Problems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following.

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1 Problems -- Chapter 1 1. Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following. (a) NaNO and HNO answers: see end of problem set (b) NaHCO 3 and H CO 3 (c) HClO and KClO (d) RbF and HF (e) KCl and HCl (f) H 3 PO and KH PO (g) (CH 3 ) NH NO 3 and (CH 3 ) NH. Write the appropriate equilibrium constant expressions (K a, etc.) for each of the the solutions above. 3. Determine the of a mixture of 0.0 M solutions of the two components in part (a) above (Ka =.5 x - ) Answer: = Calculate the of the following: (a) 0.35 M NaIO/0.0M HIO (Ka = 5.x -9 ) (b) 0. M NaIO/0.7 M HIO (Ka =.0x -11 ) (c) 0.0 M NH3 (Kb = 1.x -5 )/0.55 M NHCl. Answers: (a).9 (b).9 (c) HNO is a weak acid whose K a =.5x -. How many grams of NaNO would have to be added to 50 ml of a 0.M HNO acid solution to give a buffer of =.00. (3. g). A 0.5-gram sample of an unknown weak acid (call it HA for short) is dissolved in enough water to make 5.0 ml of solution. This weak acid solution is then titrated with 0.0 M NaOH and 5.0 ml of the NaOH solution is required to reach the equivalence point. Using a meter, the of the solution at the equivalence point is found to be.5. (a) Determine the molecular mass of the unknown acid g/mole (b) Determine the pk a value of the unknown acid The pk b value for ammonia (NH 3 ) is.7. Calculate the mass (in grams) of solid ammonium chloride (NH Cl, formula mass = 53.5 g/mole) that must be added to 300 ml of 0.5 M NH 3 solution to make a buffer solution with a equal to g. A 50 ml portion of a 0. M solution of a weak acid, HA, whose Ka equals 1.0 x -, is diluted to 50 ml and then titrated with 0. M NaOH. Calculate after the following ml of the NaOH solution have been added. (a) 0 (b) 5 (c) 5 (d) 50 (e) 0 (a).5 (b) 3.05 (c).00 (d).11 (e) Fifty ml of 0.1 M NH3 is titrated with 0. M HCl. The Kb of the weak base NH3 is 1. x -5. Calculate the after the following ml of the HCl solution have been added. (a) 0 (b) (c) 5 (d) 50 (e) 55 (a) ( b) 9. (c) 9. (d) 5. (e).3

2 . Shown on the next page is the titration curve for the titration of ml of a solution of the monoprotic acid, HA, with 0.01 M NaOH. What is the molarity of the acid? Is the acid a weak acid or a strong one? If it is a weak acid, what is the value of Ka? (0.0 M, weak, Ka=. x - ) Titration of ml of HA with 0.01M NaOH ml NaOH 11. Shown below is the titration curve for the titration of 50.0 ml of a solution of the weak ammoniatype base, methyl amine, CH3NH, with 0.01M HCl. What is the molarity of the base? What is the value of Kb for 1 methyl amine? (0.0 M answer given; K b = 3.x - ) ml 0.01M HCl 1. Consider reactions involving the following acids and bases. State in each case whether the at the equivalence point would be below 7, at 7, or above 7.

