisely measure the endpoint for a precipitation titration. Let's suppose that instead of measuring the volume of AgNO3 solution added, I just measure the weight of precipitate from the above experiment. I determine that the precipitate weighs 93.9 mg. Based on the weight of the solid precipitate, what is the concentration (in mM) of iodide anions in Solution A? mM I