Chemistry homework questions
tenuised
chem.docxCalculate the pH after 0.017 mole of HCl is added to 1.00 L of each of the four solutions. (Assume that all solutions are at 25°C.)
(a) 0.133 M acetic acid (HC2H3O2, Ka = 1.8 ✕ 10−5) (b) 0.133 M sodium acetate (NaC2H3O2) (c) pure H2O (d) 0.133 M HC2H3O2 and 0.133 M NaC2H3O2
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25°C.)
(a) pH = 5.16 (b) pH = 5.53 (c) pH = 4.74 (d) pH = 4.93
Consider the titration of 41.5 mL of 0.198 M HCl with 0.124 M NaOH. Calculate the pH of the resulting solution after the following volumes of NaOH have been added. (Assume that all solutions are at 25°C.)
(a) 0.0 mL (b) 10.0 mL (c) 40.0 mL (d) 80.0 mL (e) 100.0 mL
Consider the titration of 100.0 mL of 0.240 M benzoic acid (Ka = 6.4 ✕ 10−5) with 0.120 M KOH. Calculate the pH of the resulting solution after each of the following volumes of KOH has been added. (Assume that all solutions are at 25°C.)
(a) 0.0 mL (b) 50.0 mL (c) 100.0 mL (d) 150.0 mL (e) 200.0 mL (f) 250.0 mL
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (Assume that the temperature is 25°C.)
(a) 101.1 mL of 0.17 M HF (Ka= 7.2 ✕ 10−4) titrated with 0.17 M KOH
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(b) 100.7 mL of 0.15 M C2H5NH2 (Kb = 5.6 ✕ 10−4) titrated with 0.30 M HNO3
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(c) 100.9 mL of 0.51 M HCl titrated with 0.26 M KOH
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Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties.
(a) Ca3(PO4)2, Ksp = 1.3 ✕ 10−32 mol/L (b) MgF2, Ksp = 6.4 ✕ 10−9 mol/L (c) AgBr, Ksp = 5.0 ✕ 10−13 mol/L
The Ksp for silver chromate (Ag2CrO4) is 9.0 ✕ 10−12. Calculate the solubility of silver chromate in each of the following.
(a) water mol/L (b) 0.15 M AgNO3 mol/L (c) 0.34 M Na2CrO4 mol/L
Use the following data to calculate the Ksp value for each solid.
(a) The solubility of MnCO3 is 1.1 ✕ 10−3 g/L. (b) The solubility of Al(OH)3 is 5.5 ✕ 10−9 mol/L.
The concentration of Ba2+ in a solution saturated with BaF2(s) is 1.82 ✕ 10−2 M. Calculate Ksp for BaF2.
Calculate the solubility (in mol/L) of Co(OH)3 (Ksp = 3 ✕ 10−43) in each of the following. (Assume that all solutions are at 25°C.)