3 3 (a) acid = HClO base = KOH (b) acid = HNO3 base = NH3 (c) acid = HF base = LiOH (a) 7 (b) <7 (c) >7 13. A 3.0 ml sample of a 0.0 M HNO 3 solution was titrated with 0. M KOH. Calculate the after the following volumes of KOH have been added: (a) 0 ml (b).0 ml (c) 0.0 ml (30.0 ml (e) 0.0 ml ( f) 50.0 ml. (a) 0.0 (b) 0. (c) 1.07 d) 7.00 (e) 1.0 (f) Calculate the s of the following: (a) the solution formed by mixing 0.0 ml of a 0.30M HCl solution with 1 ml of a 0.5 M NaOH. (b) the solution formed by mixing 1.0 ml of a 0.M HC H 7 O solution with.0 ml of a 0.35M NaOH (K a for HC H 7 O =.0x 5 ) (c) the solution formed by mixing 15.0 ml of a 0.7M HF with 0.0 ml of a 0.0M KOH solution (K a for HF = 7.1x ) (d) the solution formed by mixing 30.0 ml of a 0.0 M HCHO solution with.0 ml of a 0.0 M KOH solution (K a for HCHO = 1.7x ) (e) the solution formed by dissolving.5 g of KF in ml of a 0.30 M HF solution (K a for HF = 7.1x ) (f) the end point of the titration of 5.0 ml of a 0. M HCHO with 0.0 M KOH. (a) 1.03 (b) 3.9 (c) 3.7 (d) 1.73 (e) 3. (f) A 0.0 ml sample of a 0.0 M HNO solution was titrated with 0.0 M KOH. Given that HNO is a weak acid whose K a =.5x -, calculate the after the following volumes of KOH have been added: (a) 0 ml; (b) 5.0 ml; (c).0 ml; (d) 0.0 ml; (e) 30.0 ml; (f) 0.0 ml (a) 1.7 (b).7 (c) 3.35 (d).39 (e) 13.0 (f) Drawn below is a plot of vs ml of 0.0 M NaOH for the titration of 50.0 ml of a weak diprotic acid. What is the concentration of the acid? What are the values of Ka1 and Ka for the acid? (Answer: 0.0M, Ka1 = 5.0x -3, Ka =.3x - ) ml 0.M NaOH 17. The Ksp of Pb(IO3) at 5 C = 3. x -13. What is the solubility of Pb(IO3) in moles per liter and in grams per liter? (.3 x -5 mol/l ; g/l = 0.0)

4 1. Calculate the Ksp of the following compounds. The solubilities are given in moles per liter. (a) Mg(OH) = 1.3 x - M (. x -1 ) (b) AgCO = 1. x - M (1.1 x -11 ) 19. Calculate the Ksp of the following salts. Solubilities are given in grams/liter. (a) BaCrO =.3 x - -3 g/l (.3 x -11 ) (b) CaF =.7 x - g/l (1.7 x - ) 0. What [SO - ] must be exceeded to produce a RaSO precipitate in 500 ml of a solution containing moles of Ra +? (Ksp = x -11 ). ( x -7 M) 1. A solution contains an Mg + concentration of mole/liter. Will Mg(OH) (Ksp =.9 x -1 ) precipitate if the OH - concentration of the solution is (a) -5 mole/liter? (b) - mole/liter? (a) Q = 1x -13, no (b) Q = 1x -11, yes]. How many grams of NaOH are required to start the precipitation of Mg(OH) in 0 ml of a solution which contains 0.1 g of MgCl? (1.1 x - g) 3. The value of Ksp for PbCl is 1. x -5. Will a precipitate of PbCl form when the following solutions are mixed? (a) 0 ml of 0.01 M Pb(NO3) and 0 ml of 0.00 M NaCl. (b) ml of 0.01 M Pb(NO3) and 30 ml of 0. M NaCl. (c) ml of 0.01 M Pb(NO3) and 0 ml of 0.0 M NaCl. (d) ml of 0.01 M Pb(NO3) and 0 ml of 0.0 M CaCl. (a) no, Q = 5x 9 (b) yes, Q= 5.x 5 (c) no, Q= 5.3x (d) yes, Q=.1x 5. Silver chromate, Ag CrO, is an "insoluble" substance with a K sp value of 1. x -1. Silver ion forms a stable complex ion with cyanide ion that has the formula Ag(CN) - and a formation constant (K f ) of 5.3 x 1. Calculate the molar solubility of Ag CrO in each of the following solutions. Write balanced chemical equations for any important equilibrium reactions that are occurring. (a) in water.9 x -5 M (b) in.00 M Na CrO 3.7 x -7 M (c).00 M NaCN 0.50 M 5. A saturated solution of Mg 3 (PO ) has a concentration of mg per liter. Calculate the solubility product constant for Mg 3 (PO )..7 x -. Cadmium carbonate, CdCO3, is a sparingly soluble salt whose Ksp=.5x -1. It is also known that Cd + forms the [Cd(NH3)] + complex ion that has a formation constant, Kf = 1.0x 7. (a) Calculate the molar solubility of CdCO3 in.0m NH3. (0.01 mol/l) (b) What NH3 concentration would be required to dissolve.00 mmol of CdCO3 in one liter of the solution? (.3 M)

5 5 Answers to #1 (a) HNO H + + NO - (b) H CO 3 HCO H + (c) HClO H + + ClO - (d) HF F - + H + (e) not a buffer: the only equilibrium in this neutral solutions is dissociation of water, i.e., H O H + + OH - (f) H 3 PO H + + H PO - (g) (CH 3 ) NH + H + + (CH 3 ) NH

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